The dissociation constant of acetic acid is 1-8- 10 -5 and that of ammonium hydroxide is also 1-8- 10 -5 at 25 o C- Hence- an aqueous solution of ammonium acetate is-

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Ways of Representing the Concentration of a Solution

The dissociat...

Question

The dissociation constant of acetic acid is $1.8 \times 10^{- 5}$ and that of ammonium hydroxide is also $1.8 \times 10^{- 5}$ at $25^{o} C$ . Hence, an aqueous solution of ammonium acetate is:

Acidic

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Basic

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Neutral

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Slightly acidic

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Solution

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K_{a}

1.77 \times 10^{- 5}

K_{b}

1.82 \times 10^{- 5}

(C H_{3} C O O N H_{4})

25^{\circ} C

K_{a}

1.77 \times 10^{- 5}

K_{b}

1.82 \times 10^{- 5}

(C H_{3} C O O N H_{4})

25^{\circ} C

25^{o} C

p H = 5

K_{a}

1.8 \times 10^{- 5}

{log}_{10} 1.8 = 0.25 and 10^{(0.25)} = 1.8

1.8 \times 10^{- 5}

4.2 \times 10^{- 10}

0.1

K_{a} = 1.8 \times 10^{- 5}

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