Question

A chemistry student carried out an experiment with a conducting apparatus similar to the one below. The following data was taken.



Solution Reading
0.1 M H2SO4 150 ma.
0.1 M Ba(OH)2 150 ma.
To 30 mL of the Ba(OH)2 solution, 10 mL portions of H2SO4 were added until a total of 50 mL of H2SO4 were used. The following results were recorded.

DATA TABLE

Total H2SO4 Added Meter Reading Observations
0 mL 150 ma. Ba(OH)2 and H2SO4 clear, colorless
10 mL 65 ma. milky white precipitate forms
20 mL 31 ma. more precipitate forms
30 mL 0 ma. precipitate heavy and settles
40 mL 29 ma. no

Answer 1

Explain the data.

Is any evidence shown that a reaction has occurred?


2.does the conductivity increase or decrease?
3.Does the number of ions in solution increase, decrease, or remain constant?
4.How can you tell?
5.How does this evidence indicate that the reaction has occurred between ions?

Answer 2

6.When the conductivity is at a minimum, what must be true about the amount of Ba(OH)2 compared to H2SO4?

Answer 3

7.Why does it not conduct at this low point?

Answer 4

8.Why does it conduct more before and after this minimum point?

Answer 5

1. a precipitate is formed
2. It decreases at first, then increases.
3. It increases at first, then decreases.
6. There is much less Ba(OH)2.
Sorry, I don't remember the others.