Question

A 0.100 mol/kg solution of the acid HX is found to have 0.00055 mol/kg of H3O+. Find the Ka for this acid.

Answer #1

SOLUTION :

INITIAL CONCENTRATION OF [HX] = X M = 0.1 M

[ H3O+] = 0.00055 M

REACTION :

HX + H2O
H3O+ +

INITIALLY 0.1 M 0 M 0 M

CHANGE - X M X M X M

EQUILIBRIUM (0.1 -X) M X M X M

FOR THIS WEAK ACID REACTION

M

SUMMARY :

M

a. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.1×10−5.
b.Find the percent dissociation of this solution.
c. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.8×10−3
d. Find the percent
dissociation of this solution.
e.Find the
pH of a 0.100 M solution of a weak monoprotic
acid having Ka= 0.16.
f.Find the percent dissociation of this solution.

What is the pH of a buffer solution (0.100 L containing 0.166
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A 0.10 mol/L solution of a weak acid was found to be 4.0%
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1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL
of 0.300 M HX, a weak monoprotic acid, the pH of the resulting
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2. Will the equivalence point of ammonia plus HCl be
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Express the concentration to two significant figures.

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answer: 2.7x10-4

1. A 0.735 M solution of a weak acid is 12.5% dissociated.
(a)Calculate the [H3O+], pH, [OH -], and pOH of the solution. (b)
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