Question

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the pH of a 0.12 M solution of this acid?

Answer #1

Dear friend your answer should be by taking acetic acid because
acetic acid is a weak monoprotic acid. only weak acids can have
acid dissociation constant K_{a}

CH_{3}COOH -----> CH_{3}COO^{-} +
H^{+}

K_{a} = [H^{+}][CH_{3}COO^{-}] /
[CH_{3}COOH] = 1.6 x 10^{-6}

Let x = the amount of CH_{3}COOH that dissociates.

[H^{+}] = x

[CH_{3}COO^{-}] = x

[CH_{3}COOH] = 0.12 - x = 0.12 (assuming x <<
0.12)

1.6 x 10^{-6} = (x) (x) / (0.12)

x = 0.00043817 = [H+]

pH = - log (0.00043817) = 3.3583

**P ^{H} of a given monoprotic acid is
3.3583**

**Thank you.**

If the Ka of a monoprotic weak acid is 7.5 × 10-6, what is the
pH of a 0.12 M solution of this acid?

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the
[H ] of a 0.27 M solution of this acid?

If the Ka of a monoprotic weak acid is 3.3 × 10-6, what is the
pH of a 0.30 M solution of this acid?

If the Ka of a monoprotic weak acid is 5.7 × 10-6, what is the
pH of a 0.14 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
pH of a 0.43 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
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1.) If the Ka of a monoprotic
weak acid is 4.5 x 10^-6, what is the pH of a 0.30M solution of
this acid?
2.) The Ka of a monoprotic weak
acid is 7.93 x 10^-3. What is the percent ionization of a 0.170 M
solution of this acid?
3.) Enolugh of a monoprotic acid
is dissolved in water to produce a 0.0141 M solution. The pH of the
resulting solution is 2.50. Calculate the Ka for the
acid.

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.

1. The Ka of a monoprotic weak acid is 5.90 × 10-3. What is the
percent ionization of a 0.148 M solution of this acid?
2. If the Kb of a weak base is 4.5 × 10-6, what is the pH of a
0.26 M solution of this base?
3. Assuming complete dissociation, what is the pH of a 3.00 mg/L
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The Ka of a monoprotic weak acid is 6.69 × 10-3. What is the
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