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Concentration of Solutions
Recall that a solution consists of two components: solute (the dissolved material) and solvent (the liquid in which the solute is dissolved). The amount of solute in a given amount of solution or solvent is known as the concentration. The two most common ways of expressing concentration are molarity and molality.
Molarity
The molar concentration (M) of a solution is defined as the number of moles of solute (n) per liter of solution (i.e, the volume, V solution):
M = n / V solution
The units of molarity are mol/L, often abbreviated as M.
For example, the number of moles of NaCl in 0.123L of a 1.00M solution of NaCl can be calculated as follows:
[tex]0.123 \: l \: \: of \: solution \: \times \: \frac{1.00 \: mole}{1.00 \: l \: of \: solution \: } \: \\ = 0.123 \: moles[/tex]
Molality :
The molal concentration (m) of a solution is defined as the number of moles of solute (n) per kilogram of solvent (i.e., the mass of the solvent, msolvent):
[tex]m = \frac{n}{v \: solution} [/tex]
For example, the number of moles of NaCl dissolved in 0.123kg of H2O (the solvent), in order to make a 1.00m solution of NaCl, can be calculated as follows:
[tex]0.123 \: kg \: of \: solvent \: = \frac{1.00 \: mole}{1.00 \: kg \: of \: solvent \: } \\ = 0.123 \: moles[/tex]
