1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid?
pOH =
2. What is the pH of an aqueous solution of
1.77×10-2 M nitric
acid?
pH =
3. What is the pOH of an aqueous solution of
3.08×10-2 M potassium
hydroxide?
pOH =
4. What is the pH of an aqueous solution of
3.08×10-2 M potassium
hydroxide?
pH =
5. Calculate the pH of a 0.409 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).
6. Calculate the pH of a 0.0130 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4).
7. Calculate the pH of a 0.409 M aqueous solution of morphine (C17H19O3N, Kb = 7.4×10-7).
pH =
8. Calculate the pH of a 0.0237 M aqueous
solution of triethylamine
((C2H5)3N,
Kb = 5.2×10-4).
pH =
9. Calculate the percent ionization of a
0.347 M solution of formic
acid, HCOOH.
% Ionization=
1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid? pOH =...
#6a What is the pOH of an aqueous solution of 0.289 M hydrobromic acid? pOH = 6B- What is the pH of an aqueous solution of 2.92×10-2 M hydrobromic acid? pH = 6C- What is the hydronium ion concentration in an aqueous nitric acid solution with a pH of 3.740? __ [H3O+] = M
What is the pOH of an aqueous solution of .243 M hydrochloric acid? What is the pH of an aqueous solution of 2.47x10^-2 M perchlorate acid? What is the pH of an aqueous solution of 4.37x10^-2 M potassium hydroxide?
What is the percent ionization of a 0.205 M aqueous solution of formic acid? Ka (HCOOH) = 1.7x10-4
What is the percent ionization of a 0.213 M aqueous solution of formic acid? Ka (HCOOH) = 1.7x10-4
Calculate the pH of a 0.0140 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4). pH =
1) The pH of an aqueous solution at 25°C was found to be 13.00. The pOH of this solution is ___ The hydronium ion concentration is ____M. The hydroxide ion concentration is ____M. 2) The hydronium ion concentration in an aqueous solution at 25°C is 3.6×10-2M. The hydroxide ion concentration is M. The pH of this solution is ____. The pOH is _____ . 3) What is the pOH of an aqueous solution of 0.467 M hydrochloric acid? pOH = ___...
What is the  percent ionization of a 0.461 M aqueous solution of formic acid? Ka (HCOOH) = 1.7x10-4
1. Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7). pH = 2. Calculate the pH of a 0.1250 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3). pH = 3. Calculate the pH of a 0.0774 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb = 5.20×10-4). pH =
Salt of a Weak Base and a Strong Acid. pH of Solution. Calculate the pH of a 1.19 M aqueous solution of triethylamine hydrochloride ((C2H5)3NHCI) (For triethylamine, (C2H5)3N, Kb = 4.00x 10-4.) Give two decimal places in your answer.
Calculate the pH, pOH, [H3O +] and [OH-] and formic acid (HCOOH) in a 0.0500M formic acid solution (Ka formic acid: 2.1x 10 –4).