   Chapter 16, Problem 43PS

Chapter
Section
Textbook Problem

Equal molar quantities of acetic acid and sodium hydrogen phosphate (Na2HPO4) are mixed. (a) Write a 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 CH3COOH and Na2HPO4.

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 CH3COOH and Na2HPO4 are mixed in equal molar concentration. The CH3COOH dissociates faster into its ions H+ and CH3COO as it is a stronger acid compared to the conjugate acid ( H2PO4). The HPO42 ion from Na2HPO4 will combine with H+ and forms   H2PO4.

The net ionic balanced reaction between CH3COOH and Na2HPO4 is written as,

CH3

(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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