# Solving Dilution Problems

In other cases it may be inconvenient to weigh accurately a small enough mass of sample to prepare a small volume of a dilute solution.

In other cases it may be inconvenient to weigh accurately a small enough mass of sample to prepare a small volume of a dilute solution.

Usually this is done by evapourating or boiling, assuming that the heat of boiling does not affect the solute.

The dilution equation is used in these circumstances as well.

We are often concerned with how much solute is dissolved in a given amount of solution.

We will begin our discussion of solution concentration with two related and relative terms - dilute and concentrated.

The highly concentrated solution is typically referred to as the stock solution.

Example $$\Page Index$$: Diluting NITRIC ACID Nitric acid $$\left( \ce \right)$$ is a powerful and corrosive acid.

The aide is expected to use a syringe to draw up some stock solution and inject it into the waiting IV bag and dilute it to the proper concentration. Of course, the addition of the stock solution affects the total volume of the diluted solution, but the final concentration is likely close enough even for medical purposes.

Medical and pharmaceutical personnel are constantly dealing with dosages that require concentration measurements and dilutions.

A dilution is a solution made by adding more solvent to a more concentrated solution (stock solution), which reduces the concentration of the solute.

An example of a dilute solution is tap water, which is mostly water (solvent), with a small amount of dissolved minerals and gasses (solutes).

## Comments Solving Dilution Problems

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Problem #1 If you dilute 175 mL of a 1.6 M solution of LiCl to 1.0 L, determine the new concentration of the solution. Solution M1V1 = M2V2. 1.6 mol/L 175.…