1litre of aqueous solution of HCl has pH=1 . How many litres of water must be added to create an aqueous solution with pH of 2 ?

Question

1litre of aqueous solution of HCl has pH=1 . How many litres of water must be added to create an aqueous solution with pH of 2 ? (A) 2.0 (B) 9.0 (C) 0.1 (D) 0.9

Tardigrade Admin · Accepted Answer

pH=1=-log[H+] [H+]=10- 1M Final pH=2;[H+]=10- 2 M M1V1=M2V2 (0 . 1 M × 1 Litre)=(0 . 01)V2 V2=10L Final volume =10L Water added =10-1=9L

Q. $1 l i t re$ of aqueous solution of $H Cl$ has $p H = 1$ . How many litres of water must be added to create an aqueous solution with $p H$ of $2$ ?

$2.0$

$9.0$

$0.1$

$0.9$

$p H = 1 = - l o g [H^{+}]$
$[H^{+}] = 1 0^{- 1} M$
Final $p H = 2; [H^{+}] = 1 0^{- 2} M$
$M_{1} V_{1} = M_{2} V_{2}$
$(0.1 M \times 1 L i t re) = (0.01) V_{2}$
$V_{2} = 10 L$
Final volume $= 10 L$
Water added $= 10 - 1 = 9 L$

Q. 1litre of aqueous solution of HCl has pH=1 . How many litres of water must be added to create an aqueous solution with pH of 2 ?

2.0

9.0

0.1

0.9