NOTES: a) Hydrochloric Acid #1(unknown concentration) b) Sodium Chloride 0.100m

Question

NOTES: a) Hydrochloric Acid #1(unknown concentration) b) Sodium Chloride 0.100m 1. Poured 50ml of sodium chloride into burette(initial NaOH volume) 2. Added 10ml hydrochloric acid;TV=10ml and 10ml of water to Erlenmeyer flask 3. Added 2 drops of phenophthalein; TV=20.1 4. Placed flask unto burette Coarse Titration: (delivered in 2ml increments) 2ml=48ml(burette); 22.10ml(flask) 4ml=46ml(burette); 24.10ml(flask) 6ml=44ml(burette); 26.09ml(flask) 8ml=42ml(burette), 28.09ml(flask) 10ml=40ml(burette); 26.09ml(flask) CHANGE IN COLOR: 11.25 ml=38.75ml(burette); 31.34ml(flask) 12ml=38ml(burette); 32.09ml(flask) 14ml=36ml(burette); 34.09ml(flask) 16ml=34ml(burette); 36.09ml(flask) Fine Titration: (delivered in drops) Followed steps 1-4 above and added 16ml into burette to bring back to 50ml. Final NaOH= 38.75ml(burette), 11.25ml dispensed, 31.34ml(flask)

Is this correct so far?

1. For your most exact titration, record the following:

a Volume of NaOH solution in the burette at the start (mL): 50ml

b Volume of NaOH solution in the burette at the end (mL): 38.75ml

c Volume of NaOH solution delivered to the flask (mL): 31.34ml

d Volume of HCl solution in the flask (mL): 20.1ml

Explanation / Answer

The calculations shown on the page above,

for the volumes of NaOH dispensed and HCl volume looks alright as shown above.

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