What is the relationship between the K_sp expressions for a chemical reaction and its reverse chemical reaction?

What is the relationship between the K_w value for H₂O and its reverse chemical reaction?

For the equilibrium

$${\text{PCl}}_{\text{3}}{\text{(g) + Cl}}_{\text{2}}\text{(g)}\rightleftarrows {\text{PCl}}_{\text{5}}\text{(g) + 60 kJ}$$

list four stresses that serve to increase the amount of PCl₅.

For the equilibrium

$${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}\text{ + 57 kJ}\rightleftarrows {\text{2NO}}_{\text{2}}$$

list four stresses that serve to increase the amount of NO₂.

Does a very large K_eq favor the reactants or the products? Explain your answer.

Is the K_eq for reactions that favor reactants large or small? Explain your answer.

Show that K_a × K_b = K_w by determining the expressions for these two reactions and multiplying them together.

$$\text{HX(aq)}\rightleftarrows {\text{H}}^{\text{+}}{\text{(aq) + X}}^{\text{–}}\text{(aq)}$$ $${\text{X}}^{\text{–}}{\text{(aq) + H}}_{\text{2}}\text{O(}\ell \text{)}\rightleftarrows {\text{HX(aq) + OH}}^{\text{–}}\text{(aq)}$$

Is the conjugate base of a strong acid weak or strong? Explain your answer.

What is the solubility in moles per liter of AgCl? Use data from Table 13.2 "Solubility Product Constants for Slightly Soluble Ionic Compounds".

What is the solubility in moles per liter of Ca(OH)₂? Use data from Table 13.2 "Solubility Product Constants for Slightly Soluble Ionic Compounds".

Under what conditions is K_eq = K_P?

Under what conditions is K_eq > K_P when the temperature is 298 K?

What is the pH of a saturated solution of Mg(OH)₂? Use data from Table 13.2 "Solubility Product Constants for Slightly Soluble Ionic Compounds".

What are the pH and the pOH of a saturated solution of Fe(OH)₃? The K_sp of Fe(OH)₃ is 2.8 × 10⁻³⁹.

For a salt that has the general formula MX, an ICE chart shows that the K_sp is equal to x², where x is the concentration of the cation. What is the appropriate formula for the K_sp of a salt that has a general formula of MX₂?

Referring to Exercise 15, what is the appropriate formula for the K_sp of a salt that has a general formula of M₂X₃ if the concentration of the cation is defined as 2x, rather than x?

Consider a saturated solution of PbBr₂(s). If [Pb²⁺] is 1.33 × 10⁻⁵ M, find each of the following.

1. [Br⁻]
2. the K_sp of PbBr₂(s)

Consider a saturated solution of Pb₃(PO₄)₂(s). If [Pb²⁺] is 7.34 × 10⁻¹⁴ M, find each of the following.

1. [PO₄³⁻]
2. the K_sp of Pb₃(PO₄)₂(s)