Question

A 1.30M solution of BaCl2 has a density of 1.230 g/ml. a) What is the mole fraction of BaCl2 in this solution?

Answer 1

Answer: The mole fraction of barium chloride in the solution is 0.024

Step-by-step explanation:

We are given:

Molarity of barium chloride solution = 1.30 M

This means that 1.30 moles of barium chloride is present in 1 L or 1000 mL of solution.

• To calculate the mass of solution, we use the equation:

`\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}`

Density of solution = 1.230 g/mL

Volume of solution = 1000 mL

Putting values in above equation, we get:

`1.230g/mL=\frac{\text{Mass of solution}}{1000mL}\\\\\text{Mass of solution}=(1.230g/mL* 1000mL)=1230g`

• To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}` .....(1)

Moles of barium chloride = 1.30 moles

Molar mass of barium chloride = 208 g/mol

Putting values in equation 1, we get:

`1.30mol=\frac{\text{Mass of barium chloride}}{208g/mol}\\\\\text{Mass of barium chloride}=(1.30mol* 208g/mol)=270.4g`

Mass of water = Mass of solution - Mass of barium chloride

Mass of water = 1230 - 270.4 = 959.6 g

Calculating the moles of water:

Given mass of water = 959.6 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

`\text{Moles of water}=(959.6g)/(18g/mol)\\\\\text{Moles of water}=53.31mol`

Mole fraction of a substance is given by:

`\chi_A=(n_A)/(n_A+n_B)`

• For barium chloride:

`\chi_{\text{(barium chloride)}}=\frac{n_{\text{(barium chloride)}}}{n_{\text{(water)}}+n_{\text{(barium chloride)}}}`

`\chi_{\text{(barium chloride)}}=(1.30)/(1.30+53.31)\\\\\chi_{\text{(barium chloride)}}=0.024`

Hence, the mole fraction of barium chloride in the solution is 0.024