Multiple Choice
Which is the correct form of the Henderson-Hasselbalch equation?
18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
Back18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
- Multiple Choice
The Kb of C6H5NH2 (aniline) is 3.9 × 10−10. Determine pH of a buffer solution made up of 500 mL of 1.4 M C6H5NH2 and 230 mL of 2.3 M C6H5NH3+.
- Multiple Choice
Determine the buffer component concentration ratio (CB/WA) for a buffer with a pH of 4.7. Ka of boric acid (H3BO3) is 5.4 × 10−10.
- Multiple Choice
Calculate mass of NaN3 that needs be added to 1.8 L of 0.35 M HN3 in order to make a buffer with a pH of 6.5. Ka of hydrazoic acid is 1.9 × 10−5.
- Multiple Choice
Which of the following weak acid-conjugate base combinations would result in an ideal buffer solution with a pH of 9.4?
a) formic acid (HCHO2) and sodium formate (Ka = 1.8 x 10-4)
b) benzoic acid (HC7H5O2) and potassium benzoate (Ka = 6.5 x 10-5)
c) hydrocyanic acid (HCN) and lithium cyanide (Ka = 4.9 x 10-10)
d) iodic acid (HIO3) and sodium iodate (Ka = 1.7 x 10-1)
- Open Question
buffer 2: 50.0 mL of 0.18 M NH3 with 5.0 mL of 0.36 M HBr.
- Open Question
What is the pH of a solution of 0.300 M HNO2 containing 0.100 M NaNO2? (Ka of HNO2 is 4.5 × 10–4)
- Open Question
What is the ratio of [A–]/[HA] at pH 5.75? The pKa of formic acid (methanoic acid, H–COOH) is 3.75.
- Open Question
What ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (Ka of HCN is 4.9 × 10-10)
- Open Question
How much more acetic acid (pKa = 4.76) than acetate should be in solution to maintain a pH of 4.00?
- Open Question
Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 m HBrO (Ka = 2.5 × 10-9)
- Multiple ChoiceA 1.0 L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8 × 10⁻⁵. Calculate the pH of the solution upon the addition of 0.015 mol of NaOH to the original buffer.
- Multiple ChoiceA 1.0 L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10⁻⁵. Calculate the pH of the solution upon the addition of 10.0 mL of 1.00 M HCl to the original buffer using the Henderson-Hasselbalch equation.
- Multiple ChoiceA 270.0 mL buffer solution initially contains 3.0×10⁻² M of HCHO₂ and 3.0×10⁻² M of NaCHO₂. To adjust the buffer pH to 4.10, should you add NaOH or HCl to the buffer mixture?
- Multiple ChoiceA buffer consists of 0.120 M HNO2 and 0.150 M NaNO2 at 25 °C. The pKa of HNO2 is 3.40. What is the pH of the buffer?