The molarity of a solution is related to the amount of solute dissolved within a solvent.

Concept #1: Molarity is the concentration of a solution represented as moles of solute per liter of solution:

Concept #2: Ionic molarity or osmolarity represents the molarity of dissolved ions in a solution.

Concept #3: Whenever two molarities or two volumes are given for one compound then a dilution is usually involved.

Example #1: Stock hydrochloric acid solution is 21.0% by mass HCl and has a specific gravity of 1.75. What is the molarity of the solution.

Example #2: What is the concentration of nitrate ions in a solution that contains 83.3 g lead (IV) nitrate, Pb(NO_{3})_{4}, dissolved in 700 mL solution? MW of Pb(NO_{3})_{4} is 455.24 g/mol.

Example #3:

How many micrograms of K_{2}CO_{3} are required to prepare 120 mL of 0.325 M K_{2}CO_{3}? MW of K_{2}CO_{3} is 138.21 g/mol.

Example #4:

If 50.0 mL of water is added to 80.0 mL of a 6.00 M solution, what will be the new concentration of the new solution?

Example #5:

To what volume should you dilute 72.93 mL of a 7.505 M LiCl solution so that 23.25 mL contains 2.25 g LiCl? MW of LiCl is 42.392 g/mol.

Example #6: 870.0 g of water contains 0.990 g of sodium phophate, Na_{3}PO_{4}. Determine the concentration of Na_{3}PO_{4} if the density of the solution is 1.10g/mL. MW of NA_{3}PO_{4} is 163.94 g/mol.