Answer:
The most common unit of concentration is molarity, which is also the most useful for calculations involving the stoichiometry of reactions in solution. The molarity (M) of a solution is the number of moles of solute present in exactly 1 L of solution. Molarity is also the number of millimoles of solute present in exactly 1 mL of solution:
Equation 4.4
molarity =moles of soluteliters of solution=mmoles of solutemilliliters of solution
The units of molarity are therefore moles per liter of solution (mol/L), abbreviated as M. An aqueous solution that contains 1 mol (342 g) of sucrose in enough water to give a final volume of 1.00 L has a sucrose concentration of 1.00 mol/L or 1.00 M. In chemical notation, square brackets around the name or formula of the solute represent the concentration of a solute. So
[sucrose] = 1.00 M
is read as “the concentration of sucrose is 1.00 molar.” The relationships between volume, molarity, and moles may be expressed as either
Explanation:
Equation 4.5
VLMmol/L=L(molL)= moles
or
Equation 4.6
VmLMmmol/mL=mL(mmolmL)= mmoles
