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Ionic Reactions and Tests - Practice Questions (30)

Question 1: 1. At room temperature, the following groups of ions must be able to coexist in large quantities in ...

1. At room temperature, the following groups of ions must be able to coexist in large quantities in aqueous solution is

  • A. A. $\mathrm { Na } ^ { + } , \mathrm { NH } _ { 4 } ^ { + } , \mathrm { I } ^ { - } , \mathrm { ClO } ^ { - }$
  • B. B. $\mathrm { Ba } ^ { 2 + } , \mathrm { H } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { CH } _ { 3 } \mathrm { COOO } ^ { - }$
  • C. C. $\mathrm { K } ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { Cl } ^ { - } , \mathrm { NO } _ { 3 } ^ { - }$
  • D. D. $\mathrm { Cu } ^ { 2 + } , \mathrm { Ag } ^ { + } , \mathrm { OH } ^ { - } , \mathrm { Br } ^ { - }$

Answer: C

Solution: A. I and $\mathrm { ClO } ^ { - }$ undergo a redox reaction, and they cannot coexist in large amounts; B. $\mathrm { H } ^ { + }$ and $\mathrm { CH } _ { 3 } \mathrm { COO } ^ { - }$ react to form $\mathrm { CH } _ { 3 } \mathrm { COOH }$, which cannot coexist in large amounts; INLINE_FORMULA_3]] cannot coexist in large quantities, B is incorrect; $\mathrm { C } . \mathrm { K } ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { Cl } ^ { - } , \mathrm { NO } _ { 3 } ^ { - }$ can coexist in large quantities, C is correct; D. $\mathrm { OH } ^ { - }$ reacts with $\mathrm { Ag } ^ { + } , \mathrm { Cu } ^ { 2 + }$ to form a hydroxide precipitate, and silver ions react with bromine ions to form a silver bromide precipitate, which cannot coexist in large amounts; The answer is C.

Question 2: 2. At room temperature, the following groups of ions can coexist in large amounts

2. At room temperature, the following groups of ions can coexist in large amounts

  • A. A. $\mathrm { Cu } ^ { 2 + } , \mathrm { Ca } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { Cl } ^ { - }$
  • B. B. $\mathrm { K } ^ { + } , \mathrm { NH } _ { 4 } ^ { + } , \mathrm { CO } _ { 3 } ^ { 2 - } , \mathrm { OH } ^ { - }$
  • C. C. $\mathrm { Na } ^ { + } , \mathrm { Ba } ^ { 2 + } , \mathrm { SO } _ { 3 } ^ { 2 - } , \mathrm { I } ^ { - }$
  • D. D. $\mathrm { H } ^ { + } , \mathrm { Fe } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { ClO } ^ { - }$

Answer: A

Solution: A. The four ions do not react with each other and can coexist in large quantities; B. Hydroxide and ammonium will combine to form the weak electrolyte ammonia monohydrate, which cannot coexist in large quantities, so B does not meet the meaning of the question; C. Sulfite and barium ions will combine to form a precipitate, which cannot coexist in large quantities, so C does not meet the meaning of the question; D. In an acidic environment, hypochlorite and nitrate will oxidize ferrous ions, which cannot coexist in large quantities, so D does not meet the meaning of the question; D. In an acidic environment, hypochlorite and nitrate will oxidize ferrous ions.

Question 3: 5. A solution contains only $\mathrm { K } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { NO } _ { 3...

5. A solution contains only $\mathrm { K } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { SO } _ { 4 } ^ { 2 - }$ four ions, and the ratio of the number of the first three ions to the number of $3 : 2 : 1$ is known, then the ratio of the number of ions of $\mathrm { K } ^ { + }$ and $\mathrm { SO } _ { 4 } ^ { 2 - }$ in the solution is

  • A. A. $1 : 1$
  • B. B. 2:3
  • C. C. 3:4
  • D. D. 5:2

Answer: A

Solution: Since the solution is not electrically charged, the total number of positive charges carried by the cations is equal to the total number of negative charges carried by the anions; $\mathrm { K } ^ { + }$, $\mathrm { Mg } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - }$ the ratio of the numbers of the three ions is $3 : 2 : 1$, and it is assumed that the numbers of the three ions of $\mathrm { K } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - }$ are respectively 3, $2 , 1$, and let the number of ions in $\mathrm { SO } _ { 4 } ^ { 2 - }$ be $x$, then there are $3 + 2 \times 2 = 1 \times 1 + 2 x$, and $x = 3$, and $\mathrm { K } ^ { + }$. FORMULA_9]] and $\mathrm { SO } _ { 4 } ^ { 2 - }$ have $3 : 3 = 1 : 1$, A is correct.

Question 4: 6. The following reactions are both redox reactions and ionic reactions

6. The following reactions are both redox reactions and ionic reactions

  • A. A. You can achieve your aim if you try hard without giving up.
  • B. B. Aluminum hydroxide for hyperacidity
  • C. C. Sodium metal in water
  • D. D. Combustion of fuels

Answer: C

Solution: A. water droplets, calcium carbonate, water and carbon dioxide reaction to generate calcium bicarbonate, carried out in solution, there are ions generated, belong to the ionic reaction, before and after the reaction, there is no change in valence, not a redox reaction, A error; B. Aluminum hydroxide treatment of hyperacidity, acid-base neutralization reaction, there are ions in the solution to participate in the reaction, belonging to the ionic reaction, there is no valence change before and after the reaction, not a redox reaction, B error; C. Sodium metal into the water, the generation of sodium hydroxide and hydrogen gas, reaction in solution, there are ions generated, belongs to the ionic reaction, before and after the reaction there is a change in valence, belongs to the redox reaction, C is correct; D. The combustion of fuel, no ions involved in the reaction process, is not an ionic reaction, there is oxygen to participate, belongs to the redox reaction, D error; Therefore, the answer is: C. ## 7. B Knowledge points] four basic types of reactions, ionic reactions occurring conditions A. Sodium chloride and silver nitrate react to form silver chloride and sodium nitrate, which is a complex decomposition reaction, A is correct; B. After the reaction, the solution is sodium nitrate solution, the particles present are sodium ions and nitrate ions, and water molecules and hydrogen ions and hydroxide ions, B error; C. The essence of the reaction is that silver ions and chloride ions combine to form silver chloride, C is correct; D. The essence of the reaction between silver nitrate and barium chloride is also the combination of silver ions and chloride ions, which is the same as the reaction, and D is correct.

Question 5: 7. As shown in the figure is silver nitrate solution and sodium chloride solution just completely re...

