Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 20.7, Problem 2Q
Interpretation Introduction

Interpretation: It should be defined for the concentration of various hydroxides at a certain pH value. With showing the dissolved Carbon values

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-]

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1.Calculate the ratio of conjugate base/ weak acid at pH 9.3. Show all details of your working out for each individual mathematical manipulation that you apply In each step of your working out use the chemical formulas of the compounds that constitute the weak acid and conjugate base. Provide the answer to 3 decimal places, make sure to round the result accordingly. State the final answer in a complete sentence. 2.Calculate the concentration of the weak acid and conjugate base for a total buffer concentration of 150 mM at pH 9.3. Show all details of your working out for each individual mathematical manipulation that you do apply . In each step of your working out use the chemical formulas of the compounds that constitute the weak acid and conjugate base. Provide the final answer to 3 decimal places using the unit molar ‘M’, make sure to round the result accordingly. State the final answer in a complete sentence. HCO3- (aq) ------->  CO32- (aq) + H+    pKa= 10.2
If the pH of a solution is increased from pH 5 to pH 7, it means that the: (please select one correct option below) the concentration of OH-is one-hundredth what it was at pH 5. the concentration of H+ is twice what it was at pH5. The concentration of H+is 100 times greater and the concentration of OH+ is one-hundredth what they were at pH 5. the concentration of H+ is one-half what it was at pH 5. the concentration of OH- is 100 times greater than what it was at pH 5 and the concertation of H+ is one-hundredth what they were in pH 5.

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