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: Find the pH of each mixture of acids.1.5×10−2 M in HBr and 2.0×10−2 M in HClO4

Solution: Find the pH of each mixture of acids.1.5×10−2 M in HBr and 2.0×10−2 M in HClO4

Problem

Find the pH of each mixture of acids.

1.5×10−2 M in HBr and 2.0×10−2 M in HClO4

Solution

In this problem, we are asked to find the pH of a mixture of acids.


Remember that HClO4 and HBr are strong, monoprotic oxyacid.

Recall that strong acids completely dissociate in water and that acids donate H+ to the base (water in this case). 


The dissociation of HClO4 is as follows:


HClO4(aq) + H2O(l)  H3O+(aq) + ClO4(aq)



The dissociation of HBr is as follows:


HBr(aq) + H2O(l)  H3O+(aq) + Br(aq)


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