4 textml of HCl solution of pH=2 is mixed with 6 ml of NaOH solution of pH=12 . What would be the final pH of solution? [ log 2 = 0.3]

Question

4 textml of HCl solution of pH=2 is mixed with 6 ml of NaOH solution of pH=12 . What would be the final pH of solution? [ log 2 = 0.3] (A) 10.3 (B) 11.3 (C) 11 (D) 4.3

Tardigrade Admin · Accepted Answer

[.HCl].=0.01[.NaOH].=0.01 M textmixt=(6 × 0.01 - 4 × 0.01/10)=(0.02/10) [. oversetΘOH].=0.002 textpOH = - textlog (. 0.002 .) = 2.7

Q. $4 ml$ of $H Cl$ solution of $p H = 2$ is mixed with $6 m l$ of $N a O H$ solution of $p H = 12$ . What would be the final $p H$ of solution?
$[lo g 2 = 0.3]$

$10.3$

$11.3$

$11$

$4.3$

$[H Cl] = 0.01 [N a O H] = 0.01$
$M_{mixt} = \frac{6 \times 0.01 - 4 \times 0.01}{10} = \frac{0.02}{10}$
$[O Θ H] = 0.002$
$pOH = - log (0.002) = 2.7$

Q. 4ml of HCl solution of pH=2 is mixed with 6ml of NaOH solution of pH=12 . What would be the final pH of solution? [log2=0.3]

10.3

11.3

11

4.3