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: What is the [OH-] in a solution that has a pH of 11.70?a. 5.0x10-3 Mb. 2.0x10-12 Mc. 1.0x10-7 Md. 2.0x102 Me. 5.0x1011 M

Problem

What is the [OH-] in a solution that has a pH of 11.70?

a. 5.0x10-3 M
b. 2.0x10-12 M
c. 1.0x10-7 M
d. 2.0x102 M
e. 5.0x1011 M

Solution

We’re being asked to calculate [OH-] in a solution that has a pH of 11.70.


The OH- concentration can be calculated from pOH using the following equation:

OH-=10-pOH


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

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