How many grams of solute are needed to make each of the...

How many grams of solute are needed to make each of the following solutions?
(a) $250.0 \mathrm{~mL}$ of $0.100 \mathrm{M}$ potassium sulfate
(b) $100.0 \mathrm{~mL}$ of $0.250 \mathrm{M}$ iron(III) chloride
(c) $500.0 \mathrm{~mL}$ of $0.400 \mathrm{M}$ barium acetate

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Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction, which in solution preparation includes calculating the number of moles of solute needed. Once the moles are determined from the product of molarity and volume, they are converted to grams using the solute's molar mass.

Molar Mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. It is used to convert the number of moles of a substance to its mass in grams, which is the final step in preparing a solution with a specified concentration.

Molarity

Molarity is the concentration of a solution expressed as the number of moles of solute per liter of solution. It is used to determine the amount of solute needed when preparing a solution of a certain volume, linking the concentration directly to the volume through moles.

Unit Conversion

Unit conversion is crucial when working with volumes in chemical calculations, especially converting milliliters to liters. This conversion is essential because molarity is defined in terms of liters, so the provided volume in milliliters must be converted to liters before performing any calculations.

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