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pH Calculations Practice Questions & Answers (A+ Prep 2025–2026), Exams of Chemistry

Texas State UniversityChemistry

This set of pH calculation questions focuses on using key formulas such as pH = −log[H⁺], pOH = −log[OH⁻], and pH + pOH = 14. Practice includes finding pH from hydrogen ion concentration, determining [H⁺] from pH, and calculating pOH and hydroxide levels. Correct answers apply logarithm rules and show step-by-step reasoning for accuracy. These problems strengthen understanding of acids, bases, and neutral solutions, helping students achieve A+ performance in chemistry exams

Typology: Exams

2025/2026

Available from 07/02/2026

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PH CALCULATIONS PREP
QUESTIONS AND
CORRECT ANSWERS
GRADED A+ 2025-2026
Determine the pH of a 0.010 M HNO₃ solution. - ANS-pH = 2
What is the pH of a 2.5x10⁻⁶ M solution of HCl? - ANS-pH = 5.6
Calculate the pH of a solution of 0.0025 M H₂SO₄. - ANS-pH = 2.6
Calculate the pH of a 0.0010 M NaOH solution. - ANS-pH = 11
What is the pH of a 0.020 M Sr(OH)₂ solution? - ANS-pH = 12.3
What is the hydrogen ion concentration of an aqueous HCl solution that has a pH of
3.0? - ANS-[H⁺] = 0.001 M
What is the hydroxide ion concentration of an aqueous HCL solution that has a pH of
3.0? - ANS-[OH⁻] = 1x10⁻¹¹ M
Find the [H⁺] and the [OH⁻] of a solution with a pH of 3.494. - ANS-[H⁺] = 3.2 x 10⁻⁴ M
[OH⁻] = 3.1 x 10⁻¹¹ M
Calculate [H⁺] of a solution whose [OH⁻] = 1x10⁻⁵ M. - ANS-[H⁺] = 1x10⁻⁹ M
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PH CALCULATIONS PREP

QUESTIONS AND

CORRECT ANSWERS

GRADED A+ 2025- 2026

Determine the pH of a 0.010 M HNO₃ solution. - ANS-pH = 2 What is the pH of a 2.5x10⁻⁶ M solution of HCl? - ANS-pH = 5. Calculate the pH of a solution of 0.0025 M H₂SO₄. - ANS-pH = 2. Calculate the pH of a 0.0010 M NaOH solution. - ANS-pH = 11 What is the pH of a 0.020 M Sr(OH)₂ solution? - ANS-pH = 12. What is the hydrogen ion concentration of an aqueous HCl solution that has a pH of 3.0? - ANS-[H⁺] = 0.001 M What is the hydroxide ion concentration of an aqueous HCL solution that has a pH of 3.0? - ANS-[OH⁻] = 1x10⁻¹¹ M Find the [H⁺] and the [OH⁻] of a solution with a pH of 3.494. - ANS-[H⁺] = 3.2 x 10⁻⁴ M [OH⁻] = 3.1 x 10⁻¹¹ M Calculate [H⁺] of a solution whose [OH⁻] = 1x10⁻⁵ M. - ANS-[H⁺] = 1x10⁻⁹ M

Calculate [OH⁻] of a solution whose [H⁺] = 1x10⁻² M. - ANS-[OH⁻] = 1x10⁻¹² M Calculate [H⁺] of a solution whose [OH⁻] = 2.5x10⁻⁴ - ANS-[H⁺] = 4x10⁻¹¹ M Calculate [OH⁻] of a solution whose [H⁺] = 0.00375 M. - ANS-[OH⁻] = 2.67x10⁻¹² M Calculate the pH of a solution whose [H⁺] = 1x10⁻⁶ M. - ANS-pH = 6 Calculate the pH of a solution whose [H⁺] = 9.65x10⁻³ M. - ANS-pH = 2. Calculate the [H⁺] of a solution whose pH = 2.68. - ANS-[H⁺] = 2.1x10⁻³ M Calculate the [H⁺] of a solution whose pH = 11.93. - ANS-[H⁺] = 1.17x10⁻¹² M Calculate the pOH of a solution whose [OH⁻] = 1x10⁻¹¹ M. - ANS-pOH = 11 Calculate the pOH of a solution whose [OH⁻] = 7.24x10⁻³ M. - ANS-pOH = 2. Calculate the [OH⁻] of a solution whose pOH = 4.00. - ANS-[OH⁻] = 1x10⁻⁴ M Calculate the [OH⁻] of a solution whose pOH = 1.14. - ANS-[OH-] = 0.072 M Calculate the pOH of a solution whose pH = 6.00. - ANS-pOH = 8. Calculate the pOH of a solution whose pH = 9.78. - ANS-pOH = 4. Calculate the pH of a solution whose pOH = 12.00 - ANS-pH = 2. Calculate the pH of a solution whose pOH = 3.88. - ANS-pH = 10.