Reference no: EM131139447

Read the appropriate section of the lab introduction and procedure before starting each section.

Part A - Data Table

	KHP Sample 1	KHP Sample 2	KHP Sample 3
Mass of flask and KHP (B)
Mass of empty flask (A)
Mass of KHP (B - A)
Final buret reading (D)
Initial buret reading (C)
Volume of base used (D - C)

Part B - Calculations. Show all of the calculation setups for each question in the space provided beneath the question. You must show your work!

1. Calculate the moles of acid in each flask:

KHP Sample 1:

KHP Sample 2:

KHP Sample 3:

2. Calculate the moles of base used for each sample (convert the moles of acid into moles of base using the balanced chemical equation):

Titration 1:

Titration 2:

Titration 3:

3. Using the moles of base determined above, and the volume of the base solution you dispensed from the buret, calculate the molarity of the base solution for each sample:

Titration 1:

Titration 2:

Titration 3:

4. Calculate the average molarity of the base solution you used in the titrations:

Instructor Initials: ______

Part C - Questions. Answer the following questions using complete sentences. For any questions requiring a calculation show the calculation setups and place a box around your final answer.

1. If you added 40 mL of water to a sample of KHP instead of 30 mL, would the titration of that sample then have required more, less, or the same amount of base? Explain.

2. A student weighs out 2.045 g of KHP. How many moles of KHP are in this sample?

3. A titration required 23.8 mL of a 0.15 M NaOH solution. How many moles of NaOH were in this volume?

4. A student weighed a sample of KHP and found it weighed 0.9803 g. The titration of this KHP required 23.45 mL of base (NaOH). Calculate the molarity of the base.