A solution contains .10 M Cl- and .10 M Br-. If Ag+ is added until AgCl just begins to...
Question:
A solution contains .10 M Cl- and .10 M Br-. If Ag+ is added until AgCl just begins to precipitate, what are the concentrations of Ag+ and Br-? ( Ksp for AgCl=1.8x10^-10, Ksp for AgBr= 3.3x10^-13)
Fractional Precipitation:
In fractional precipitation, a solution is added dropwise until one solid precipitates first over the other. To evaluate fractional precipitation, use solubility products.
The solubility product {eq}K_{sp} {/eq} is an equilibrium constant for partially soluble ionic solids. For a chemical reaction {eq}A_xB_{y(s)} \rightleftharpoons xA_{(aq)}^{y+}+ yB_{(aq)}^{x-} {/eq} the solubility product is equal to:
{eq}\displaystyle K_{sp}= \left[A^{y+} \right]^x \left[B^{x-}\right]^y \\ {/eq}
Answer and Explanation: 1
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View this answerThe concentration of silver needed to precipitate AgCl is:
{eq}\displaystyle [Ag^+] = \frac{1.8 \times 10^{-10}}{0.1} = 1.8 \times 10^{-9} \ M...
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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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