7. As shown in the figure is silver nitrate solution and sodium chloride solution just completely reacted microscopic schematic, the conclusion drawn from the error is that ![](/images/questions/ionic-reactions/image-001.jpg)

  • A. A. The reaction is a complex decomposition reaction
  • B. B. The only particles present in the solution after the reaction are $\mathrm { NO } ^ { 3 }$ and $\mathrm { Na } ^ { + }$
  • C. C. The essence of this reaction is that $\mathrm { Ag } ^ { + }$ and $\mathrm { Cl } ^ { - }$ combine to form AgCl
  • D. D. The substance of the reaction between silver nitrate solution and barium chloride solution is the same as this reaction

Answer: B

Solution:

Question 6: 8. The following statements are correct

8. The following statements are correct

  • A. A. Ionization of electrolytes requires not only an aqueous or molten state, but also an electrically charged
  • B. B. Melting is an absorptive process and dissolving is exothermic.
  • C. C. Substances composed of the same element are pure substances
  • D. D. Reactions of electrolytes in solution are essentially reactions between ions

Answer: D

Solution: A. Electrolyte is dissolved in water or in the molten state can conduct electricity compounds, do not need to be energized, so A error; B. Material melting is a heat-absorbing process, the dissolution process is accompanied by energy changes, such as the dissolution of sodium hydroxide solids, exothermic, such as ammonium nitrate, dissolution of heat absorption, so B error; C. by the same elements of the substance is not necessarily pure, such as oxygen and ozone composition of the mixture, so C error; D. The reaction of electrolytes in solution is essentially a reaction between ions, so D is correct;

Question 7: 9. All of the ions in the following ion groups can co-exist in large amounts

9. All of the ions in the following ion groups can co-exist in large amounts

  • A. A. $\mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Cl } ^ { - } , \mathrm { CO } _ { 3 } ^ { 2 - }$
  • B. B. $\mathrm { Na } ^ { + } , \mathrm { K } ^ { + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { SO } _ { 4 } ^ { 2 - }$
  • C. C. $\mathrm { Ca } ^ { 2 + } , \mathrm { NH } _ { 4 } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { SO } _ { 4 } ^ { 2 - }$
  • D. D. $\mathrm { Na } ^ { + } , \mathrm { Fe } ^ { 3 + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { I } ^ { - }$

Answer: B

Solution: A. Magnesium ions and carbonate ions combine to form a magnesium carbonate precipitate that cannot coexist in large quantities, A is wrong; B. The four ions can coexist in large quantities without reacting with each other, B is correct; C.Calcium ions and sulfate ions combine to form calcium sulfate microsolutes that cannot coexist in large quantities, C is wrong; D. Trivalent iron ions and iodide ions cannot coexist in large quantities by redox, D is wrong;

Question 8: 10. catalytic conditions so that the decomposition of water to produce hydrogen is one of the effect...

10. catalytic conditions so that the decomposition of water to produce hydrogen is one of the effective ways to obtain clean energy hydrogen, and the preparation of the catalyst is the key, Tongji University, Prof. Wen Ming's group has prepared an ultrathin structure of the catalyst CoFePS. the following statement is correct

  • A. A. The decomposition of water is an ionic reaction
  • B. B. CoFePS is a mixture of four monomers
  • C. C. Before and after the reaction, the mass and chemical properties of the catalyst CoFePS remain unchanged
  • D. D. The mass of ${ } ^ { 1 \mathrm {~m} ^ { 3 } \mathrm { H } _ { 2 } }$ produced by water decomposition is

Answer: C

Solution: A. The decomposition of water is not a reaction in which ions are involved, and it is not an ionic reaction, A. Wrong; B. CoFePS is a compound of four elements; C. The mass and chemical properties of the catalyst remain unchanged before and after the reaction, C is correct; D. There is no standardized condition to calculate the amount of hydrogen and determine its mass, D error;

Question 9: 11. The following ionization equation is written correctly

11. The following ionization equation is written correctly

  • A. A. $\mathrm { NaOH } = \mathrm { Na } ^ { + } + \mathrm { O } ^ { 2 - } + \mathrm { H } ^ { + }$
  • B. B. $\mathrm { FeCl } _ { 3 } = \mathrm { Fe } ^ { 3 + } + \mathrm { Cl } _ { 2 }$
  • C. C. $\mathrm { Ca } \left( \mathrm { NO } _ { 3 } \right) _ { 2 } = \mathrm { Ca } ^ { 2 + } + 2 \left( \mathrm { NO } _ { 3 } \right) ^ { 2 - }$
  • D. D. $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 } = 2 \mathrm { H } ^ { + } + \mathrm { SO } ^ { 4 }$

Answer: D

Solution: A. The ionization equation of NaOH is $\mathrm { NaOH } = \mathrm { Na } ^ { + } + \mathrm { OH } ^ { - }$, A is wrong; B. The ionization equation of $\mathrm { FeCl } _ { 3 }$ is $\mathrm { FeCl } _ { 3 } = \mathrm { Fe } ^ { 3 + } + 3 \mathrm { Cl } ^ { - } , \mathrm { B }$; C. The ionization equation of $\mathrm { Ca } \left( \mathrm { NO } _ { 3 } \right) _ { 2 }$ is: $\mathrm { Ca } \left( \mathrm { NO } _ { 3 } \right) _ { 2 } = \mathrm { Ca } ^ { 2 + } + 2 ^ { \mathrm { NO } _ { 3 } ^ { - } }$, C is wrong; D. The ionization equation of $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$ is $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 } = 2 \mathrm { H } ^ { + } + \mathrm { SO } ^ { 2 - }$, D is correct; Therefore, the answer is D.

Question 10: 12. The reaction represented by the ionic equation $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } =...

12. The reaction represented by the ionic equation $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O }$ can be

  • A. A. Neutralization reactions between all acids and bases
  • B. B. Reaction between sodium bicarbonate and sodium hydroxide
  • C. C. Reactions of all soluble acids and soluble bases
  • D. D. Reaction of dilute hydrochloric acid with barium hydroxide

Answer: D

Solution: A. Weak acids and bases can't be written as ions, so $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O }$ can't represent the neutralization reaction between all acids and bases, and A doesn't fit the question; B. The ionic equation for the reaction between sodium bicarbonate and sodium hydroxide is $\mathrm { HCO } ^ { 3 } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O } + \mathrm { CO } ^ { 2 - }$; C. Soluble acids and soluble bases may also react to form precipitates, such as the reaction between sulfuric acid and barium hydroxide, which cannot be expressed by $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O }$; D. Dilute hydrochloric acid reacts with barium hydroxide to form barium chloride and water, and the ionic equation is $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O } , \mathrm { D }$.

