   # A 50.0-mL sample of 0.00200 M AgNO 3 is added to 50.0 mL of 0.0100 M NaIO 3 . What is the equilibrium concentration of Ag + in solution? ( K sp for AgIO 3 is 3.0 × 10 −8 .) ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 15, Problem 55E
Textbook Problem
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## A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 M NaIO3. What is the equilibrium concentration of Ag+ in solution? (Ksp for AgIO3 is 3.0 × 10−8.)

Interpretation Introduction

Interpretation: The concentration and volume of AgNO3,NaIO3 and solubility product of AgIO3 is given. The equilibrium concentration of Ag+ is to be calculated.

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

Solubility product Ksp is defined as the 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 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 of Solution

Explanation

To determine: The equilibrium concentration of Ag+ in a solution prepared by adding 50mL of 0.00200M AgNO3 to 50mL of 1.0M NaIO3 .

The initial concentration of Ag+ is 0.001M_ and initial concentration of IO3(aq) is 0.005M_ .

Given

Concentration of AgNO3 is 0.00200M .

Concentration of NaIO3 is 0.0100M .

Solubility product of AgIO3 is 3×108 .

Volume of AgNO3 is 50mL .

Volume of NaIO3 is 50mL .

The AgIO3 will only precipitate out during mixing of AgNO3 and NaIO3 if,

Ksp<Q

It is assumed that the concentration of Ag+ and IO3(aq) is same as the concentration of AgNO3 and NaIO3 . Hence, concentration of Ag+ and IO3(aq) is,

[Ag+]=0.00200M[IO3(aq)]=0.0100M

Formula

The initial concentration of compound is calculated using the formula,

Substitute the values of volume, given concentration of Ag+ and volume of original solution in the above equation.

Substitute the values of volume, given concentration of IO3 and volume of original solution in equation (1).

The ion product of AgIO3 is 5×106_ .

Formula

The ion product of AgIO3 is calculated as,

Q=[Ag+]0[IO3]0

Where,

• Q is ion product.
• [Ag+]0 is initial concentration of Ag+ .
• [IO3]0 is initial concentration of IO3 .

Substitute the value of [Ag+]0 and [IO3]0 in the above expression.

Q=[Ag+]0[IO3]0=(0

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