Multiple 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?
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17. Acid and Base Equilibrium
pH of Weak Acids
Back17. Acid and Base Equilibrium
pH of Weak Acids
- Multiple ChoiceWhat is the pH of a 0.1 M solution of acetic acid (CH3COOH) given that its acid dissociation constant (Ka) is 1.8 x 10^-5?
- Open Question
What is the pH of a 3.4x10-8 M HClO4 solution at room temperature?
- Multiple ChoiceCalculate the pH at 25°C of a solution prepared by adding 50.0 mL of 1.60 M NaOH solution to 0.500 L of 0.0850 M HC5H3O3. Furoic acid (HC5H3O3) has a Ka value of 6.76×10⁻⁴ at 25°C.
- Multiple ChoiceCalculate the pH of a 0.03 M aqueous solution of a weak acid, HA, that has a pKa of 3.39.
- Open Question
Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.
- Multiple ChoiceWhat 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)
- Multiple ChoiceCalculate the pH of a 0.03 M aqueous solution of a weak acid, HA, with a pKa of 3.39.
- Multiple ChoiceCalculate the pH of a 0.300 M NaHCOO solution, given that the Ka for HCOOH is 1.8 x 10^-4.
- Open Question
Calculate the percent ionization of 1.45 m aqueous acetic acid
- Multiple ChoiceFind the pH of a solution that is 9.0×10⁻² M in H₂CO₃. Express your answer using two decimal places.
- Open Question
Calculate [H3O+], [ClO4–], and [OH–] in an aqueous solution that is 0.130 M in HClO4(aq) at 25 °C.
- Open Question
What is the pH of a 0.0620 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-10)?
- Multiple ChoiceWhat is the pH of a solution that is 8.0 × 10⁻² M in H₂CO₃, given that the first dissociation constant (Ka1) of H₂CO₃ is 4.3 × 10⁻⁷?
- Multiple ChoiceA particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar contains, what is the concentration of acetic acid in the vinegar?