A chemist determines the concentration of an aqueous solution to be 0.224 mol L ⁻¹ . If a measured volume of 3.4 L of this solution is transferred to a reaction flask, what is the number of moles of the solute present, reported to the correct number of significant figures?

Step-by-step solution

The number of moles of solute is calculated by multiplying the concentration by the volume. n = C V n = 0.224 mol L ⁻¹ 3.4 L = 0.7616 mol The concentration 0.224 mol L ⁻¹ has three significant figures, and the volume 3.4 L has two significant figures. In multiplication, the final result must be reported to the least number of significant figures present in the measured quantities, which is two. Rounding 0.7616 mol to two significant figures gives 0.76 mol . Answer: 0.76 mol