Question

What is the percent dissociation of a 0.0217 M solution of chloroacetic acid, (HC2H2ClO2 )? (Ka = 1.35 × 10−3 )

Answer #1

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 Ka of a 2.41 M aqueous acid solution that
has a % dissociation of 2.4 %?

A 7.5×10−2 M solution of a monoprotic acid has a percent
dissociation of 0.61%. Determine the acid ionization constant (Ka)
for the acid.

A 8.5×10−2 M solution of a monoprotic acid has a percent
dissociation of 0.59%.Determine the acid ionization constant (Ka)
for the acid. Express your answer using two significant
figures.

a) What is the percent dissociation of a 0.45 M solution of
nitrous acid?
b) What is the present dissociation of a 0.28 M solution of
methylmine?
c)0.0950 M soution of acetic acid is 1.4% dissociated.
Calculated concentration of three species present in this solution:
hydronium ion, acetic acid, and acetate ion(not H2O or OH-):
d)what is present dissociation of a 0.35 M solution of
hydrobromic acid?

What is the percent ionization of a monoprotic weak acid
solution that is 0.186 M? The acid-dissociation (or ionization)
constant, Ka, of this acid is 2.43 × 10-12.

What is the percent dissociation of citric acid if the solution
has a pH=3.17 an a Ka=4.0x10^-6

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
Ba(OH)2 solution?

Find the pH of a 0.300 M HF (Ka=6.3×10−4) solution.
Find the percent dissociation of a 0.300 M HF solution

What is the percent ionization of hypobromous acid in a 0.035 M
HBrO solution? Ka = 2.8 x 10-9

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