Question

(a) Calculate the percent ionization of 0.00260 M carbonic acid
(K_{a} = 4.3e-07).

% ionization = .003344 %

(b) Calculate the percent ionization of 0.00260 M carbonic acid in
a solution containing 0.0110 M sodium hydrogen carbonate.

% ionization = .00001018 %

these were my answers and both are incorrect! Please Help!

Answer #1

(a) Calculate the percent ionization of 0.00250 M acetic acid
(Ka = 1.8e-05).
% ionization = %
(b) Calculate the percent ionization of 0.00250 M acetic acid in
a solution containing 0.0110 M sodium acetate.
% ionization = %

(a) Calculate the percent ionization of 0.00360 M hypobromous
acid (Ka = 2.5e-09).
% ionization = ________%
(b) Calculate the percent ionization of 0.00360 M hypobromous
acid in a solution containing 0.0260 M sodium hypobromite.
% ionization = _________%

(a) Calculate the percent ionization of 0.00840 M hypochlorous
acid (Ka = 3e-08). % ionization = % (b) Calculate the percent
ionization of 0.00840 M hypochlorous acid in a solution containing
0.0190 M sodium hypochlorite. % ionization = %

(a) Calculate the percent ionization of 0.00230 M butanoic acid
(Ka = 1.5e-05). % ionization=
(b) Calculate the percent ionization of 0.00230 M butanoic acid
in a solution containing 0.0510 M sodium butanoate. % ionization
=

A. Calculate the percent ionization of 8.0×10−3 M butanoic acid
(Ka=1.5×10−5) B. Calculate the percent ionization of 8.0×10−3 M
butanoic acid in a solution containing 8.0×10−2 M sodium
butanoate.

Calculate the percent ionization of 0.130 M lactic acid
(Ka=1.4×10−4). Calculate the percent ionization of 0.130 M lactic
acid in a solution containing 7.0×10−3 M sodium lactate. Calculate
the pH of a buffer that is 0.200 M in NaHCO3 and 0.280 M in Na2CO3.
Calculate the pH of a solution formed by mixing 65 mL of 0.35 M
NaHCO3 with 75 mL of 0.23 M Na2CO3.

The Ka of a monoprotic weak acid is 2.29 × 10-3. What is the
percent ionization of a 0.129 M solution of this acid? I got 104.8%
which I know is impossible.
The Ka value for acetic acid, CH3COOH(aq), is 1.8× 10–5.
Calculate the pH of a 2.40 M acetic acid solution.
I also got these incorrect, but am not sure why and would like
to understand. Please help me understand these before my upcoming
test! Thanks! Calculate the pH...

calculate the percent ionization of a 0.600 M solution of the
monoprotic acetylsalicyclic acid (aspirin). (ka=3.0 x10 ^-4)

Calculate the percent ionization of 0.120 M lactic acid in a
solution containing 7.0×10−3 M sodium lactate.

A certain weak acid, HA, has a Ka value of 4.6×10−7.
A) Calculate the percent ionization of HA in a 0.10 M
solution.
B) Calculate the percent ionization of HA in a 0.010 M
solution.

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