Question

Experimental Procedure, Part A.1. Calculate the mass of disodium ethylenediaminetetraacetate (molar mass = 372.24 g/mol) required to prepare 250 mL of a 0.010 M solution. Show the calculation here and on the Report Sheet. Express the mass to the correct number of significant figures.

Answer 1

Answer:

0.93 g of disodium ethylenediaminetetraacetate is required.

Explanation:

Molarity of a solution = (Number of moles of solute in solution)/(Volume of solution in liter)

Here, disodium ethylenediaminetetraacetate is the solute.

Volume of solution = 0.250 L

Molarity of solution to be prepared = 0.010 M

So, number of moles of disodium ethylenediaminetetraacetate required = $(0.250\times 0.010)$ moles = 0.0025 moles

We know, number of moles = (mass)/(molar mass)

So, mass of disodium ethylenediaminetetraacetate required = $(372.24\times 0.0025)g$ = 0.93 g

Hence, 0.93 g of disodium ethylenediaminetetraacetate is required.