Multiple Choice
Using the Henderson-Hasselbalch equation, what can you conclude about the relative concentrations of CH3NH2 and CH3NH3Cl in a buffer solution where the pH is 10.64 and the pKb of CH3NH2 is 3.36?
18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
Back18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
- Multiple ChoiceWhich of the following correctly represents the Henderson-Hasselbalch equation for a solution of propanoic acid (C2H5COOH) and its conjugate base (C2H5COO^-)?1views
- Multiple ChoiceWhich is the correct form of the Henderson-Hasselbalch equation?2views
- 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+.
15views - Multiple ChoiceConsider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb = 4.75. Calculate the pH of 1.0 L of the solution upon addition of 30.0 mL of 1.0 M HCl to the original buffer solution.
- Multiple ChoiceUsing the Henderson-Hasselbalch equation, what is the pH of a buffer solution containing 0.6 M HF and 0.2 M NaF? The acid dissociation constant, Ka, for HF is 6.8 × 10^{-4}.1views
- 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)
2views - 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.
3views - 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?
- 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 ChoiceUse the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.255 M in CH3NH2 and 0.120 M in CH3NH3Br. The pKa of CH3NH3+ is 10.64.
- Multiple Choice
Which of the following weak acid-conjugate base combinations would result in an ideal buffer solution with a pH of 9.4?
3views - Open Question
How much more acetic acid (pKa = 4.76) than acetate should be in solution to maintain a pH of 4.00?
1views - Multiple ChoiceConsider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb = 4.75. Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of solid NaOH to the original buffer solution.
- 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.
1views