Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Determine the pH of each of the following solutions.0.21 M KCHO2

Solution: Determine the pH of each of the following solutions.0.21 M KCHO2

Problem

Determine the pH of each of the following solutions.

0.21 M KCHO2

Solution

We are being asked to calculate the pH of 0.21 M KCHO2.


KCHO2 is an ionic compound and will break up into its ions in the solution:

KCHO2(aq)  K+(aq) + CHO2-

• main group metals should have a +3 charge or higher to be considered acidic. K+ has only a +1 charge and is a neutral ion so it will not contribute to the pH of the solution

• CHO2- is the conjugate base of the weak acid CHO2H

CHO2H(aq)   +   H2O(l)       CHO2-(aq)   +    H3O+(aq)                     Ka = 1.8x10-4           
(weak acid)                        (conjugate base)

      **Ka value can be found in books or online sources


CHO2- also acts as weak base and can ionize in the solution to form the weak acid

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