Question 11: 13. For the following groups of substances, no reaction can occur

13. For the following groups of substances, no reaction can occur

  • A. A. $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ Solution and hydrochloric acid
  • B. B. Fe and ${ } ^ { \mathrm { CuSO } _ { 4 } }$ solutions
  • C. C. $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ solution and KCl solution
  • D. D. $\mathrm { Na } _ { 2 } \mathrm { SO } _ { 4 }$ solution and $\mathrm { BaCl } _ { 2 }$ solution

Answer: C

Solution: A. A small amount of hydrochloric acid reacts $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 } + \mathrm { HCl } = \mathrm { NaHCO } _ { 3 } + \mathrm { NaCl }$ and a sufficient amount of hydrochloric acid reacts $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 } + 2 \mathrm { HCl } = \mathrm { H } _ { 2 } \mathrm { O } + \mathrm { CO } _ { 2 } \uparrow + 2 \mathrm { NaCl }$, A does not fit the question; B. Fe reacts with $\mathrm { CuSO } _ { 4 }$ solution $\mathrm { Fe } + \mathrm { CuSO } _ { 4 } = \mathrm { FeSO } _ { 4 } + \mathrm { Cu }$; C. $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ solution and KCl solution do not form insoluble substances, gases, weak electrolytes, or chemical reactions; D. $\mathrm { Na } _ { 2 } \mathrm { SO } _ { 4 }$ solution and $\mathrm { BaCl } _ { 2 }$ solution react $\mathrm { Na } _ { 2 } \mathrm { SO } _ { 4 } + \mathrm { BaCl } _ { 2 } = \mathrm { BaSO } _ { 4 } \downarrow + 2 \mathrm { NaCl }$, D does not meet the meaning of the question; Therefore, the answer is C.

Question 12: 14. The following groups of two substances in solution, the reaction can be expressed by the same io...

14. The following groups of two substances in solution, the reaction can be expressed by the same ionic equation is

  • A. A. Sodium hydroxide and hydrochloric acid; sodium hydroxide and carbonic acid
  • B. B. $\mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$ reacts with sulfuric acid; $\mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$ with hydrochloric acid
  • C. C. $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ solution with nitric acid solution; $\mathrm { CaCO } _ { 3 }$ solution with nitric acid solution
  • D. D. $\mathrm { BaCl } _ { 2 }$ solution with $\mathrm { Na } _ { 2 } \mathrm { SO } _ { 4 }$ solution; $\mathrm { Ba } ( \mathrm { OH } ) _ { 2 }$ solution with $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$ solution

Answer: B

Solution: A. Hydrochloric acid is strongly acidic and is completely ionized in solution, while carbonic acid is a weak dibasic acid and is partially ionized in solution, so acetic acid retains its molecular form when writing ionic equations, and the ionic equations for the two reactions with sodium hydroxide are different, so A does not match; B. $\mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$ reacts with sulfuric acid and $\mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$ reacts with hydrochloric acid with the same ionic equation, both of which are met by $\mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } + 6 \mathrm { H } ^ { + } = 2 \mathrm { Al } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \mathrm { O } , ~ \mathrm {~B}$; C. $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ is a labile salt and calcium carbonate is a refractory salt, so when writing the ionic equations, calcium carbonate should retain its chemical form, and the ionic equations for the two are different from those for the nitric acid solution, so C does not match; D. $\mathrm { BaCl } _ { 2 }$ solution reacts with $\mathrm { Na } _ { 2 } \mathrm { SO } _ { 4 }$ solution to form barium sulfate and sodium chloride, and $\mathrm { Ba } ( \mathrm { OH } ) _ { 2 }$ solution reacts with $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$ solution to form barium sulfate and water, the ionic equations are different, and D does not match; The answer is B.

Question 13: 15. The following experimental operations will achieve the desired purpose or will lead to the appro...

15. The following experimental operations will achieve the desired purpose or will lead to the appropriate conclusion. | Select <br> Item | Experimental Procedure | Expected Purpose or Conclusion | :--- | :--- | :--- | :--- | :--- | :--- | :--- | | A | Hydrochloric acid is added dropwise to a colorless solution and odorless bubbles are produced | There must be <br> $\mathrm { CO } _ { 3 } ^ { 2 - }$ | in the solution. | B | pass a gas mixture containing $\mathrm { CO } _ { 2 }$ and a small amount of HCl slowly through a saturated $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$ solution | remove the HCl from ${ } ^ { \mathrm { CO } _ { 2 } }$ | C | add a drop of hydrochloric acid to a clean solution. C | dip a clean platinum wire into solution Z and then cauterize it in an alcohol flame and observe | determine whether Z is a sodium salt | D | test the solution on a clean platinum wire wrapped in [INLINE_FORMULA_2]. | D | Put a few drops of water on a cotton wool wrapped in sodium peroxide and the cotton wool burns | $\mathrm { Na } _ { 2 } \mathrm { O } _ { 2 }$ reacts with water and emits heat | | [INLINE_FORMULA_3]] is a sodium salt.

  • A. A. A
  • B. B. B
  • C. C. C
  • D. D. D

Answer: D

Solution: A. $\mathrm { HCO } _ { 3 } ^ { - }$ can also produce bubbles when it meets hydrochloric acid; B. $\mathrm { CO } _ { 2 } , \mathrm { HCl }$ can react with $\mathrm { Na } _ { 2 } \mathrm { CO } _ { 3 }$; C.Sodium salts have the same flame color as NaOH, so it is not possible to determine whether Z is a sodium salt; D. $\mathrm { Na } _ { 2 } \mathrm { O } _ { 2 }$ reacts with water and releases heat, causing the cotton wool to burn;

Question 14: 18. In the following processes, a clear reaction phenomenon can be observed ( )

18. In the following processes, a clear reaction phenomenon can be observed ( )

  • A. A. Add NaOH solution dropwise to dilute hydrochloric acid.
  • B. B. Add a small amount of $\mathrm { CO } _ { 2 }$ dropwise to the $\mathrm { CaCl } _ { 2 }$ solution.
  • C. C. Add NaCl solution dropwise to $\mathrm { NaHCO } _ { 3 }$ solution.
  • D. D. Add a small amount of $\mathrm { H } _ { 2 } \mathrm { O } _ { 2 }$ dropwise to $\mathrm { FeCl } _ { 2 }$ solution, then add KSCN solution dropwise.

Answer: D

Solution: A. Hydrochloric acid and sodium hydroxide solution are colorless and react to form sodium chloride and water, this reaction has no phenomenon, A error; B.Calcium chloride solution and carbon dioxide do not react and there is no phenomenon; C. $\mathrm { NaHCO } _ { 3 }$ solution and NaCl solution do not react, no phenomenon, C error; D. $\mathrm { H } _ { 2 } \mathrm { O } _ { 2 }$ oxidizes $\mathrm { Fe } ^ { 2 + }$ into $\mathrm { Fe } ^ { 3 + }$, and the solution turns red when KSCN is added;

Question 15: 19. Graphical representations of the relationships between different types of reactions are often us...

19. Graphical representations of the relationships between different types of reactions are often used. For example, decomposition and redox reactions can be represented in Figure 1. Figure 2 shows the relationship between ionic reactions, redox reactions and replacement reactions. ![](/images/questions/ionic-reactions/image-002.jpg) Figure 1 ![](/images/questions/ionic-reactions/image-003.jpg) Figure 2

  • A. A. ionic reaction
  • B. B. redox reaction
  • C. C. displacement reaction (chemistry)
  • D. D. All three.

Answer: C

Solution: There must be a change of elemental valence in the replacement reaction, it must be a redox reaction, redox reaction and replacement reaction is a containment relationship, some replacement reactions carried out in aqueous solution are ionic reactions, ionic reaction and replacement reaction is a cross-relationship, some ionic reactions do not have a change of elemental valence, it is not a redox reaction, ionic reaction and redox reaction is a cross-relationship, then A is a redox reaction, B is a replacement reaction and C is an ionic reaction.

