   Chapter 14, Problem 159AE

Chapter
Section
Textbook Problem

# Is an aqueous solution of NaHSO4 acidic, basic, or neutral? What reaction occurs with water? Calculate the pH of a 0.10-M solution of NaHSO4.

Interpretation Introduction

Interpretation: The nature of the given aqueous solution of NaHSO4; its reaction with water and the pH value of 0.10M solution of NaHSO4 is to be stated.

Concept introduction: Weak acids dissociate up to a small extent and furnish limited number of protons in an aqueous solution. Major species present in a given solution determine the pH of the solution.

To determine: The nature of the given aqueous solution of NaHSO4 its reaction with water and the pH value of solution of 0.10MNaHSO4

Explanation

Explanation

The aqueous solution of NaHSO4 is acidic in nature.

The dissociation reaction of NaHSO4 is.

NaHSO4Na++HSO4.

The aqueous solution contains Na+ and HSO4 as the major species. The cation Na+ is neither an acid nor a base. The anion HSO4 is the conjugate base of H2SO4 but it also capable of releasing H+ ions. Therefore, it can be termed as a weak acid.

Therefore, the aqueous solution of NaHSO4 is weakly acidic in nature.

Upon reaction with water, HSO4 further dissociates to give a proton.

The reaction of HSO4 with water is,

HSO4+H2OH3O++SO4

This step is reversible in nature and has very low rate of dissociation.

The [H+] concentration in the aqueous solution is 3.0×10-2_.

The reaction of HSO4 with water is,

HSO4+H2OH3O++SO4

The ICE (Initial Change Equilibrium) table is formed for the above stated reaction.

HSO4+H2OH3O++SO42Initial(M):0.1000Change(M):xxxEquilibrium(M):0.10xxx

The equilibrium constant expression for the above stated reaction,

Ka=[SO42][H3O+][HSO4]

The standard Ka value of HSO4 is 1

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