Question

Calculate the molarity of a solution of glycerol made by dissolving 42.000 mLmL glycerol at 15 ∘C∘C in enough water to make 340.00 mLmL of solution.

Answer 1

Answer:

The molarity of a solution of glycerol is 1.6902 M.

Explanation:

Volume of glycerol = 42.000 mL

Mass of glycerol = m

Density of glycerol = d = 1.26 g/mL

$m=d\times V = 1.26 g/mL\times 42.000 mL=52.9200 g$

$Molarity=\frac{\text{Moles of compound}}{\text{Volume of solution (L)}}$

Moles of glycerol = $\frac{52.9200 g}{92.09 g/mol}=0.57466 mol$

Volume of the solution = 340.00 mL = $340.00\times 0.001 L$

( 1 mL=0.001 L)

$M=\frac{0.57466 mol}{340.00\times 0.001 L}=1.6902 M$

The molarity of a solution of glycerol is 1.6902 M.

Answer 2

Molar concentration is a calculation of the concentration of solution measured by dividing the solute per litre by the number of moles of the solute present in the solution.

Molarity is calculated by using the formula:

                                     $\text {M}&= \dfrac {\text{n}}{\text{V}}$

Where M is molarity, n is moles of solute, and V is the volume of solution in litres.

Given,

• glycerol volume  = 42.000 mL

• glycerol mass = unknown

• glycerol density = 1.26 g/mL

Mass can be calculated as:

$\text {M}&= \dfrac {\text{d}}{\text{V}}$

$\text {M}&= \dfrac {\text{1.26gram per mL}}{\text{42.000 mL}}$

= 52.9200 g

The number of moles of glycerol present is calculated as:

$\text {M}&= \dfrac {\text{Mass of glycerol}}{\text{Molar mass of glycerol}}$

$\text {M}&= \dfrac {\text{ 52.9200g}}{\text{92.09g/mol}}$

= 0.57466 mol

The volume of solution in litres = 340.00 × 0.001 L

(As ml= 0.001 L)

Thus the molarity:

$\text {M}&= \dfrac {\text{Moles present in a compound}}{\text{Volume of solution in litres.}}$

$\text {M}&= \dfrac {\text{0.57466 mol}}{\text{340.00} \times { 0.001 L}} = 1.6902 M$

Therefore, molarity of a solution of glycerol is 1.6902 M.

To learn more about, molarity follow the given link:

https://brainly.com/question/8732513