Question 16: 20 . The following ionic reaction equation is correct ()

20 . The following ionic reaction equation is correct ()

  • A. A. Reaction of calcium carbonate with acetic acid: $\mathrm { CaCO } _ { 3 } + 2 \mathrm { H } ^ { + } \rightarrow \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$
  • B. B. Chlorine gas in ferrous chloride solution: $2 \mathrm { Fe } ^ { 2 + } + \mathrm { Cl } _ { 2 } \rightarrow 2 \mathrm { Fe } ^ { 3 + } + 2 \mathrm { Cl } ^ { - }$
  • C. C. Reaction of iron with dilute sulfuric acid: $2 \mathrm { Fe } + 6 \mathrm { H } ^ { + } \rightarrow 2 \mathrm { Fe } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \uparrow$
  • D. D. Mixing of copper sulfate and barium hydroxide solution: $\mathrm { Ba } ^ { 2 + } + \mathrm { SO } _ { 4 } ^ { 2 - } - \rightarrow \mathrm { BaSO } _ { 4 } \downarrow$

Answer: B

Solution: A. Acetic acid is a weak acid and can only be written as a chemical formula, so calcium carbonate and acetic acid react to form calcium acetate, carbon dioxide, and water: $\mathrm { CaCO } _ { 3 } + 2 \mathrm { CH } _ { 3 } \mathrm { COOH } \rightarrow \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O } + 2 \mathrm { CH } _ { 3 } \mathrm { COO } ^ { - }$, A is incorrect ; B. Chlorine gas is passed into a ferrous chloride solution and reacts to form iron ions and chloride ions: $2 \mathrm { Fe } ^ { 2 + } + \mathrm { Cl } _ { 2 } \rightarrow 2 \mathrm { Fe } ^ { 3 + } + 2 \mathrm { Cl } ^ { - }$, so B is correct; C. Iron and dilute sulfuric acid react with ferrous sulfate and hydrogen: $\mathrm { Fe } + 2 \mathrm { H } ^ { + } \rightarrow \mathrm { Fe } ^ { 2 + } + \mathrm { H } _ { 2 } \uparrow$, so C is wrong; D. Copper sulfate and barium hydroxide solution mix to form barium sulfate and copper hydroxide precipitate: $\mathrm { Ba } ^ { 2 + } + \mathrm { SO } _ { 4 } ^ { 2 - } + \mathrm { Cu } ^ { 2 + } + 2 \mathrm { OH } ^ { - } - \rightarrow \mathrm { BaSO } _ { 4 } \downarrow + \mathrm { Cu } ( \mathrm { OH } ) _ { 2 } \downarrow$, so D is wrong. In summary, the answer is B.

Question 17: 21. The following ionic equations are written correctly ()

21. The following ionic equations are written correctly ()

  • A. A. Dissolving eggshells in acetic acid: $2 \mathrm { H } ^ { + } + \mathrm { CO } _ { 3 } ^ { 2 - } = \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$
  • B. B. Adding an aluminum sheet to a caustic soda solution : $2 \mathrm { Al } + 2 \mathrm { OH } - + 2 \mathrm { H } _ { 2 } \mathrm { O } = 2 ^ { \mathrm { AlO } _ { 2 } ^ { - } } + 3 \mathrm { H } _ { 2 } \uparrow$
  • C. C. Reaction of iron with hydrochloric acid: $2 \mathrm { Fe } + 6 \mathrm { H } ^ { + } = 2 \mathrm { Fe } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \uparrow$
  • D. D. Reaction of dilute sulfuric acid and ammonia: $\mathrm { H } ^ { + } + \mathrm { OH } - = \mathrm { H } _ { 2 } \mathrm { O }$

Answer: B

Solution: A. Acetic acid dissolves eggshells: $2 \mathrm { CH } _ { 3 } \mathrm { COOH } + \mathrm { CaCO } _ { 3 } = \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O } + \mathrm { Ca } ^ { 2 + } + 2 \mathrm { CH } _ { 3 } \mathrm { COO } -$ , so A is wrong; B.An aluminum sheet is added to a caustic soda solution to produce hydrogen gas: $2 \mathrm { Al } + 2 \mathrm { OH } - + 2 \mathrm { H } _ { 2 } \mathrm { O } = 2 ^ { \mathrm { AlO } _ { 2 } ^ { - } } + 3 \mathrm { H } _ { 2 } \uparrow$ , so B is correct ; C. Iron reacts with hydrochloric acid: $\mathrm { Fe } + 2 \mathrm { H } ^ { + } = \mathrm { Fe } ^ { 2 + } + \mathrm { H } _ { 2 } \uparrow$, so C is wrong; D. Dilute sulfuric acid reacts with ammonia: $\mathrm { H } ^ { + } + \mathrm { NH } _ { 3 } \cdot \mathrm { H } _ { 2 } \mathrm { O } = \mathrm { H } _ { 2 } \mathrm { O } + \mathrm { NH } _ { 4 } ^ { + }$, so D is wrong. In summary, the answer is B.

Question 18: 23. The following ionic equations are written correctly ()

23. The following ionic equations are written correctly ()

  • A. A. Reaction of copper with silver nitrate solution: $\mathrm { Cu } + \mathrm { Ag } ^ { + } = \mathrm { Cu } ^ { 2 + } + \mathrm { Ag }$
  • B. B. Reaction of calcium carbonate with dilute hydrochloric acid: $\mathrm { CaCO } _ { 3 } + 2 \mathrm { H } ^ { + } = \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$
  • C. C. Reaction of iron with dilute sulfuric acid: $2 \mathrm { Fe } + 6 \mathrm { H } ^ { + } = 2 \mathrm { Fe } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \uparrow$
  • D. D. Reaction of magnesium sulfate solution with barium hydroxide solution: $\mathrm { Mg } ^ { 2 + } + 2 \mathrm { OH } ^ { - } = \mathrm { Mg } ( \mathrm { OH } ) _ { 2 } \downarrow$

Answer: B

Solution: A. Copper and silver nitrate undergo a substitution reaction to form silver and copper nitrate, and the ionic equation is: $\mathrm { Cu } + 2 \mathrm { Ag } ^ { + } = \mathrm { Cu } ^ { 2 + }$ + 2 Ag, so A is wrong; B. Calcium carbonate reacts with dilute hydrochloric acid to form calcium chloride, carbon dioxide and water; the ionic equation is $\mathrm { CaCO } _ { 3 } + 2 \mathrm { H } ^ { + } = \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$, so B is correct; C. Iron and dilute sulfuric acid react to form $\mathrm { Fe } ^ { 2 + }$, the ionic equation is: $\mathrm { Fe } + 2 \mathrm { H } ^ { + } = \mathrm { Fe } ^ { 2 + } + \mathrm { H } _ { 2 } \uparrow$, so C is wrong; D. Magnesium sulfate solution reacts with barium hydroxide solution to form barium sulfate and magnesium hydroxide precipitate, the ionic equation is: $\mathrm { SO } _ { 4 } ^ { 2 - }$ $+ \mathrm { Ba } ^ { 2 + } + \mathrm { Mg } ^ { 2 + } + 2 \mathrm { OH } ^ { - } = \mathrm { Mg } ( \mathrm { OH } ) _ { 2 } \downarrow + \mathrm { BaSO } _ { 4 } \downarrow$, so D is wrong; The answer is B.

