Question

the ph of 0.15 M solution of HOCl (Ka= 9.6*10-6)​

Answer 1

Answer:

5.85.

Explanation:

Since, the concentration of the HOCl is given in the question as 0.15M. While the Ka value is given as 9.6*10^-6. So, to find the pH we need to find the H+ ion concentration of the compound.

So, the [H+] will be given as √(Ka*c) which can be written as √(9.6*10^-6 * 0.15) which on solving we will get that 1.44*10^-6. So, to find the pH we have to take the logarithm value of the H+. Which is pH=-log(H+) or -log(1.44*10^-6) which is 6-log(1.44) = 6-0.15 which on solving we will get 5.85.

Answer 2

Answer:

Explanation:We know that for acidic solution

[H  +  ]=  K  a  C =9.6×10  −6  ×0.15  =  1.44×10  −6   =0.0012M

pH=−log[H  +  ]=−log[0.0012]=2.920818

∴   Ans :- Option B.