Part A. The mass of KHC8H4O4 is measured to the nearest milligram; however, the
ID: 553166 • Letter: P
Question
Part A. The mass of KHC8H4O4 is measured to the nearest milligram; however, the volume of water in which it is dissolved is neverof concern—water is even added to the wall of the Erlenmeyer flask during the titration. Explain why water added to the KHC8H4O4has no effect on the data, whereas water added to the NaOH solution may drastically affect the data.
5. Part B.2. The wall of the Erlenmeyer flask is occasionally rinsed with water from the wash bottle (see Part A.6) during the analysis of the acid solution. Will this technique result in the molar concentration of the acid solution being reported as too high, too low, or unaffected? Explain.
6. Parts A.6 and B.2. For the standardization of the NaOH solution in Part A.6, the endpoint was consistently reproduced to a faint pink color. However, the endpoint for the titration of the acid solution in Part B.2 was consistently reproduced to a dark pink color. Will the reported molar concentration of the acid solution be too high, too low, or unaffected by the differences in the colors of the endpoints. Explain.
Explanation / Answer
Part A)
The mass of KHC8H4O4 is 204.22 g/mol, therefore we know the moles of it. No matter how much water you add to the KHC8H4O4 the number of moles will never change. if you add water to NaOH that changes the concentration which would result the number of moles used titrating
5) Part B.2:In the flask the moles of titrant are reacting with moles of titrand. So on adding water to flask the number of moles of reactant will remain the same hence the water will not affect the reaction.
6) the dark pink colour shows that we have added excess of NaOH to the flask. So
M1V1 = M2V2
M1 = molarity of base
V1 = Volume of base
M2 = molarity of acid
V2 = Volume of acid
So,M2 = M1V1 / V2
so addition of extra volume of base, the concentration of acid will appear to be too high.