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

Step-by-step explanation:

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

`M=(n)/(V)`

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

`n=(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) =(13.252g)/(198.17g/mol) \\=0.0669mol`

The number of moles of NaCl is:

`n_(NaCl) =(0.686 g)/(58.5g/mol) \\\\=0.01177 mol`

Thus, the molarity of dextrose is:

`M_d=(n_d)/(0.250 L) \\=0.0669mol/0.250L\\=0.268 M`

The molarity of NaCl is:

`M_Na_Cl=(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.