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Standard XII

Chemistry

Amino Acids

The ionizatio...

Question

The ionization constant of acetic acid is 1.74 × 10^–5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

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Solution

Method 1

Since Ka >> K_w,:

Method 2

Degree of dissociation,

c = 0.05 M

K_a = 1.74 × 10^–5

Thus, concentration of CH₃COO– = c.α

Hence, the concentration of acetate ion in the solution is 0.00093 M and its Ph is 3.03.

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The ionization constant of acetic acid is 1.74 × 10–5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

Method 1 Since Ka >> Kw, : Method 2 Degree of dissociation, c = 0.05 M Ka = 1.74 × 10–5 Thus, concentration of CH3COO– = c.α Hence, the concentration of acetate ion in the solution is 0.00093 M and its Ph is 3.03.

The ionization constant of acetic acid is 1.74 × 10^–5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

Method 1

Since Ka >> K_w,:

Method 2

Degree of dissociation,

c = 0.05 M

K_a = 1.74 × 10^–5

Thus, concentration of CH₃COO– = c.α

Hence, the concentration of acetate ion in the solution is 0.00093 M and its Ph is 3.03.