Question 19: 25. The ions that may also coexist in large amounts in a solution containing a large amount of $\mat...

25. The ions that may also coexist in large amounts in a solution containing a large amount of $\mathrm { Ba } ^ { 2 + } , \mathrm { H } ^ { + } , \mathrm { NO } _ { 3 }$ are ( )

  • A. A. $\mathrm { SO } _ { 4 } { } ^ { 2 - }$
  • B. B. $\mathrm { Fe } ^ { 2 + }$
  • C. C. $\mathrm { HCO } _ { 3 } { } ^ { - }$
  • D. D. $\mathrm { NH } _ { 4 } { } ^ { + }$

Answer: D

Solution: A. $\mathrm { SO } _ { 4 } { } ^ { 2 - }$ and $\mathrm { Ba } ^ { 2 + }$ produce barium sulfate precipitate, which cannot coexist in large quantities in the solution, so A is wrong; B. $\mathrm { Fe } ^ { 2 + } , \mathrm { H } ^ { + } , \mathrm { NO } _ { 3 }$-undergoes redox reaction and cannot coexist in large quantities, so B is wrong; C. $\mathrm { HCO } _ { 3 }$ reacts with $\mathrm { H } ^ { + }$ and cannot coexist in large quantities in the solution, so C is wrong; D. $\mathrm { NH } _ { 4 } { } ^ { + }$ does not react with $\mathrm { Ba } ^ { 2 + } , \mathrm { H } ^ { + } , \mathrm { NO } _ { 3 } { } ^ { - }$ and cannot coexist in large amounts in the solution, so D is correct;

Question 20: 26. The following ionic equations can represent only one chemical reaction ( ) (1) $2 \mathrm { OH }...

26. The following ionic equations can represent only one chemical reaction ( ) (1) $2 \mathrm { OH } ^ { - } + \mathrm { CO } _ { 2 } = \mathrm { CO } ^ { 2 - } + \mathrm { H } _ { 2 } \mathrm { O }$ (2) $\mathrm { CuO } + 2 \mathrm { H } ^ { + } = \mathrm { Cu } ^ { 2 + } + \mathrm { H } _ { 2 } \mathrm { O }$ (3) $\mathrm { Ag } ^ { + } + \mathrm { Cl } ^ { - } = \mathrm { AgCl } \downarrow$ (4) $\mathrm { Fe } + \mathrm { Cu } ^ { 2 + } = \mathrm { Fe } ^ { 2 + } + \mathrm { Cu }$

  • A. A. (1) (3)
  • B. B. (2) (4)
  • C. C. (2) (3)
  • D. D. hasn't

Answer: D

Solution: (1) Indicates a reaction in which a soluble strong base reacts with carbon dioxide to form a soluble carbonate and water, such as the reaction between $\mathrm { NaOH } , \mathrm { KOH }$ and $\mathrm { CO } _ { 2 }$, and (1) does not meet the meaning of the question; (2) Indicates a reaction in which CuO reacts with a strong soluble acid to form a soluble copper salt and water, such as the reaction between CuO and $\mathrm { HCl } , \mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$, etc., and (2) does not meet the meaning of the question; (3) denotes the reaction of a soluble silver salt with a soluble chloride or hydrochloric acid, such as the reaction of $\mathrm { AgNO } _ { 3 }$ with $\mathrm { NaCl } , \mathrm { HCl }$, etc. (3) does not meet the meaning of the question; (4) represents the reaction of Fe with soluble copper salts, such as the reaction of Fe with $\mathrm { CuSO } _ { 4 } , \mathrm { CuCl } _ { 2 }$, etc., and (4) does not fit the question; Answer choice D.

Question 21: 28. The following reactions are both ionic and redox reactions

28. The following reactions are both ionic and redox reactions

  • A. A. NaCl solution and $\mathrm { AgNO } _ { 3 }$ solution
  • B. B. Zinc tablets and hydrochloric acid
  • C. C. Hydrogen burning in oxygen
  • D. D. Ba(NO3)2 solution and $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$ solution

Answer: B

Solution: A. The formation of silver chloride precipitate from NaCl solution and $\mathrm { AgNO } _ { 3 }$ solution is not a redox reaction because there is no change in the valence of the elements; B. Zinc and hydrogen ions in hydrochloric acid to generate hydrogen and zinc ions, redox reactions, ionic reactions, B meets the question; C. The reaction between hydrogen and oxygen is a nonionic reaction; D. Ba(NO3) ${ } _ { 2 }$ solution and $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$ solution produce barium sulfate precipitate, there is no change in the elemental valence, not a redox reaction, D does not meet the meaning of the question;

Question 22: 29. The correct ionic equation for the following reaction is

29. The correct ionic equation for the following reaction is

  • A. A. Putting iron powder into dilute sulfuric acid: $6 \mathrm { H } ^ { + } + 2 \mathrm { Fe } = 2 \mathrm { Fe } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \uparrow$
  • B. B. Insertion of a copper sheet into a dilute hydrochloric acid solution : $\mathrm { Cu } + 2 \mathrm { H } ^ { + } = \mathrm { Cu } ^ { 2 + } + \mathrm { H } _ { 2 } \uparrow$
  • C. C. Reaction of calcium carbonate with dilute hydrochloric acid: $\mathrm { CaCO } _ { 3 } + 2 \mathrm { H } ^ { + } = \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$
  • D. D. Reaction of clarified limewater with dilute hydrochloric acid $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 } + 2 \mathrm { H } ^ { + } = \mathrm { Ca } ^ { 2 + } + 2 \mathrm { H } _ { 2 } \mathrm { O }$

Answer: C

Solution: A. The ionic reaction of putting iron powder into dilute sulfuric acid is: $2 \mathrm { H } ^ { + } + \mathrm { Fe } = \mathrm { Fe } ^ { 2 + } + \mathrm { H } _ { 2 } \uparrow$ , A error. B.The insertion of a copper sheet into a dilute hydrochloric acid solution does not react, and B is incorrect. C. The ionic reaction between calcium carbonate and dilute hydrochloric acid is: $\mathrm { CaCO } _ { 3 } + 2 \mathrm { H } ^ { + } = \mathrm { Ca } ^ { 2 + } + \mathrm { CO } _ { 2 } \uparrow + \mathrm { H } _ { 2 } \mathrm { O }$ , C is correct. D. Clarified limewater reacts with dilute hydrochloric acid $\mathrm { OH } ^ { - } + \mathrm { H } ^ { + } = \mathrm { H } _ { 2 } \mathrm { O }$ , D is wrong. The answer is C.

Question 23: 33. The group of ions that must be able to coexist in large quantities under the following condition...

