Question

What is the molarity of a 10.2 % by mass glucose (C6H12O6) solution? (The density of the solution is 1.03 g/mL .) Express your answer with the appropriate units.

Answer 1

Answer: 0.58 M

Step-by-step explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

`Molarity=(n* 1000)/(V_s)`

where,

n= moles of solute

`V_s` = volume of solution in ml

Given : 10.2 g of glucose is present in 100 g of solution

density of solution = 1.03 g/ml

volume of solution =
`\frac{\text {mass of solution}}{\text {density of solution}}=(100g)/(1.03g/ml)=97.1ml`

`{\text {moles of solute}}=\frac{\text {given mass}}{\text {molar mass}}=(10.2g)/(180g/mol)=0.057moles`

Now put all the given values in the formula of molarity, we get

`Molarity=(0.057moles* 1000)/(97.1ml)=0.58mole/L`

Thus the molarity of solution will be 0.58 M.