After 20.0g of $Na_2SO_4$ are added to a 0.5 L saturated solution of $CaSO_4$ , does the concentration of $Ca^(2+)$ increase, decrease, or stay the same?

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After 20.0g of $Na_2SO_4$ are added to a 0.5 L saturated solution of $CaSO_4$ , does the concentration of $Ca^(2+)$ increase, decrease, or stay the same?

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Answer 1 · 2016-04-01T13:00:44

$[Ca^(2+)]$ will reduce.

Explanation:

The calcium sulfate is saturated. That is, the reaction,

$Ca^(2+) + SO_4^(2-) rightleftharpoons CaSO_4(s)$ is at equilibrium. The addition of more sulfate anion will drive the equilibrium to the right. Calcium sulfate will precipitate, with reduction in $[Ca^(2+)]$ , so that the ion product resatisfies the solubility expression, $K_(sp) = [Ca^(2+)][SO_4^(2-)]$ .

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After 20.0g of $Na_2SO_4$ are added to a 0.5 L saturated solution of $CaSO_4$ , does the concentration of $Ca^(2+)$ increase, decrease, or stay the same?

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Explanation:

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After 20.0g of Na_2SO_4Na_2SO_4 are added to a 0.5 L saturated solution of CaSO_4CaSO_4, does the concentration of Ca^(2+)Ca^(2+) increase, decrease, or stay the same?

1 Answer

Explanation:

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After 20.0g of $Na_2SO_4$ are added to a 0.5 L saturated solution of $CaSO_4$ , does the concentration of $Ca^(2+)$ increase, decrease, or stay the same?