Question

Resultant molarity of h+ ion in a mixture of 100 ml of 0.1 m h2so4 and 200 ml of 0.1 m h3po3 is:

Answer 1

dissociation of $H_2SO_4$ is ...

$H_2SO_4\Leftrightarrow 2H^++SO_4^{2-}$

here it is clear that , 1 mole of $H_2SO_4$ dissociation into 2 mole of $H^+$ and 1 mole of $SO_4^{2-}$

so, concentration of $H^+$ = 2 × concentration of $H_2SO_4$ = 2 × 0.1 = 0.2M

similarly, dissociation of $H_3PO_3$ is ...

$H_3PO_3\Leftrightarrow 3H^++PO_3^{3-}$

e.g., concentration of $H^+$ = 3 × concentration of $H_3PO_3$ = 3 × 0.1 = 0.3M

now, molarity of $H^+$ :

$M(V_1+V_2)=M_1V_1+M_2V_2$

or, M × (100mL + 200mL) = 0.2M × 100mL + 0.3 × 200mL

or, M × 300mL = 20 + 60 = 80mol

or, M = 80/300 = 8/30 = 0.266

hence, molarity of $H^+$ is 0.266M

Answer 2

Answer:

Explanation:

your answer is 0.2M