33. The group of ions that must be able to coexist in large quantities under the following conditions are

  • A. A. In a solution containing a large amount of $\mathrm { S } ^ { 2 - }$: $\mathrm { Fe } ^ { 3 + } , \mathrm { Cl } ^ { - } , \mathrm { Na } ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - }$
  • B. B. In the solution that makes phenolphthalein solution red: $\mathrm { NH } _ { 4 } ^ { + } , \mathrm {~K} ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { NO } _ { 3 } ^ { - }$
  • C. C. In a clear solution: $\mathrm { K } ^ { + } , \mathrm { Na } ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { MnO } _ { 4 } ^ { - }$
  • D. D. In an aqueous solution containing a large amount of $\mathrm { CH } _ { 3 } \mathrm { COO } ^ { - }$: $\mathrm { NH } _ { 4 } ^ { + } , \mathrm { Fe } ^ { 2 + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { H } ^ { + }$

Answer: C

Solution: A. $\mathrm { S } ^ { 2 - }$ reacts with $\mathrm { Fe } ^ { 3 + }$ in a redox reaction and cannot coexist in large amounts; B. The solution that makes phenolphthalein solution red is alkaline, and $\mathrm { OH } ^ { - }$ reacts with $\mathrm { NH } _ { 4 } ^ { + }$ in alkaline solution, so they cannot coexist in large quantities; C. The ions do not react with each other and can coexist, C is correct; D. In an aqueous solution containing a large amount of $\mathrm { CH } _ { 3 } \mathrm { COO } ^ { - }$, $\mathrm { H } ^ { + }$ can react with $\mathrm { CH } _ { 3 } \mathrm { COO } ^ { - }$ to form a weak electrolyte, which cannot coexist in large quantities, D is wrong;

Question 24: 34 . At room temperature, each of the following groups of ions can coexist in large quantities in a ...

34 . At room temperature, each of the following groups of ions can coexist in large quantities in a given solution ()

  • A. A. Solution of $\mathrm { pH } = 12$: $\mathrm { Na } ^ { + } , \mathrm {~K} ^ { + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { CO } _ { 3 } ^ { 2 - }$
  • B. B. Solution that turns phenolphthalein red: $\mathrm { Mg } ^ { 2 + } , \mathrm { Ba } ^ { 2 + } , \mathrm { ClO } ^ { - } , \mathrm { SO } _ { 3 } ^ { 2 - }$
  • C. C. $0.1 \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$ in $\mathrm { FeCl } _ { 3 }$ solution: $\mathrm { Al } ^ { 3 + } , \mathrm { NH } _ { 4 } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { I } ^ { - }$
  • D. D. Water ionized solution of $\mathrm { c } \left( \mathrm { H } ^ { + } \right) = 1 \times 10 ^ { - 13 } \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$: $\mathrm { K } ^ { + } , \mathrm { NH } _ { 4 } ^ { + } , \mathrm { I } ^ { - } , \mathrm { C } _ { 6 } \mathrm { H } _ { 5 } \mathrm { O } ^ { - }$

Answer: A

Solution: A, $\mathrm { pH } = 12$ contains a large amount of $\mathrm { OH } ^ { - }$ in solution, which is able to coexist with $\mathrm { Na } ^ { + } , \mathrm {~K} ^ { + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { CO } _ { 3 } ^ { 2 - }$ in large amounts, so A is correct; B, the solution that can make phenolphthalein turn red, the solution is alkaline, a large number of $\mathrm { OH } ^ { - } , \mathrm { Mg } ^ { 2 + }$ can not coexist in large quantities in the solution, and $\mathrm { ClO } ^ { - } , \mathrm { SO } _ { 3 } ^ { 2 - }$ can undergo a redox reaction, can not be coexisted in large quantities, so B is wrong; C. $\mathrm { FeCl } _ { 3 }$ solution is oxidizing and cannot coexist with $\mathrm { I } ^ { - }$ in large amounts, so C is wrong; D. The solution of $\mathrm { c } \left( \mathrm { H } ^ { + } \right) = 1 \times 10 ^ { - 13 } \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$ ionized by water may be alkaline or acidic, and it cannot coexist with $\mathrm { c } \left( \mathrm { H } ^ { + } \right) = 1 \times 10 ^ { - 13 } \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$ under acidic conditions. D, the solution of water-ionized $\mathrm { c } \left( \mathrm { H } ^ { + } \right) = 1 \times 10 ^ { - 13 } \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$ may be alkaline or acidic, and it cannot coexist with ${ } ^ { \mathrm { NH } _ { 4 } ^ { + } }$ in large quantities under acidic conditions, so D is incorrect.

Question 25: 35. A process for purifying a sample of white phosphorus (with inert impurities) is shown in the fig...

35. A process for purifying a sample of white phosphorus (with inert impurities) is shown in the figure, and the following statements are false ( ) ![](/images/questions/ionic-reactions/image-004.jpg)

  • A. A. If white phosphorus accidentally gets on the skin, rinse with a dilute solution of $\mathrm { CuSO } _ { 4 }$.
  • B. B. The ratio of the amounts of oxidized and reduced products in process I is $3 : 5$
  • C. C. In Process II, in addition to $\mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 }$, $\mathrm { Ca } \left( \mathrm { H } _ { 2 } \mathrm { PO } _ { 4 } \right) _ { 2 } , \mathrm { CaHPO } _ { 4 }$ may be generated.
  • D. D. The chemical equation for Process III is $2 \mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 } + 6 \mathrm { SiO } _ { 2 } + 10 \mathrm { C } \xlongequal { \text { high temperature } } 6 \mathrm { CaSiO } _ { 3 } + \mathrm { P } _ { 4 } + 10 \mathrm { CO } \uparrow$

Answer: B

Solution: A. White phosphorus is toxic and corrosive to the skin, and from the figure, white phosphorus can react with copper sulfate solution. Therefore, white phosphorus can be rinsed with copper sulfate solution if it is accidentally dipped into the skin, so A is correct; B. As can be seen from the figure, the reaction of process I is $11 \mathrm { P } _ { 4 } + 60 \mathrm { CuSO } _ { 4 } + 96 \mathrm { H } _ { 2 } \mathrm { O } = 20 \mathrm { Cu } _ { 3 } \mathrm { P } \downarrow + 24 \mathrm { H } _ { 3 } \mathrm { PO } _ { 4 } + 60 \mathrm { H } _ { 2 } \mathrm { SO } _ { 4 }$, the reaction of the phosphorus element of the valence of the oxidized and lowered by the reduction of the copper element of the valence of the reduction of the copper element of the reduction of the copper phosphide is the reaction of the reduction product of phosphoric acid is the reaction of the oxidation product, the oxidized product and the reduction of the product of the ratio of the quantity of matter is 6:5, so B is wrong; C. Phosphoric acid is a strong acid in the ternary, and calcium hydroxide solution reaction, can generate calcium phosphate and calcium phosphate precipitate, can also generate calcium dihydrogen phosphate, so C is correct; D. As can be seen from the figure, the process III reaction occurs for calcium phosphate and silica and carbon under high-temperature conditions to generate calcium silicate, white phosphorus and carbon monoxide, the reaction of the chemical equation for $2 \mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 } + 6 \mathrm { SiO } _ { 2 } + 10 \mathrm { C } \xlongequal { \text { high temperature } } 6 \mathrm { CaSiO } _ { 3 } + \mathrm { P } _ { 4 } + 10 \mathrm { CO } \uparrow$, so D is correct;

