Question

An intravenous solution was prepared by add-in 13.252 g of dextrose (C6H12O6) and 0.686 g of sodium chloride to a 250.0 mL volumetric flask and diluting to the calibration mark with water. What is the molarity of each component of the solution

Answer 1

Explanation:

Molarity(M) of a solution is defined as the number of moles of solute(n) present in one liter of solution(V).

$M=\frac{n}{V}$

The number of moles(n) can be calculated as shown below:

$n=\frac{mass of solute}{molar mass of solute}$

Molar mass of dextrose is 198.17 g/mol

Molar mass of NaCl is 58.5 g/mol.

Volume of the solution =250.0mL=0.250 L

The number of moels of dextrose($n_{d}$) is:

$n_{d} =\frac{13.252g}{198.17g/mol} \\=0.0669mol$

The number of moles of NaCl is:

$n_{NaCl} =\frac{0.686 g}{58.5g/mol} \\\\=0.01177 mol$

Thus, the molarity of dextrose is:

$M_d=\frac{n_d}{0.250 L} \\=0.0669mol/0.250L\\=0.268 M$

The molarity of NaCl is:

$M_Na_Cl=\frac{n_d}{0.250 L} \\\\=0.0118mol/0.250L\\\\=0.0472 M$

Answer:

The molarity of dextrose is 0.268 M.

The molarity of NaCl is 0.0472 M.