Multiple Choice
Consider 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 the addition of 30.0 mL of 1.0 M HCl to the original buffer solution.
18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
Back18. Aqueous Equilibrium
Henderson-Hasselbalch Equation
- Multiple ChoiceUsing the Henderson-Hasselbalch equation, what is the pH of a buffer solution that is 0.250 M in HCN and 0.170 M in KCN, given that the pKa of HCN is 9.31?
- 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.
2views - Multiple ChoiceA buffer solution has 0.625 M HCN and 0.575 M CN⁻. If 0.030 mol of HCl is added to 400. mL of the buffer solution, what is the pH after the addition? The pKa of hydrocyanic acid is 9.23.
- Multiple ChoiceWhat is the pH of a buffer system that has 0.25 M HCN and 0.38 M CN⁻, given that the pKa of hydrocyanic acid is 9.23?
- 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)
1views - Multiple ChoiceWhat mass of CH3COONa must be added to create 300.0 mL of a buffer solution with a pH of 5.00 and a CH3COOH concentration of 0.100 M? The pKa of acetic acid is 4.75.1views
- Multiple ChoiceWhat is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10^-5 for CH3CO2H.
- Open Question
buffer 2: 50.0 mL of 0.18 M NH3 with 5.0 mL of 0.36 M HBr.
1views - 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)
- Multiple ChoiceWhat mass of KNO2 must be added to create 200.0 mL of a buffer solution with a pH of 3.00 and an HNO2 concentration of 0.150 M? The pKₐ of nitrous acid is 3.34.1views
- 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 ChoiceUsing the Henderson-Hasselbalch equation, what is the pH of a buffer system that contains 0.87 M dimethylamine ((CH3)2NH) and 0.68 M dimethylammonium ion ((CH3)2NH2+)? The Kb of dimethylamine is 5.9 × 10⁻⁴.
- 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.