Question 26: 36. The following ions must be able to coexist in large quantities under the specified conditions ()

36. The following ions must be able to coexist in large quantities under the specified conditions ()

  • A. A. $c \left( \mathrm { H } ^ { + } \right) = c \left( \mathrm { OH } ^ { - } \right)$ in solution : $\mathrm { Al } ^ { 3 + } , \mathrm { Na } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { SO } _ { 4 } ^ { 2 - }$
  • B. B. In the solution of ${ } ^ { \mathrm { AlO } _ { 2 } ^ { - } }$ produced by the addition of aluminum powder : $\mathrm { K } ^ { + } , \mathrm { Ba } ^ { 2 + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { Cl } ^ { - }$
  • C. C. In a solution that turns dark blue with litmus: $\mathrm { Na } ^ { + } , \mathrm {~K} ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { HCO } _ { 3 } ^ { - }$
  • D. D. In a solution that produces a precipitate when hydrochloric acid is added dropwise: $\mathrm { Ca } ^ { 2 + } , \mathrm { Na } ^ { + } , \mathrm { NO } _ { 3 } ^ { - } , \mathrm { Cl } ^ { - }$

Answer: B

Solution: A. A solution of $c \left( \mathrm { H } ^ { + } \right) = c \left( \mathrm { OH } ^ { - } \right)$ is neutral, while a solution containing $\mathrm { Al } ^ { 3 + }$ is acidic and cannot coexist in large quantities in a neutral solution, A is wrong; B. The solution with ${ } ^ { \mathrm { AlO } _ { 2 } ^ { - } }$ generated by adding aluminum powder is alkaline, and the solution with a large amount of $\mathrm { OH } ^ { - } , \mathrm { OH } ^ { - }$ and the option ions cannot react with each other, so they can coexist in large quantities, B is correct; C. The solution that turns dark blue when met with litmus is alkaline, and contains a large amount of $\mathrm { OH } ^ { - } , \mathrm { OH } ^ { - }$ which reacts with $\mathrm { HCO } _ { 3 } ^ { - }$ to produce $\mathrm { CO } _ { 3 } ^ { 2 - }$ and $\mathrm { H } _ { 2 } \mathrm { O }$, which cannot coexist in large quantities, and is incorrect, and is wrong, and is not correct, C. The solution that turns dark blue when met with litmus is alkaline; D. The solution that can produce a precipitate by adding hydrochloric acid may contain $\mathrm { Ag } ^ { + }$ or $\mathrm { SiO } _ { 3 } ^ { 2 - } , \mathrm { Ag } ^ { + }$ and $\mathrm { Cl } ^ { - }$ will react to produce a white precipitate of AgCl, which cannot coexist in large quantities; Therefore, the reasonable choice is $B$.

Question 27: 37. The following images are correctly interpreted () | A | B | | :---- | :--- | | ![](/images/ques...

37. The following images are correctly interpreted () | A | B | | :---- | :--- | | ![](/images/questions/ionic-reactions/image-005.jpg) | ![](/images/questions/ionic-reactions/image-006.jpg) | | $\mathrm { AgNO } _ { 3 }$ solution is added drop by drop to dilute hydrochloric acid, and the curve of the conductivity of the mixture over time | $8 \mathrm { Al } + 3 \mathrm { Fe } _ { 3 } \mathrm { O } _ { 4 } \xlongequal { \text { high temperature } } 9 \mathrm { Fe } + 4 \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$ , the reaction <br> type belongs to the shaded part of the diagram | | C | D | | ![](/images/questions/ionic-reactions/image-007.jpg) | ![](/images/questions/ionic-reactions/image-008.jpg) | ![](/images/questions/ionic-reactions/image-008.jpg) | Copper reacts with concentrated sulfuric acid single line bridge | Schematic diagram of hydrated chloride ions formed by dissolution of NaCl solids |

  • A. A. A
  • B. B. B
  • C. C. C
  • D. D. D

Answer: D

Solution: A. When $\mathrm { AgNO } _ { 3 }$ solution is added drop by drop to dilute hydrochloric acid, the reaction is $\mathrm { HCl } + \mathrm { AgNO } _ { 3 } = \mathrm { AgCl } \downarrow + \mathrm { HNO } _ { 3 }$ which The conductivity of the mixed solution does not drop to 0. A. Wrong; B. The shaded reaction is a redox reaction in addition to the four basic reaction types, $8 \mathrm { Al } + 3 \mathrm { Fe } _ { 3 } \mathrm { O } _ { 4 } \xlongequal { \text { high temperature } }$ $9 \mathrm { Fe } + 4 \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 }$, which is a replacement reaction, does not meet the requirements, B is wrong; C. Copper reacts with concentrated sulfuric acid to form copper sulfate and sulfur dioxide, water, copper loses electrons, sulfur gains electrons, and the arrow of the single-wire bridge points from copper to sulfur, C is wrong; D. Chloride ions are negatively charged, the water molecule H shows a positive valence, so the diagram shows the formation of hydrated chloride ions from the dissolution of NaCl solids, D is correct; Answer choice D.

Question 28: 38. In the following reaction, the ionic equation is $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - }...

38. In the following reaction, the ionic equation is $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O }$.

  • A. A. $\mathrm { CH } _ { 3 } \mathrm { COOH } + \mathrm { NaOH } = \mathrm { CH } _ { 3 } \mathrm { COONa } + \mathrm { H } _ { 2 } \mathrm { O }$
  • B. B. $\mathrm { HNO } _ { 3 } + \mathrm { KOH } = \mathrm { KNO } _ { 3 } + \mathrm { H } _ { 2 } \mathrm { O }$
  • C. C. $3 \mathrm { HCl } + \mathrm { Fe } ( \mathrm { OH } ) _ { 3 } = \mathrm { FeCl } _ { 3 } + 3 \mathrm { H } _ { 2 } \mathrm { O }$
  • D. D. $\mathrm { H } _ { 2 } \mathrm { SO } _ { 4 } + \mathrm { Ba } ( \mathrm { OH } ) _ { 2 } = \mathrm { BaSO } _ { 4 } \downarrow + 2 \mathrm { H } _ { 2 } \mathrm { O }$

