   Chapter 16, Problem 47PS

Chapter
Section
Textbook Problem

A 0.025 M solution of hydroxyl amine has a pH of 9.11. What is the value of Kb for this weak base?H3NOH(aq) + H2O(ℓ) ⇄ H3NOH+(aq) + OH−(aq)

Interpretation Introduction

Interpretation:

The base ionization constant (Kb) of weak base hydroxylamine has to be calculated.

Concept introduction:

The base dissociation constant or base ionization constant of weak base hydroxylamine can be calculated by using the pOH value of hydroxylamine base (which gives the concentration of hydroxide ion) and from the given concentration of. weak base hydroxylamine.

Calculate the base dissociation constant (Kb) for the base as follows -

It is known that:pH + pOH = 14

Explanation

Calculate the Kb for Hydroxylamine base.

Given data

The pH of Hydroxylamine base is 9.11

The concentration of Hydroxylamine base is 0.025M

Calculate the base dissociation constant (Kb) for the base as follows -

It is known that:pH + pOH = 14

pOH = 14 - pH =14 - 9.11=4.89

Therefore, [OH] can be calculated as:

pOH=log[OH]4.89=log[OH][OH]=1.3×105M

The ICE Table for the dissociation of hydroxylamine base is represented as below:

EquilibriumNH2OH(aq)+H2O(l)NH3OH+(aq)+OH(aq)Initial(M)0.02500Change(M)x+x+xEquilibrium(M)0

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