Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
All Chapters
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 [OH-] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. A solution in which [H+] is 1000 times greater than [OH-]. Express your answer using two significant figures.
[OH-] = _____ M

Problem

Calculate [OH-] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. 

A solution in which [H+] is 1000 times greater than [OH-]. Express your answer using two significant figures.

[OH-] = _____ M

Solution

We’re being asked to determine the OH- concentration if [H3O+] is 1000 times greater than [OH]


Recall: Kw = 1.0 × 10–14 at 25.0 ˚C.

Kw is the auto-ionization product of water. For the following reaction:


2 H2O(l) H3O+(aq) + OH(aq)


the auto-ionization product constant is given by:



Note that each concentration is raised by the stoichiometric coefficient:[H3O+] and [OH] are raised to 1.


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