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How many liters of a 3.59 m K2SO4 solution are needed to provide 97.7 g of K2SO4 (molar mass 174.01 g/mol)?

Recall that m is equivalent to mol/L.

Express your answer to three significant figures.

Answer :

Final answer:

We are asked about the volume in liters of a 3.59 M solution of K2SO4 needed to yield 97.7 grams of K2SO4. After calculating the number of moles in 97.7 g of K2SO4, we then find the volume of the solution required to get this number of moles. The final answer is 0.156 liters.

Explanation:

The given question falls in the domain of Chemistry, specifically in the field of stoichiometry and solutions concentration. The task here is to determine the volume in liters of a 3.59 M solution of K2SO4 needed to obtain 97.7 g of K2SO4.

First, we calculate the number of moles of K2SO4 in 97.7 grams using its molar mass 174.01 g/mol:

Number of Moles = Mass / Molar Mass = 97.7 g / 174.01 g/mol = 0.561 moles

From the question, we also know that we have a 3.59 M solution of K2SO4, which means we have 3.59 moles of K2SO4 in every liter of the solution.

Hence, the volume of the solution required to get 0.561 moles of K2SO4 would be:

Volume = number of moles / concentration = 0.561 moles / 3.59 mol/L = 0.156 L

Therefore, 0.156 liters of the solution is needed to provide 97.7 g of K2SO4, rounded to three significant figures: 0.156 L, is the final answer.

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