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: Given the following values of pK, which is the weakest base of those listed in the answers?pKb of NH3 = 4.75pKa of HNO2 = 3.37pKb C5H5NH = 8.75pKa of HBrO = 8.69pKa of HClO = 7.53

Problem

Given the following values of pK, which is the weakest base of those listed in the answers?

pKof NH= 4.75

pKa of HNO2 = 3.37

pKb C5H5NH = 8.75

pKa of HBrO = 8.69

pKa of HClO = 7.53

Solution

We're being asked to identify the weakest base based on the given pK values.

Ka represents the acid dissociation constant and it measures the strength of weak acids. In general:

• The higher the Ka the stronger the acid and the greater the concentration of H+

pKa is the negative base-10 logarithm of the base dissociation constant (Ka) of a solution.

• The lower the pKa, the stronger the acid

Kb represents the base dissociation constant and it measures the strength of weak bases. In general:

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