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: Calculate the hydronium ion concentration for a solution with a pH of 6.8.(A) 6.3 × 10−8(B) 1.6 × 10−7(C) 6.8 M (D) 0.83 M (E) 6.3 × 106 M

Problem

Calculate the hydronium ion concentration for a solution with a pH of 6.8.

(A) 6.3 × 10−8

(B) 1.6 × 10−7

(C) 6.8 M 

(D) 0.83 M

 (E) 6.3 × 106 M

Solution

Establish the related equations for pH and [OH-] then calculate the concentration of OH- using the provided pH 

The pH and pOH of a compound determine its acidity and basicity.

• pOH

▪ pOH stands for the negative logarithmic function of hydroxide concentration
can be calculated using the following equation:

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