   # A 2.14 g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution pH is 11.32. What is K b for the hypoiodite ion? ### 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 13, Problem 187IP
Textbook Problem
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## A 2.14 g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution pH is 11.32. What is Kb for the hypoiodite ion?

Interpretation Introduction

Interpretation: The value of Kb for the hypoiodite ion is to be calculated.

Concept introduction: The term molarity is used to measure the concentration of any species and is defined as the number of moles of solute present in solvent (kg) The formula of molarity is,

Molarity=NumberofmolesofsoluteAmountofsolvent(kg)

To determine: The value of Kb for the hypoiodite ion.

### Explanation of Solution

Explanation

Given

The amount of sodium hypoiodite is 2.14g.

The volume of solution is 1.25L.

The pH is 11.32.

The number of moles for Sodium hypoiodite is calculated by the expression.

Numberofmoles=GivenMassMolarMass

Substitute the value of given mass and molar mass in the above expression.

Numberofmoles=2.14g165.896g/mol=0.012

The value of molarity is calculated by the formula.

Molarity=NumberofmolesofsoluteAmountofsolvent(kg)

Substitute the value of number of moles of solute and amount of solvent in the above expression.

Molarity=0.0121.25=0.0103M

The sum,

pH+pOH=14

Substitute the given value of pH in the above expression.

11.32+pOH=14pOH=1411.32pOH=2.68

The value of [OH] is calculated by the expression.

pOH=log[OH][OH]=10pOH

Substitute the value of calculated pOH in the above expression.

[OH]=102.68[OH]=0.0021M

The ICE (Initial Change Equilibrium) table for the reaction of hypoiodite ion is,

IO+H2OHOI+OHInitial(M):0

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