Multiple Choice
What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Calculate the pH of a 0.10 M HNO3 solution and a 5.0 × 10^-2 M NaOH solution.
A
pH of HNO3 is 2.0; pH of NaOH is 12.7
B
pH of HNO3 is 1.0; pH of NaOH is 13.7
C
pH of HNO3 is 2.0; pH of NaOH is 13.0
D
pH of HNO3 is 1.0; pH of NaOH is 12.7
Verified step by step guidance1
Identify the nature of the solutions: HNO3 is a strong acid and NaOH is a strong base. This means they completely dissociate in water.
For the HNO3 solution, use the formula for pH: \( \text{pH} = -\log[\text{H}^+] \). Since HNO3 is a strong acid, the concentration of \( \text{H}^+ \) ions is equal to the concentration of the acid, which is 0.10 M.
Calculate the pH of the HNO3 solution by substituting the concentration into the pH formula: \( \text{pH} = -\log(0.10) \).
For the NaOH solution, use the formula for pOH: \( \text{pOH} = -\log[\text{OH}^-] \). Since NaOH is a strong base, the concentration of \( \text{OH}^- \) ions is equal to the concentration of the base, which is 5.0 \times 10^{-2} \text{ M}.
Calculate the pOH of the NaOH solution by substituting the concentration into the pOH formula: \( \text{pOH} = -\log(5.0 \times 10^{-2}) \). Then, use the relationship \( \text{pH} + \text{pOH} = 14 \) to find the pH of the NaOH solution.
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