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Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters

pH of Strong Acids and Bases

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Sections
Acids Introduction
Bases Introduction
Binary Acids
Oxyacids
Bases
Amphoteric Species
Arrhenius Acids and Bases
Bronsted-Lowry Acids and Bases
Lewis Acids and Bases
The pH Scale
Auto-Ionization
Ka and Kb
pH of Strong Acids and Bases
Ionic Salts
pH of Weak Acids
pH of Weak Bases
Diprotic Acids and Bases
Diprotic Acids and Bases Calculations
Triprotic Acids and Bases
Triprotic Acids and Bases Calculations
Conjugate Acids and Bases

The pH of Strong Acids and Bases is determined by their H+ and OH concentrations

pH of Strong Acids and Bases

Concept #1: Strong Acids and Bases represent strong electrolytes.

Example #1: If the concentration of Ba(H)solution is 0.398 M, calculate its pOH.

Practice: An aqueous solution of HBrO4 has a pH of 4.34. Find the molar concentration of HBrO4 solution.

Practice: Calculate the pH of a 25 mL of 5.45 × 102 M LiOH solution.

Practice: HI is a strong acid (Ka = 3.2 × 109). Calculate [H+], [OH], pH and pOH of a 7.1 × 102 M HI solution.