What mass in grams of the indicated solute does each of the...

What mass in grams of the indicated solute does each of the following solution samples contain? a. $173 \mathrm{mL}$ of $1.24 \mathrm{M}$ KBr solution b. 2.04 L of $12.1 \mathrm{M} \mathrm{HCl}$ solution c. $25 \mathrm{mL}$ of $3.0 \mathrm{M} \mathrm{NH}_{3}$ solution d. $125 \mathrm{mL}$ of $0.552 \mathrm{M} \mathrm{CaCl}_{2}$ solution

What mass in grams of the indicated solute does each of the following solution samples contain?
a. $173 \mathrm{mL}$ of $1.24 \mathrm{M}$ KBr solution
b. 2.04 L of $12.1 \mathrm{M} \mathrm{HCl}$ solution
c. $25 \mathrm{mL}$ of $3.0 \mathrm{M} \mathrm{NH}_{3}$ solution
d. $125 \mathrm{mL}$ of $0.552 \mathrm{M} \mathrm{CaCl}_{2}$ solution

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Key Concepts

Molar Mass Calculation

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. Once the number of moles is determined, multiplying it by the molar mass of the solute gives the total mass of the solute in the solution. This conversion is crucial for quantifying the chemical amounts in practical applications.

Unit Conversion

Unit conversion is essential in these calculations since volumes are often given in milliliters but must be converted to liters to be compatible with the molarity unit (moles per liter). Accurate conversion ensures that subsequent calculations, such as moles of solute, are correct.

Molarity

Molarity is a measure of the concentration of a solution, defined as the number of moles of solute per liter of solution. It provides a direct relationship between the volume of the solution and the amount of solute present, which is critical when determining how much of a solute is required or present in a given volume.

Calculation of Moles

The calculation of moles from a solution involves using the formula: moles = molarity × volume (in liters). This step translates the concentration and volume information into the actual amount of solute in terms of moles, which is a central concept in stoichiometry.

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