Question

What will be the molarity of 4M H2SO4 solution when its 30 ml is diluted by adding 470 ml water?

Answer 1

ANSWER:

• The molarity of resulting solution = 0.255 M.

GIVEN:

• 30 mL of 4 M H₂SO₄ is diluted by adding 470 mL water.

TO FIND:

• The molarity of resulting solution.

EXPLANATION:

Molarity of Dilution:

$\boxed{ \bold{ \green{ \large{M_1 V_1 = M_2 V_2}}}}$

$\implies \sf M_1 = 4\ M$

$\implies \sf V_1 = 30\ mL$

$\implies \sf V_2= 470\ mL$

$\sf \dashrightarrow 4(30) = M_2 (470)$

$\sf \dashrightarrow 4(3) = M_2 (47)$

$\sf \dashrightarrow M_2 = \dfrac{12 }{47}$

$\sf \dashrightarrow M_2 = 0.255 \ M$

$\bigstar \ \blue{\textsf{The molarity of resulting solution = 0.255 M}}$

EXTRA CALCULATION:

NORMALITY:

$\boxed{ \bold{ \orange{ \large{Normality = Molarity \times Basicity}}}}$

$\implies \sf Molarity= 0.255\ M$

$\implies \sf Basicity = 2$

$\sf \hookrightarrow N = 0.255 \times 2$

$\sf \hookrightarrow \pink{Normality= 0.51 \ N}$