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: Determine the pH of each solution.a solution that is 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl

Solution: Determine the pH of each solution.a solution that is 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl

Problem

Determine the pH of each solution.

a solution that is 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl

Solution

We are asked to calculate the pH of the solution with 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl.


The pH of a compound determines its acidity.

 pH

▪ pH stands for the negative logarithmic function of hydronium ion concentration
can be calculated using the following equation:

pH=-log H3O+


Strong acids are considered strong electrolytes. They completely dissociate into ions when dissolved in water.

Strong binary acids – paired with a highly electronegative atom

Strong binary acids are:              HCl, HBr, and HI

Strong oxyacids (or oxoacids) - have 2 or more oxygens than hydrogens

Oxyacids → possess H+ ion, connected to nonmetal and oxygen

Common strong oxyacids are:                  HNO3, HClO3, HClO4, H2SO4

Exceptions to the rule are:                            Oxalic acid (H2C2O4) and Iodic acid (HIO3)

▪ both have 2 more O than H but are weak acids because carbon and iodine have low electronegativity


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