A solution contains 0.01 M Ba^2+ and 0.01 M Ag^+. Can 99.92% of either ion be precipitated by...
Question:
A solution contains 0.01 M {eq}\rm Ba^{2+} {/eq} and 0.01 M {eq}\rm Ag^+ {/eq}. Can {eq}\rm 99.92\% {/eq} of either ion be precipitated by chromate ({eq}\rm CrO_4^{2-} {/eq}) without precipitating the other metal ion? The {eq}\rm K_{sp} {/eq} for {eq}\rm BaCrO_4 {/eq} is {eq}\rm 2.1 \times 10^{-10} {/eq} and {eq}\rm K_{sp} {/eq} for {eq}\rm Ag_2CrO_4 {/eq} is {eq}1.2 \times 10^{-12} {/eq}.
Solubility Product Constant:
The equilibrium constant for the dissolution of a sparingly soluble salt is known as the solubility product constant. The value of the solubility product constant can give the extent of dissociation of a particular salt. The lower the value, the less soluble a salt is.
Answer and Explanation: 1
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View this answerThe strategy is to determine the concentration of chromate ions required to begin precipitating the salts. This is obtained by using the solubility...
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Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations
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Chapter 11 / Lesson 5
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Learn about solubility product constant. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp.
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