A student made the following mistakes while performing the titration experiment.
ID: 520379 • Letter: A
Question
A student made the following mistakes while performing the titration experiment. Explain how it will affect the results of the experiment. i. The student forgot to add the indicator. ii. The initial volume of NaOH solution in the buret was not 0.00 mL, but 5.12 mL. iii. The student forgot to add 40 mL water into the flasks 1 and 2. 2. A standard solution of 1.25 M HCI was used to determine the concentration of 52.8 mL of an unknown solution of potassium hydroxide (KOH). If 12.6 mL of the acid was required to reach endpoint, determine the molarity of the KOH solution? What volume of a 0.5310 M solution of HNO_3 would be needed to titrate 120.00 mL of a 0.1525 M solution of NaOH?Explanation / Answer
Q1.
a)
if no indicator is added, there will never be an equivalence point, so this is actualy never going to have an end; tehre wil be excess titrant for sure
b)
If Vinitial = 5.12 but we account fo 0, then we are actually using LESS base, than we are accounting, so the concentration will be larger thanr eal value
c)
if students forget to add water, this will be much more concentrated, so the samples are gong to be accounted with a different Value
the concentratio will be lower than it actually is (calculated)
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