Open Question
The ph of a 1.00 m solution of urea, a weak organic base, is 7.050.
17. Acid and Base Equilibrium
pH of Weak Acids
Back17. Acid and Base Equilibrium
pH of Weak Acids
- Open Question
Calculate the percent ionization of 1.45 m aqueous acetic acid
- Open Question
Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80.
- 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 [H⁺] in a 0.270 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 × 10⁻⁵)?
- Open Question
Nitrous acid, HNO2, has a ka of 7.1 x 10–4. what is the [H3O+] in a 0.60 M solution of HNO2?
- Open Question
What is the pH of a 3.4x10-8 M HClO4 solution at room temperature?
- Open Question
Find the percent ionization of a 0.337 m HF solution. the ka for hf is 3.5 × 10-4. What would you expect the percent ionization to be for the same concentration of hydrochloric acid (HCl)? Explain.
- Multiple ChoiceWhich of the following is the correct pH of a solution formed by mixing 1.3 L of 0.45 M HCl with 5.5 L of 1.95 M HI?
- Multiple ChoiceA 0.10 M HClO(aq) solution is prepared. Calculate the pH of this solution given that the Ka of HClO is 1.58 x 10^-4.
- 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?
- Multiple ChoiceA student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 × 10^-5 at room temperature.) Calculate the initial pH of the acetic acid solution before any NaOH is added.
- Multiple ChoiceAn 8.36 g sample of NH4Cl was added to 26.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L. What is the pH of this buffer solution?
- Multiple ChoiceCalculate the [H3O+] of a 0.115 M H2CO3 solution, given that Ka1 = 4.3 x 10^-7 and Ka2 = 5.6 x 10^-11.
- Multiple ChoiceCalculate the pH of the solution made by adding 0.50 mol of HOBr and 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HOBr is 2.0 × 10⁻⁹. What is the pH of the solution?