   Chapter 16, Problem 89GQ

Chapter
Section
Textbook Problem

Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?

Interpretation Introduction

Interpretation:

The balanced equation for the acid-base reaction has to be written and the equilibrium lie towards the products or the reactants has to be identified.

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

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.

Explanation

The balanced equation for the acid-base reaction is written below,

H2S(aq) + CH3COO-(aq) CH3COOH(aq) + HS-(aq).

H2S and NaCH3CO2 both are mixed in the water. NaCH3CO2 is dissociates into Na+ and CH3COO-. Na+ is stronger anion therefore, there is no effect for the PH of the solution. Therefore, it is does not involve in the equilibrium reaction.

Acetate ion (CH3COO-) react with H2S, the equilibrium chemical reaction is as follows

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