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3 years ago

Calculate the molarity of a solution of monoprotic KHP prepared by mixing a 0.5237 g KHP in 50.0 mL of water .

Chemistry

1 answer:

Sergio039 [100]3 years ago

3 0

Answer:

$M=0.0513M$

Explanation:

Hello!

In this case, since the molarity of a solution is computed by dividing the moles of solute by the volume of solution, we notice we first need the moles of KHP as shown below:

$n=0.5237g*\frac{1mol}{204.22 g} =0.00256mol$

Next, the volume in liters:

$V=50.0mL*\frac{1L}{1000mL}\\\\V=0.0500L$

Thus, the molarity turns out to be:

$M=\frac{n}{V}\\\\M=\frac{0.00256mol}{0.05000L} \\\\M=0.0513M$

Best regards!

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$\Delta T_f=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}$

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