Multiple Choice
What is the pH of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of solution? (Ka = 1.8 × 10⁻⁵)
17. Acid and Base Equilibrium
pH of Weak Acids
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the pH of the buffer prepared by mixing 200 mL of 0.15 M HNO2 (Ka = 4.0 x 10^-4) and 150 mL of 0.10 M sodium nitrite?
A
3.35
B
2.85
C
3.75
D
4.25
Verified step by step guidance1
Calculate the moles of HNO2 by multiplying its concentration (0.15 M) by its volume (200 mL converted to liters).
Calculate the moles of sodium nitrite (NaNO2) by multiplying its concentration (0.10 M) by its volume (150 mL converted to liters).
Use the Henderson-Hasselbalch equation to find the pH of the buffer: \( \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \( \text{pKa} = -\log(\text{Ka}) \).
Substitute the calculated moles of \( \text{A}^- \) (sodium nitrite) and \( \text{HA} \) (HNO2) into the Henderson-Hasselbalch equation.
Solve the equation to find the pH of the buffer solution.
0:44mWatch next
Master ICE Charts of Weak Acids with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
pH of Weak Acids practice set
Problem sets built by lead tutorsExpert video explanations