2. A student was performing an acid/base titration to determine the molar concen

Question

2. A student was performing an acid/base titration to determine the molar concentration of a sample of vinegar, using phenolphthalein as an indicator. After dispensing a 10.00 mL sample of vinegar that she was going to titrate, she noticed droplets of her solution clinging to the inside of her pipette She performed her titration of the sample of some of the sample remaining in the pipette affect the calculated value for the molarity of acetic acid in the sample of vinegar? Would it be higher or lower than the true value? Explain why her titration of the sample of vinegar to a light pink end-point. How would 3. A student was performing an acid/base titration, to determine the molar concentration of a sample of vinegar, using phenolphthalein as an indicator. After dispensing a 10.00 mL sample of vinegar, she noticed some sample remaining in the tip of the pipet. She blew out the sample in the tip of the pipette combining it with the solution she previously dispensed. How would blowing out the sample of vinegar in the tip of the pipette affect the calculated value for the molarity of acetic acid in the sample of vinegar? Would it be higher or lower than the true value? Explain why

Explanation / Answer

Ans 2 :

Since some of the sample solution was clinging to the inside of the pipette , the volume of the vinegar and acetic acid in it is used less than the one assumed.

Now when M1V1 = M2V2 formula is used to determine the concentration of acid , the low volume of sample will cause the volume of base also to decrease.

So the calculated molarity of sample will come out to be less , which will be lower than the true value.

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