Question

Part I: Titration with an indicator
Insert a complete data table, including appropriate significant figures and units, in the space below. Be sure to include all trials that were completed in part I. Also include any observations that you made over the course of part I. (5 points)
Volume of HCl 20.0 mL
Initial volume of NaOH in buret 50.0 mL
Final volume of NaOH in buret 34.0 mL
Trial 2 (If needed)
Volume of HCl 20.0 mL
Initial volume of NaOH in buret 50.0 mL
Final volume of NaOH in buret 34.0 mL
Trial 3 (If needed)
Volum

Answer 1

I did all of the lab stuff I just can't do the calculations that are in the attached file

Answer 2

@k142

Answer 3

@ankit042@thomaster @rvc @faRiz @midhun.madhu1987 @Love.Kat123

Answer 4

You know how much NaOH you needed to reach the equivalence point, and you know its concentration so it is a simple matter of:

1. Determine volume of NaOH needed to reach equivalence point
Final buret reading - initial reading = volume of NaOH needed

Convert volume from mL to L
1000mL = 1L

(you can just multiply mL by (1/1000) to get to liters)

2. Find moles of NaOH needed to reach equivalence point (I dont see a concentration but I will assume it is in molarity)

Molarity = Moles/Volume (in litres)

solve for moles of NaOH

3. Use the reaction formula:
NaOH + HCl -> H2O + NaCl

No balancing required it is 1 to 1

Use the reaction formula to find moles of HCl

Since it is 1 to 1,

Moles of NaOH = Moles of HCl

4.

Take the formula:

Molarity = Moles/Volume (Litres)

Solve for Molarity and you are done the problem.

Answer 5

It pretty much explains this in your lab

Answer 6

Sorry for step 4

Volume in the formula will be the original volume of HCl solution

Answer 7

Make sure it is in litres

Answer 8

By equivalence point I mean the point at which the indicator changed to the colour desired

Answer 9

If you have any questions feel free to ask

Answer 10

Also for step 2 the volume you use in the formula will be the volume you determined in step 1