Calculate the number of moles of solute present in each of...

Calculate the number of moles of solute present in each of the following solutions: (a) $185 \mathrm{~mL}$ of $1.50 \mathrm{M}$ $\mathrm{HNO}_{3}(a q)$, (b) $50.0 \mathrm{mg}$ of an aqueous solution that is $1.25 \mathrm{~m} \mathrm{NaCl}$, (c) $75.0 \mathrm{~g}$ of an aqueous solution that is $1.50 \%$ sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)$ by mass.

Key Concepts

Unit Conversion

Unit conversion is a critical skill in chemistry, involving the transformation of measurements from one unit to another (for example, converting milliliters to liters, milligrams to grams, or grams to kilograms). Accurate unit conversion ensures that calculations involving concentration units such as molarity, molality, or percent by mass are performed correctly and consistently.

Percent by Mass

Percent by mass is a way to express the concentration of a solution by comparing the mass of the solute to the total mass of the solution, multiplied by 100. This unit is especially common in formulations where weight measurements are more straightforward, allowing for the calculation of the solute's mass from the overall mass of the mixture.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M) and is widely used in solution chemistry to relate the amount of substance to the volume of the solution, facilitating calculations involving chemical reactions and dilutions.

Mole Concept

The mole is a fundamental unit in chemistry that represents a specific number of particles, usually atoms or molecules, equivalent to Avogadro's number (approximately 6.022 × 10^23). It is used to convert between mass and the number of entities in a substance, and it is essential for stoichiometric calculations and determining the amount of solute in a solution.

Molality

Molality is a concentration unit defined as the number of moles of solute per kilogram of solvent. It is particularly useful in situations where temperature variations are involved since it does not depend on the volume of the solution, which can change with temperature.

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