Calculating Ksp From Molar Solubility

Mark

The salt $AB_2$ dissolves in water according to the equation: $AB_2(s) \rightleftharpoons A^{2+}(aq) + 2*B^-(aq)$ . If the molar solubility of the salt is $2.0 \times 10^{-3}\,M$ , what is the value of its solubility product constant, $K_{sp}$ ?

$8.0 \times 10^{-9}$

$1.6 \times 10^{-8}$

$3.2 \times 10^{-8}$

$6.4 \times 10^{-8}$

Hint

Did You Know?

Explain Why

Explain All Answers

Check Answer

Show Correct Answer

Report Question

Question Leaderboard

Rank	User	Correct Count	Attempt Count	Total Time	Score
#1	zamarrona	1	1	0m 00s	100
#2	khaled.aboulhoda	1	1	0m 25s	75
#3	realbloobox	1	4	1m 21s	-11

Items per page:

1 – 3 of 3

AI Tutor 1:23 AM

How can I help?

Email: apfive@apfive.orgPrivacy Policy