(a) How many milliliters of a stock solution of 10.0 M HNO3 would you have to use to prepare 0.4

step 1 In this first example, we're diluting a more concentrated solution. So we'll use our dilution fo

(a) How many milliliters of a stock solution of 10.0 M HNO3...

(a) How many milliliters of a stock solution of $10.0 \mathrm{M}$ $\mathrm{HNO}_{3}$ would you have to use to prepare $0.450 \mathrm{~L}$ of $0.500 \mathrm{M} \mathrm{HNO}_{3} ?$ (b) If you dilute $25.0 \mathrm{~mL}$ of the stock solution to a final volume of $0.500 \mathrm{~L}$, what will be the concentration of the diluted solution?

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Key Concepts

Dilution Equation

The dilution equation, expressed as M1V1 = M2V2, relates the concentrations and volumes of solutions before and after dilution. This equation allows one to determine how much of a concentrated (stock) solution is required to achieve a desired lower concentration by diluting with solvent.

Volume Conversion

Volume conversion is the process of converting between different units of volume, such as milliliters and liters, which is critical in solution preparation and titration calculations. Accurate conversion ensures that the dilution equation is applied correctly when mixing solutions.

Stock Solution

A stock solution is a concentrated solution that can be diluted to lower concentrations for various experimental needs. It is used as a starting point in laboratory settings, enabling precise and efficient preparation of solutions with specific molarities through dilution.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is a fundamental concept in chemistry used to quantify the concentration of solutions and is essential for stoichiometric calculations in reactions, including dilution procedures.

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