Question

determine the molarity of a solution made by dissolving 9.51 g of k2so4 in water where the final volume of the solution is 750.0 ml.

Answer 1

We are given –

• Weight of $\bf K_2SO_4$ is = 9.51 g
• Volume, V = 750 ml

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Molar Mass of $\bf K_2SO_4$ –

$\qquad$ $\twoheadrightarrow\bf 39.09 \times 2 + 32 + (16 \times 4)$

$\qquad$ $\twoheadrightarrow\bf 174.2$

Using formula –

$\qquad$ $\purple{\twoheadrightarrow\bf Molarity _{(Solution)} = \dfrac{ W\times 1000}{MV}}$

$\qquad$ $\twoheadrightarrow\bf Molarity _{(Solution)} = \dfrac{ 9.51 \times 1000}{174.2\times 750}$

$\qquad$ $\twoheadrightarrow\bf Molarity _{(Solution)} = \dfrac{9510}{174.2 \times 750}$

$\qquad$ $\purple{\twoheadrightarrow\bf Molarity _{(Solution)} = 0.073M}$

• Henceforth, Molarity of the solution is = 0.073M.

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