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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 7

Which of the following solutions will not form a precipitate when added to 10 mL of 0.10 M KOH? (LO 4.10, 4.11) (a) 10 mL of 0.10 NH4Cl (b) 10 mL of 0.10 M PbSO4 (c) 10 mL of 0.10 M Fe(NO3)3 (d) 10 mL of 0.10 M AgCH3CO2

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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 ionic compounds react in solution to form an insoluble compound, known as a precipitate. The solubility of the resulting compounds can be predicted using solubility rules, which state that certain combinations of ions will not dissolve in water. Understanding these rules is essential for determining whether a precipitate will form when mixing solutions.
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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is a numerical value that represents the equilibrium between a solid and its ions in a saturated solution. It helps predict whether a precipitate will form based on the concentrations of the ions in solution. If the product of the ion concentrations exceeds the Ksp, a precipitate will form; if not, the ions remain in solution.
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Common Ion Effect

The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. This phenomenon is important in precipitation reactions, as the presence of a common ion can shift the equilibrium, potentially preventing the formation of a precipitate. Recognizing the common ions in the solutions being mixed is crucial for predicting the outcome of the reaction.
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Related Practice
Textbook Question
Refer to the figure to answer questions 4 and 5. The images are a molecular representation of three different substances, AX3, AY3, and AZ3, dissolved in water. (Water molecules are omitted for clarity.)

Which of the substances is the weakest electrolyte? (LO 4.6) (a) AX3 (b) AY3 (c) AZ3 (d) All of the substances are strong electrolytes.
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Textbook Question
Refer to the figure to answer questions 4 and 5. The images are a molecular representation of three different substances, AX3, AY3, and AZ3, dissolved in water. (Water molecules are omitted for clarity.) What are the molar concentrations of A ions and X ions in a 0.500 M solution of AX3? (LO 4.7) (a) 0.500 M A and 0.500 M X (b) 0.500 M A and 0.167 M X (c) 1.500 M A and 0.500 M X (d) 0.500 M A and 1.500 M X
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Textbook Question
Which of the following substances will produce a solution that does not conduct electricity when it dissolves in water? (LO 4.6) (a) NaOH (b) HNO3 (c) Na2SO4 (d) CH3OH
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Textbook Question
Write a net ionic equation for the reaction that occurs when 10 mL of 0.5 M ammonium carbonate is mixed with 10 mL of 0.5 M silver nitrate. (LO 4.9, 4.11) (a) (b) (c) (d) A net ionic reaction cannot be written because a reaction does not take place.
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Textbook Question
When 75.0 mL of a 0.100 M lead(II) nitrate solution is mixed with 100.0 mL of a 0.190 M potassium iodide solu-tion, a yellow-orange precipitate of lead(II) iodide is formed. What is the mass in grams of lead(II) iodide formed? Assume the reaction goes to completion. (LO 4.11, 4.15) (a) 1.729 g (b) 3.458 g (c) 4.380 g (d) 8.760 g
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Textbook Question
What volume of 0.250 M HCl is needed to react completely with 25.00 mL of 0.375 M Na2CO3? (LO 4.15) (a) 75.0 mL (b) 18.8 mL (c) 37.5 mL (d) 33.3 mL
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