Question

question 39 (1 point)
the table below shows the solubility product constants of different compounds in
the same solvent and at the same temperature. which compound is the least soluble
under these conditions?

row	compound	$k_{sp}$
b.	pbcro₄, lead chromate	2.3 × 10⁻¹³
c.	pbco₃, lead carbonate	7.4 × 10⁻¹⁴
d.	pbi₂, lead iodide	9.8 × 10⁻⁹
e.	pb(oh)₂, lead hydroxide	1.4 × 10⁻²⁰

○ a
○ b
○ c
○ d
○ e

Explanation:

Step1: Recall \( K_{sp} \) and solubility relationship

For sparingly soluble salts, the solubility product constant (\( K_{sp} \)) is related to solubility. A smaller \( K_{sp} \) (for salts with similar dissociation stoichiometry) or after considering stoichiometry, a lower \( K_{sp} \) generally means lower solubility. Here, we compare the magnitudes of \( K_{sp} \) values directly (since we can analyze the exponents and coefficients).

Step2: Compare \( K_{sp} \) values

• A: \( 6.6\times10^{-6} \)
• B: \( 2.3\times10^{-13} \)
• C: \( 7.4\times10^{-14} \)
• D: \( 9.8\times10^{-9} \)
• E: \( 1.4\times10^{-20} \)

The smallest \( K_{sp} \) is \( 1.4\times10^{-20} \) (for \( \text{Pb(OH)}_2 \)), so it has the least solubility.

Answer:

E. \( \text{Pb(OH)}_2 \), Lead hydroxide