# Assume a solution with a total alkalinity of 1.00 × 10 −3 eq/L. (a) Define the concentrations of the H 2 CO 3 , bicarbonate, carbonate, and hydroxide ions at pH 7.00. (b) Now define the concentrations of the bicarbonate, car bonate, and hydroxide tons at pH 10.00. (Recall that for the carbonate equilibrium is 4.8 × 10 −11 .) HCO 3 − (aq) + H,O(ℓ) ⇄ CO 3 2− (aq) + H 3 O + (aq)

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

Chapter
Section

### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 20.7, Problem 1Q
Textbook Problem
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## Assume a solution with a total alkalinity of 1.00 × 10−3 eq/L. (a) Define the concentrations of the H2CO3, bicarbonate, carbonate, and hydroxide ions at pH 7.00. (b) Now define the concentrations of the bicarbonate, car bonate, and hydroxide tons at pH 10.00. (Recall that for the carbonate equilibrium is 4.8 × 10−11.) HCO3− (aq) + H,O(ℓ) ⇄ CO32− (aq) + H3O+(aq)

Interpretation Introduction

Interpretation: It should be defined for the concentration of various hydroxide a ta certain pH value.

Concept Introduction: Alkalinity of a water supply is its capacity to accept hydronium ions.

This factor is important to known when assessing water quality, methods of water treatment, and the biology of natural water because the amount of biomass that can be produced depends on the alkalinity.’

Alkanity (Alk) is defined by the equation

Alk = [HCO3-]+2[CO32-]+[OH-]

### Explanation of Solution

Given;

[Alk ]= 1.00×10-3

At pH=7.0

[CO32-]

[OH-]=1.0×10-7M

[Alk ]= 1.00×10-3[HCO3-] +2(0)+(1.00×10-7)

Solving for [HCO3-]= 1.00×10-3M

H2CO3(aq)+H2O(l)  HCO3-(aq)+H3O+(aq)

[H2CO3]=2.4×10-4M

Given,

The concentration  of. H2CO3 Bicarbonate, carbonate and hydroxide ions at pH=7.00

(b)

Given,

The concentration  of. H2CO3 Bicarbonate, carbonate and hydroxide ions at pH=10

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