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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4. Calculate the pH you would expect for a 0.15 M aqueous solution of each substance. - nitric acid - ascorbic acid - lithium hydroxide - methylamine (see Table 15.4, p. 682) I 5. Consider your work on the ascorbic acid solution in the previous problem. What would the equilibrium concentration of the conjugate (ascorbate, C,H;O6) be in the solution?
Solve, (a) At any instant, how many water molecules are ionized in 1 L of pure water at pH 7.0? (b) Express this number as a percentage of the total water molecules.
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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Chemistry & Chemical Reactivity

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