What will be the molarity of the resulting solutions made by...

What will be the molarity of the resulting solutions made by mixing the following? Assume that volumes are additive. (a) $175 \mathrm{~mL}$ of $3.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ with $275 \mathrm{~mL}_{2}$ of $\mathrm{H}_{2} \mathrm{O}$ (b) $350 \mathrm{~mL}$ of $0.10 \mathrm{M} \mathrm{CuSO}_{4}$ with $150 \mathrm{~mL}$ of $\mathrm{H}_{2} \mathrm{O}$ (c) $50.0 \mathrm{~mL}$ of $0.250 \mathrm{M} \mathrm{HCl}$ with $25.0 \mathrm{~mL}$ of $0.500 \mathrm{M} \mathrm{HCl}$

What will be the molarity of the resulting solutions made by mixing the following? Assume that volumes are additive.
(a) $175 \mathrm{~mL}$ of $3.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ with $275 \mathrm{~mL}_{2}$ of $\mathrm{H}_{2} \mathrm{O}$
(b) $350 \mathrm{~mL}$ of $0.10 \mathrm{M} \mathrm{CuSO}_{4}$ with $150 \mathrm{~mL}$ of $\mathrm{H}_{2} \mathrm{O}$
(c) $50.0 \mathrm{~mL}$ of $0.250 \mathrm{M} \mathrm{HCl}$ with $25.0 \mathrm{~mL}$ of $0.500 \mathrm{M} \mathrm{HCl}$

Key Concepts

Molarity

Molarity is a measure of concentration, defined as the number of moles of solute present per liter of solution. It is a fundamental concept in chemistry that allows us to relate the amount of dissolved substance to the overall volume of the solution.

Dilution

The process of dilution involves adding more solvent to a solution, thereby decreasing its concentration while keeping the total number of moles of solute constant. This principle is key when preparing solutions of lower molarity from more concentrated stock solutions.

Conservation of Moles

When solutions are mixed or diluted, the total number of moles of solute remains unchanged. This concept underpins calculations involving dilution, ensuring that the sum of the moles before mixing is equal to the sum of the moles after mixing.

Volume Addition

Volume addition is the assumption that when two solutions are mixed, their individual volumes combine additively without significant interaction effects. This simplification is often used to facilitate the calculation of the final concentration of the mixed solution.

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