   Chapter 14, Problem 55GQ

Chapter
Section
Textbook Problem

To determine the concentration dependence of the rate of the reactionH2PO3− (aq) + OH−(aq) → HPO32−(aq) + H2O(ℓ)you might measure [OH−] as a function of time using a pH meter. (To do so, you would set up conditions under which [H2PO3−] remains constant by using a large excess of this reactant.) How would you prove a second-order rate dependence for [OH−]?

Interpretation Introduction

Interpretation:

The second-order rate dependence for OH has to be proved for the given reaction.

Concept Introduction:

Rate order: It is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.

Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

Rate constant: It is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Explanation

The OH concentration for the given reaction is determined by first measuring the pH with respect to function of time. Then using this [OH], the plot of

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