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 1.8xx10^(-5) and K_b for NH_4OH is 1.8xx10^(-5). T

1.	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
Answer» 7.005 4.75 `7.0` Between 6 and 7 Solution :GIVEN that , `K_a` for `CH_3COOH=1.8xx10^(-5)` `K_b` for `NH_4OH = 1.8xx10^(-5)` AMMONIUM acetate is a salt of WEAK acid and weak base. `therefore pH=7+(pK_a+pK_b)/2` `=7+([-log 1.8xx10^(-5)]-[-log 1.8xx10^(-5)])/2` `=7+(4.74-4.74)/2`=7.00