   Chapter 16, Problem 50E

Chapter
Section
Textbook Problem

# A solution contains 1.0 × 10−5 M Ag+ and 2.0 × 10−6 M CN−. Will AgCN(s) precipitate? (Ksp for AgCN(s) is 2.2 × 10−12.

Interpretation Introduction

Interpretation: The solubility product and concentration of each ion Ag+ and CN in a solution is given. By using these values, it is to be checked that AgCN(s) will precipitate out or not.

Concept introduction: The formation of solid in a solution is known as precipitation.

The solubility product, Ksp is defined as the product of concentration of ions in a saturated solution where each ion is raised to the power of their coefficients. Ion product, Q is defined as the product of initial concentration of ions in any solution where each ion is raised to the power of their coefficients.

The relation between ion product, Q and solubility product, Ksp is as follows.

• If Ksp>Q , then no precipitate will form.
• If Ksp<Q , then precipitate will form.
• If Ksp=Q , then the solution will be in just saturation.
Explanation

Explanation

To determine: If AgCN will precipitate in the solution that contains the given concentration of Ag+ and CN ions.

The ion product of AgCN is 2.0×1011_ .

Given

Initial concentration of Ag+ is 1.0×105M .

Initial concentration of CN is 2.0×106M .

Solubility product of AgCN is 2.2×1012 .

The AgCN will only precipitate out in the solution if,

Ksp<Q

Formula

The ion product of AgCN is calculated as,

Q=[Ag+]0[CN]0

Where,

• Q is the ion product.
• [Ag+]0 is the initial concentration of Ag+ .
• [CN]0 is the initial concentration of CN

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