Multiple Choice
What is the pH of a solution that is 0.060 M in potassium propionate and 0.085 M in propionic acid, given that the Ka of propionic acid is 1.3 x 10^-5?
17. Acid and Base Equilibrium
pH of Weak Acids
Back17. Acid and Base Equilibrium
pH of Weak Acids
- Multiple ChoiceWhat is the equilibrium constant for the dissociation of a weak base in water?
- Multiple ChoiceWhat is the pH of a buffer solution after adding 0.150 mol of HCl, assuming no volume change?
- Multiple ChoiceWhat is the pH change of a 0.220 M solution of benzoic acid (pKa=4.19) if 0.175 M benzoate is added with no change in volume?
- Multiple ChoiceWhat is the pH of a 0.750 M solution of KH2PO4, considering it is a weak acid?
- Multiple ChoiceWhat is the calculated pH after adding 2.5 mL of 0.5 M NaOH to 50.0 mL of 0.25 M acetic acid, and then adding 1.0 mL of 0.5 M HCl?
- Multiple ChoiceWhat is the calculated pH after adding 2.5 mL of 0.5 M NaOH to 50.0 mL of 0.25 M acetic acid, assuming complete neutralization of the added base?
- Multiple ChoiceWhat is the concentration of H⁺ ions in a 2.0 M solution of acetic acid (HC₂H₃O₂) if the acid dissociation constant (Ka) is 1.8 x 10⁻⁵?
- Multiple ChoiceWhat is the pH of the solution at the halfway point of the titration of acetic acid with sodium hydroxide?
- Multiple ChoiceWhat is the pH of a 0.1 M solution of HF, given that the acid dissociation constant (Ka) for hydrofluoric acid is 7.1 x 10^-4?
- Multiple ChoiceWhat is the pH of a 0.150 M solution of CH3COOH, given that the Ka of CH3COOH is 1.8 × 10⁻⁵?
- Multiple ChoiceWhat is the pH of a 0.200 M CH3NH3Br solution, given that the Kb of CH3NH2 is 4.4 × 10⁻⁴?
- Multiple ChoiceWhat is the pH of a 6.00 M H3PO4 solution, given that Ka1 = 7.5 × 10⁻³, Ka2 = 6.2 × 10⁻⁸, and Ka3 = 4.2 × 10⁻¹³?
- Multiple ChoiceWhat is the pH of a buffer solution that is 0.185 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10^-4.
- Multiple ChoiceWhat is the pH of a mixture of 200 mL of a 0.39 M solution of the weak acid hydronium ion (H₃O⁺) and 250 mL of a 0.62 M solution of hypoiodous acid (HIO, Kₐ = 2.3 × 10⁻¹¹)?