Ka for CH3COOH is 1.8xx10^(-5) and Kb fo...

`K_a` for `CH_3COOH` is `1.8xx10^(-5)` and `K_b` for `NH_4OH` is `1.8xx10^(-5)` The pH of ammonium acetate will be :

7.005

4.75

`7.0`

Between 6 and 7

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Higher the amount of acid or base used to product a deinite change of pH in a buffer solution, higher will be its buffe capacity. Buffer capcity of solution is maximum under the following conditions [Salt] = [Acid](in acid buffer) [Salt] = [Base] (in base capacity] pH of buffer solution lies inthe range given below pH = pH_(a) +-1 In other words,any buffer solution can be used as buffer up to two pH units only, depending upon the value of pK_(a) or pK_(b) . A buffer is said to be efficient when pH = pK_(a) or pOH = pK_(b) K_(a) for CH_(3)COOH is 1.8 xx 10^(-5) and K_(b) for NH_(4)OH is 1.8 xx 10^(-5) . The ph of ammonium acetate will be

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For NH_(3) , K_(b)=1.8xx10^(-5) . K_(a) for NH_(4)^(+) would be

Calculate the pH of a solution of given mixture. a. (2g CH_(3)COOH +3g CH_(3) COONa) in 100mL of mixture. b. 5mL of 0.1M NH_(4)OH + 250mL of 0.1 M NH_(4)C1 . c. (0.25 "mol of" CH_(3)COOH + 0.35 "mol of" CH_(3) COONa) in 500mL mixture. K_(a) "of" CH_(3)COOH = 1.8 xx 10^(-5) (pK_(a) = 4.7447) K_(b) "of" NH_(4)OH = 1.8 xx 10^(-5) (pK_(b) = 4.7447)

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MODERN PUBLICATION-EQUILIBRIUM-Objective A.(MCQs)

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