Answer: B

Solution: A. $\mathrm { CH } _ { 3 } \mathrm { COOH }$ is a weak acid, you should write the chemical formula, and its ionic equation is $\mathrm { CH } _ { 3 } \mathrm { COOH } + \mathrm { OH } ^ { - } = \mathrm { CH } _ { 3 } \mathrm { COO } ^ { - } + \mathrm { H } _ { 2 } \mathrm { O }$ , A is wrong ; B. Nitric acid is a soluble strong acid, potassium hydroxide is a soluble strong acid, and the potassium nitrate produced by the reaction of the two is a soluble salt, so the ionic equation can be expressed by $\mathrm { H } ^ { + } + \mathrm { OH } ^ { - } = \mathrm { H } _ { 2 } \mathrm { O }$, B is correct; C. $\mathrm { Fe } ( \mathrm { OH } ) _ { 3 }$ is insoluble in water, and the chemical formula should be written. The ionic equation of the reaction between the two is $3 \mathrm { H } ^ { + } + \mathrm { Fe } ( \mathrm { OH } ) _ { 3 } = \mathrm { Fe } ^ { 3 + } + 3 \mathrm { H } _ { 2 } \mathrm { O }$, C is wrong; D. Barium ions and sulfate can also react, and the ionic equation of their reaction is $2 \mathrm { H } ^ { + } + \mathrm { SO } ^ { 2 - } + \mathrm { Ba } ^ { 2 + } + 2 \mathrm { OH } ^ { - } = \mathrm { BaSO } _ { 4 } \downarrow + 2 \mathrm { H } _ { 2 } \mathrm { O }$, D is wrong; Answer choice B.

Question 29: 39. In a solution containing the following groups of ions, the ions can still be present in large qu...

39. In a solution containing the following groups of ions, the ions can still be present in large quantities after an excess of a certain gas is passed through the solution. | Options | Ions in solution | Excess gas | | :--- | :--- | :--- | | A | $\begin{array} { l l l l l } \mathrm { H } ^ { + } & \mathrm { Ba } ^ { 2 + } & \mathrm { Al } ^ { 3 + } & \mathrm { I } ^ { - } \end{array}$ | $\mathrm { O } _ { 2 }$ | | :--- | :--- | :--- | | B | $\begin{array} { l l l l } \mathrm { HS } ^ { - } & \mathrm { Na } ^ { + } & \mathrm { Br } ^ { - } & \mathrm { SO } _ { 4 } ^ { 2 - } \end{array}$ | $\mathrm { SO } _ { 2 }$ | | C | $\mathrm { Mg } ^ { 2 + } , \mathrm { Na } ^ { + } , \mathrm { SO } _ { 4 } ^ { 2 - } , \mathrm { Cl } ^ { - }$ | $\mathrm { NH } _ { 3 }$ | | D | | $\mathrm { CO } _ { 2 }$ |

  • A. A. A
  • B. B. B
  • C. C. C
  • D. D. D

Answer: D

Solution: A. Oxygen oxidizes I to $I _ { 2 }$, so A is not chosen; B. $\mathrm { HS } ^ { - }$ reacts with $\mathrm { SO } _ { 2 }$ in a neutralization reaction to form S monomer, so B is not chosen; C. $\mathrm { Mg } ^ { 2 + }$ reacts with ammonia to form magnesium hydroxide precipitate; D. $\mathrm { Al } ^ { 3 + } , \mathrm { Cl } ^ { - } , \mathrm {~K} ^ { + } , \mathrm { NO } _ { 3 } ^ { - }$ does not react with carbon dioxide gas, and the ions still react with carbon dioxide gas in excess. can exist in large amounts, so choice D; Choice D. $40 . \mathrm { C }$ [Knowledge Points]Conditions for the occurrence of ionic reactions, ionic coexistence, ionic coexistence under limited conditions does not match; B. Phenolphthalein red solution is basic: $\mathrm { NH } _ { 4 } { } ^ { + } , \mathrm { OH } ^ { - }$ reacts to form $\mathrm { NH } _ { 3 } \cdot \mathrm { H } _ { 2 } \mathrm { O }$, so B does not match; C. A solution of $\mathrm { pH } = 12$: no precipitate, gas, water, or redox reaction occurs between $\mathrm { K } ^ { + } , \mathrm { Na } ^ { + } , \mathrm { CH } _ { 3 } \mathrm { COO } ^ { - } , \mathrm { Br } ^ { - }$ and $\mathrm { OH } -$; D. The solution that reacts with aluminum to produce large amounts of hydrogen may be acidic or basic: $\mathrm { CO } _ { 3 } { } ^ { 2 - }$ does not exist in large amounts under acidic conditions, and $\mathrm { NO } _ { 3 } { } ^ { - }$ does not react with aluminum to produce hydrogen under acidic conditions, so D is not true;

Question 30: 40. At room temperature, each of the following groups of ions must be able to coexist in large quant...

40. At room temperature, each of the following groups of ions must be able to coexist in large quantities in the specified solution High School Chemistry Assignment, October 31, 2025

  • A. A. $1.0 \mathrm {~mol} \cdot \mathrm {~L} ^ { - 1 }$ of $\mathrm { KNO } _ { 3 }$ solution: $\mathrm { H } ^ { + } , \mathrm { Fe } ^ { 2 + } , \mathrm { Cl } ^ { - } , \mathrm { SO } _ { 4 } { } ^ { 2 - }$
  • B. B. Phenolphthalein red solution: $\mathrm { NH } _ { 4 } { } ^ { + } , \mathrm { Ba } ^ { 2 + } , \mathrm { AlO } _ { 2 } { } ^ { - } , \mathrm { Cl } ^ { - }$
  • C. C. Solution of $\mathrm { pH } = 12$: $\mathrm { K } ^ { + } , \mathrm { Na } ^ { + } , \mathrm { CH } _ { 3 } \mathrm { COO } ^ { - } , \mathrm { Br } ^ { - }$
  • D. D. Solutions that react with aluminum to produce large amounts of hydrogen gas: $\mathrm { Na } ^ { + } , \mathrm {~K} ^ { + } , \mathrm { CO } _ { 3 } { } ^ { 2 - } , \mathrm { NO } _ { 3 } { } ^ { - }$

Answer: C

Solution:
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Ionic Reactions and Tests

离子反应与检验

30 Practice Questions

Practice with Chinese questions to prepare for the CSCA exam. You can toggle translations while practicing.

Topic Overview

Ionic reactions and tests are the core content of the Chemistry exam, mainly involving the judgment of whether ions can coexist in large quantities in a solution, ion test methods, and ion concentration calculations. The questions are often given through the combination of ions or experimental phenomena, to test students' understanding of the nature of ions, the law of reaction and charge conservation. Mastery of this part of the knowledge is essential for solving problems related to electrolyte solutions.

Questions:30

Key Points

  • 1Ion coexistence judgment: according to the decomposition reaction conditions (precipitate, gas, weak electrolyte) to analyze whether the ions can coexist
  • 2Ion test methods: master the characteristic reactions and identification sequence of common ions (e.g., Cl-, SO₄²-, NH₄⁺, etc.)
  • 3Application of charge conservation: calculation of unknown ion concentrations or ratios using the principle of solution electroneutrality
  • 4Implicit condition analysis: identifying the effect of pH, color, redox, and other constraints on the presence of ions in a topic

Study Tips

Systematic memorization of the color, solubility, and characteristic reactions of common ions is recommended, as well as extensive practice to develop the ability to quickly identify interactions between ions.

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