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Exp 2: Volumetric Analysis-Tutor 1: Calculating the amount of solid KHP required -Tutor 2: Calculating the exact concentration of the prepared KHP solution -Tutor 3: Calculations for the standardization of NaOH -Tutor 4: Determining the concentration of NaOH -Tutor 5: Calculations for the standardization of diluted unknown HCl -Tutor 6 Calculations for the standardization of unknown HCl |
Experiment 2 Virtual Lab Tutorial >> Acid Base Titration >> Step 1: Tutor 1
Experiment 2 Virtual Lab Tutorial: Acid Base TitrationStep 1: Calculating the amount of solid KHP required to prepare the 0.1 M standard solutionIn this tutorial, we are required to prepare 250.0 mL of about 0.1 M KHP solution with 4 significant figures precision. We will need to calculate how much of the solid KHP we will require for this purpose. Tutor 1: Calculating the amount of solid KHP required.
What mass of KHP needs to be weighed out to prepare 250.0 mL of the standard KHP solution?
Please enter your answer with two decimal places.
Hint
g KHP
Type your answer and press the ENTER key to continue.
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That's not quite right.
Hint:
If you are having trouble, scroll below to get step by step help in solving this problem.
The following tutors are a step by step walkthrough that show the details on how to solve the above problem. First, we must calculate the number of moles of KHP needed to prepare 250.0mL (0.2500L) of the 0.1M solution:
Hint
moles KHP
Please enter your answer with 2 significant figures.
Good Job!
That's not quite right.
Hint:
Since the concentration, or molarity, of a solution is defined as:
Molarity, M = # moles solute / volume of solution (in litres) Then for any solute we can express the number of moles using the respective molarities and volumes. KHP solute: # moles KHP = MKHP x VKHP where MKHP = molarity of KHP and VKHP = its volume. get next hint
Hint:
Applying the above values into the equation yields:
# moles KHP = MKHP x VKHP = 0.1 M x 0.2500 L = 0.02500 moles KHP = 0.025 moles KHP (with 2 significant figures) get previous hint
Keeping in mind that moles (n) can be defined as:
moles (n) = mass of compound / molecular mass of compound and that the molecular mass of KHP (C8H5O4K) is 204.22 g mol-1, calculate the mass of KHP.
Hint
grams KHP
Please enter your answer with 2 decimal places.
Good Job!
That's not quite right.
Hint:
We can rearrange the above equation to:
mass of compound = (moles)*(molecular mass of compound) get next hint
Hint:
Applying the calculated values into the equation yields:
mass of KHP = (0.02500 moles KHP)*(204.22 g mol-1 KHP) = 5.11 g get previous hint
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| Last Updated: Wednesday, April 14th, 2021 @ 04:06:17 pm |