Question

g A chemist prepares a solution of barium acetate by measuring out 107 umol of barium acetate into a ml 200 volumetric flask and filling the flask to the mark with water. Calculate the concentration in of the chemist's barium acetate solution. Round your answer to significant digits.

Answer 1

Answer: The concentration of barium acetate solution is $5.35\times 10^{-4}M$

Explanation:

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}$

Moles of barium acetate = $107\mu mol=1.07\times 10^{-4}mol$    (Conversion factor:  $1mol=10^6\mu mol$ )

Volume of solution = 200 mL

Putting values in above equation, we get:

$\text{Molarity of barium acetate}=\frac{1.07\times 10^{-4}\times 1000}{200}\\\\\text{Molarity of barium acetate}=5.35\times 10^{-4}M$

Hence, the concentration of barium acetate solution is $5.35\times 10^{-4}M$