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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
All textbooksBrown 15th EditionCh.4 - Reactions in Aqueous SolutionProblem 87b
Chapter 4, Problem 87b

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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1
Identify the ions present in each solution: KOH dissociates into K^+ and OH^- ions, while NiSO_4 dissociates into Ni^{2+} and SO_4^{2-} ions.
Determine the possible combinations of ions that could form a precipitate: K^+ with SO_4^{2-} and Ni^{2+} with OH^-.
Use the solubility rules to determine which combination forms a precipitate: K_2SO_4 is soluble, while Ni(OH)_2 is insoluble.
Conclude that Ni(OH)_2 is the precipitate that forms when the solutions are mixed.
Write the balanced chemical equation for the precipitation reaction: Ni^{2+} (aq) + 2OH^- (aq) \(\rightarrow\) Ni(OH)_2 (s).

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Key Concepts

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

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble compound, known as a precipitate. This process is driven by the formation of a product that is not soluble in the solvent, leading to the separation of the solid from the liquid. Understanding the solubility rules helps predict which compounds will precipitate under given conditions.
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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that quantifies the solubility of a sparingly soluble ionic compound. It is calculated from the concentrations of the ions in a saturated solution at a specific temperature. When the product of the ion concentrations exceeds the Ksp, a precipitate will form, indicating that the solution is supersaturated.
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Stoichiometry of Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. In this context, it is essential to determine the moles of KOH and NiSO4 present in the solutions to assess the potential for a reaction and the formation of a precipitate. This allows for the identification of limiting reactants and the amounts of products formed.
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Related Practice
Textbook Question

A 0.5895-g sample of impure magnesium hydroxide is dissolved in 100.0 mL of 0.2050 M HCl solution. The excess acid then needs 19.85 mL of 0.1020 M NaOH for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

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Textbook Question

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

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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. (a) Write the balanced chemical equation for the reaction that occurs.

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Textbook Question

A solution is made by mixing 15.0 g of Sr(OH)2 and 55.0 mL of 0.200 M HNO3. b. Calculate the concentration of each ion remaining in solution.

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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

A solution is made by mixing 15.0 g of Sr(OH)2 and 55.0 mL of 0.200 M HNO3. c. Is the resulting solution acidic or basic?