Question

Determine how many liters (l) of stock HCl were used in titration #1.

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EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all your work in order to receive credit. Purpose Statement: HCl stock soln = 0.103 M Part A #1 initial HCl (mL) NaOH (mL) 0.00 0.15 final 26.12 27.60 Part A - Standardization of the Strong Base 1. A buret was conditioned and filled with stock HCl solution. 2. A second buret was conditioned and filled with stock NaOH solution. 3. A sample of HCl was drained into an Erlenmeyer flask, and 3 drops of phenolphthalein indicator was added. 4. NaOH solution was drained into the flask and swirled into the HCl until the indicator changed color. 5. Steps 1-4 were repeated for a second titration Endpoint was a clear, very faint pink solution. Part A #2 HCl (mL) NaOH (mL) 0.48 0.40 initial final 25.55 27.16 Clear, very faint pink solution. Part B - Preparation of Strong Acid Solution 6. Obtained an assignment for a solution of HCI to prepare, and prepared it as a dilution of 6 M HCL. Calculate how many mL of 6 M HCl you need in order to make 250 mL of your assigned concentration. Show your work to receive credit. Part C-Titration of Prepared Acid Solution 7. A sample of the prepared HCI was measured in a graduated cylinder and transferred to a flask with phenolphthalein indicator. 8. HCl sample was then titrated to endpoint using the standardized NaOH solution. Part C initial HCI (mL) NaOH (mL) 1.20 23.0 final Clear, very faint pink solution.

Answer 1