1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6.
2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid?
3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka)
4) An unknown weak base solution with a concentration of 0.187 M has a pH of 13.87. What is the Kb value for this weak base?
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown...
(a) Determine the Kb of a weak base if a 0.847 M aqueous solution of the base at 25°C has a pH of 10.88. (Enter your answer in scientific notation.) (b) Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH 5.19 at 25°C. (c) Calculate the pH of a 0.011 M NaF solution. (Ka for HF = 7.1 × 10−4.)
An unknown weak acid with a concentration of 0.078 M has a pH of 1.80. What is the Ka of the weak acid? O of 1 point earned 2 attempts remaining An unknown weak base with a concentration of 0.170 M has a pH of 9.96. What is the Kb of this base? O of 1 point earned 2 attempts remaining
If a buffer solution is 0.270 M in a weak base (Kb = 4.7 x 10-5) and 0.480 M in its conjugate acid, what is the pH? - pH = L pH=
A 0.135 M solution of a weak base has a pH of 11.26. Determine Kb for the base.
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
2. The pH of a 1.79 M solution of a weak base B is measured to be 11.64 Determine Kb of the base Determine Ka of the weak bases's conjugate acid, HB+ Determine [H+] in a 2.00 M solution of the chloride salt, HBCl M Determine the pH of a 2.00 M solution of the chloride salt, HBCl
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+(aq) + A'(aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, Ka? Answer in scientific notation. Answer: A...
A 0.150 M solution of a weak base has a pH of 11.22. Determine Kb for the base. Express your answer using two significant figures.
a. What is the Kb for HC2O4-? b. The pH of a 2.5 M solution of a weak base is 12.68. What is the Kb for this base? c. The pH of a 1.50 M solution of a weak acid is 2.405. What is the Ka for this acid? d. Calcuate the pH of a 1.52 M solution of NH3.
Determine the Kb of a weak base if a 0.52 M solution of the base has a pH of 10.68 at 25°C. Kb = ? × 10 ? (Enter your answer in scientific notation.)