(a) Will Ca(OH)2 precipitate from solution if the pH of a 0.050 M solution of CaCl2 is adjusted to 8.0? (b) Will Ag2SO4 precipitate when 100 mL of 0.050 M AgNO3 is mixed with 10 mL of 5.0 * 10^-2 M Na2SO4 solution?

Verified step by step guidance

Step 1: Determine the solubility product constant (K_sp) for Ca(OH)_2 and Ag_2SO_4 from a reliable source or textbook.

Step 2: For part (a), calculate the concentration of OH^- ions at pH 8.0 using the formula [OH^-] = 10^{-(14 - pH)}.

Step 3: Calculate the ion product (Q) for Ca(OH)_2 using the formula Q = [Ca^{2+}][OH^-]^2, where [Ca^{2+}] is given as 0.050 M.

Step 4: Compare the ion product (Q) with the solubility product constant (K_sp) for Ca(OH)_2. If Q > K_sp, precipitation will occur.

Step 5: For part (b), calculate the concentrations of Ag^+ and SO_4^{2-} ions after mixing the solutions, then calculate the ion product (Q) for Ag_2SO_4 and compare it with its K_sp to determine if precipitation occurs.

Key Concepts

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

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 is specific to each ionic compound and helps predict whether a precipitate will form when solutions are mixed. If the product of the concentrations of the ions in solution exceeds the Ksp, precipitation occurs.

pH and its Effect on Solubility

pH is a measure of the acidity or basicity of a solution, which can significantly influence the solubility of certain compounds. For example, increasing the pH can lead to the precipitation of metal hydroxides, as many metal ions form insoluble hydroxides at higher pH levels. Understanding the relationship between pH and solubility is crucial for predicting precipitation reactions.

Stoichiometry in Precipitation Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. In precipitation reactions, it is essential to determine the molar ratios of the reactants to assess whether the concentrations of the ions will lead to the formation of a precipitate. This requires balancing the chemical equations and calculating the final concentrations after mixing solutions.