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 the [H3O+] of each aqueous solution with the following [OH-].Part A         NaOH, 1.0 x 10 -2 M         Express your answer using two significant figures.Part B          milk of magnesia, 1.

Solution: Calculate the [H3O+] of each aqueous solution with the following [OH-].Part A         NaOH, 1.0 x 10 -2 M         Express your answer using two significant figures.Part B          milk of magnesia, 1.

Problem

Calculate the [H3O+] of each aqueous solution with the following [OH-].

Part A

         NaOH, 1.0 x 10 -2 M

         Express your answer using two significant figures.


Part B

          milk of magnesia, 1.2 x 10 -5

          Express your answer using two significant figures.



Solution

A) Since NaOH is a strong base, it will dissociate completely in the solution. This means that the concentration of hydroxide ions after dissociation will be the same as the initial concentration of NaOH. [H3O+] can be calculated using the ion-product constant of water (kw) and [OH-

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