`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 :

K_a for CH_3COOH is 1.8 xx 10^-5 and K_b for NH_4OH is 1.8 xx 10^-5 . The pH of ammonium acetate will be

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

Given that K_(a) for acetic acid is 1.8xx10^(-5) and K_(b) for NH_(4)OH is 1.8xx10^(-5) at 25^(@)C . Predict the nature of aqueous solution of ammonium acetate.

Given that K_(a) for acetic acid as 1.8 xx 10^(-5) and K_(b) for NH_(4)OH As 1.8 xx 10^(-5) AT 25^(@)C , predict the nature of aqueous solution of ammonium acetate

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

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