This Lab is called Standardization of a Solution . My results are: After removin

Question

This Lab is called Standardization of a Solution.

My results are:

After removing the beaker from the desiccator and recording the mass in the table,

I followed this step --> Use the 100 mL graduated cylinder to measure and

pour 75 mL of distilled water to dissolve the citric acid in the beaker.

So now I have to answer Question #1 and I'm not sure how?

1. Calculate the exact number of moles of citric acid that you weighed

out and divide this by 0.100 L to obtain the molarity of the solution.

Mass of BeakerMass of Beaker Mass of Citric Mass of Beaker Molarity of +Citric AcidCitric Acid (Step 1; g) +Citric AcidAcid (Step 1 - Ci (Step 3; g) Step 3; g) After CoolingSolution (M) (Step 7; g) 10.3g 12.30g2.0g 1230

Explanation / Answer

mass of citric acid = 2 g;
Molecular weight = 192.124 g/mol;
number of moles = 2 / 192.124 = 0.01041

Volume of solution = volume of solvent = 75 mL = 0.075 L
Thus, molarity = n/V = 0.01041/0.075 = 0.139 M

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