   Chapter 16, Problem 42PS

Chapter
Section
Textbook Problem

Equal molar quantities of hydrochloric acid and sodium hypochlorite (NaClO) are mixed. (a) Write the balanced, net ionic equation for the acid-base reaction that can, in principle, occur. (b) Does the equilibrium lie to the right or left?

(a)

Interpretation Introduction

Interpretation: The balanced, net ionic equation is to be written for the mixture of HCl and NaClO.

Concept introduction:

Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side.

Steps in balancing the information

• Step 1: Write the unbalanced equation
• Step 2: Find the coefficient to balance the equation.
• The coefficient should be reduced to the smallest whole number
Explanation

When HCl and NaClO are mixed in equal molar concentration. The HCl dissociates completely into its ions H+ and Cl as it is a strong acid. The ClO ion from NaClO will combine with H+ and forms HOCl.

The net ionic balanced reaction between HCl and NaClO is written as,

HCl(aq) +  ClO(aq)     &

(b)

Interpretation Introduction

Interpretation: The direction of the equilibrium for the given reaction is to be determined.

Concept introduction: An acid-base reaction reaction is represented as written below.

HA(aq)+B(aq)   BH+(aq)  +    A(aq)(acid)    (base)        (conjugate     acid)   (conjugate     base)

The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants (Kaand Kb) for reactants as well as of the products. The more the value of Ka for an acid, stronger will be the acid and it will undergo faster ionization. Similarly, higher the value of Kb for a base, stronger will be the base and it will undergo faster ionization.

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