Exp 2: Volumetric Analysis

Experiment 2 Virtual Lab Tutorial >> Acid Base Titration >> Step 1: Tutor 2

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Experiment 2 Virtual Lab Tutorial: Acid Base Titration

Step 1: Calculating the amount of solid KHP required to prepare the 0.1 M standard solution

Once the required mass of KHP has been calculated we can weigh out approximately 5.11 g of KHP by difference on an analytical balance and prepare a 250.0 mL standard solution of KHP in a volumetric flask.

Tutor 2: Calculating the exact concentration of the prepared solution of KHP

If the mass of KHP weighed by difference on the analytical balance is 5.1034g, what is the concentration of the 250.0 mL standard solution of KHP?

Hint

M KHP

Please give your answer to 4 significant figures.

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That's not quite right.

Hint:

The definition of concentration is M = moles / volume. To find the concentration we must first calculate how many moles of KHP are contained in the 5.1034 g.

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Hint:

Moles KHP = mass / Molecular mass
= 5.1034 g / 204.22 g mol^-1 KHP = 0.024989 mol

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Hint:

Now that we have found the moles of KHP and know the volume of the standard solution we need to prepare, we can find its concentration.

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Hint:

M = moles of solute/Volume of solution in L

M = 0.024989 mol/0.2500 L = 0.09996 M

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