Multiple Choice
What is the pH of a solution made by mixing 25.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
Calculate the pH of a mixture of 150.0 mL of 0.0150 M HNO3 (aq) and 100.0 mL of 0.0100 M HBr (aq), assuming volumes are additive.
A
1.40
B
2.00
C
1.80
D
1.60
Verified step by step guidance1
First, understand that both HNO3 and HBr are strong acids, meaning they dissociate completely in water. Therefore, the concentration of hydrogen ions [H⁺] from each acid will be equal to the initial concentration of the acid.
Calculate the moles of H⁺ ions contributed by HNO3. Use the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). For HNO3, this is \( 0.0150 \text{ M} \times 0.150 \text{ L} \).
Calculate the moles of H⁺ ions contributed by HBr using the same formula: \( \text{moles} = \text{concentration} \times \text{volume} \). For HBr, this is \( 0.0100 \text{ M} \times 0.100 \text{ L} \).
Add the moles of H⁺ ions from HNO3 and HBr to find the total moles of H⁺ ions in the mixture.
Calculate the total volume of the mixture by adding the volumes of HNO3 and HBr solutions. Then, find the concentration of H⁺ ions in the mixture by dividing the total moles of H⁺ by the total volume. Finally, use the formula \( \text{pH} = -\log[\text{H}^+] \) to find the pH of the solution.
Related Videos
Related Practice
