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Ch.4 - Reactions in Aqueous Solution
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 87a
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Chapter 4, Problem 87a

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (a) Write the balanced chemical equation for the reaction that occurs.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, KOH acts as a strong base, providing hydroxide ions (OH-) that can react with metal cations. Understanding the nature of acids and bases is crucial for predicting the products of the reaction.
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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced equations. It allows us to determine the proportions of KOH and NiSO4 that will react, which is essential for writing the balanced chemical equation and understanding the quantities involved.
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Precipitation Reactions

Precipitation reactions occur when two soluble salts react to form an insoluble compound, or precipitate. In this scenario, the reaction between KOH and NiSO4 may produce nickel hydroxide (Ni(OH)2), which is insoluble in water. Recognizing the solubility rules helps in identifying the products of the reaction.
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Related Practice
Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide?

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Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+?

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Textbook Question

An 8.65-g sample of an unknown group 2 metal hydroxide is dissolved in 85.0 mL of water. An acid–base indicator is added and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 56.9 mL of the hydrochloric acid solution has been added. (b) What is the identity of the metal cation: Ca2+, Sr2+, or Ba2+?

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Textbook Question

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (b) What precipitate forms?

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Textbook Question

A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (e) What is the concentration of each ion that remains in solution?

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Textbook Question

A solution is made by mixing 1.5 g of LiOH and 23.5 mL of 1.000 M HNO3. (b) Calculate the concentration of Li+ remaining in solution.

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