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

here are the questions i cannot understand how to do...

Answer 2

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 3

Well you are reacting an acid (H2SO4) with a base Ba(OH)2
thus you get a salt, water and sometimes CO2

so draw a reaction mechanism

Then since there is precipitate leaving the solution, it is most likely the salt if the salt is leaving the solution the amount of ions decreases. If the amount of ions decrease the amount of conductivity decreases (remember water is an isolator but when it has ions dissolved in it conducts electricity).

Evidence is the participant if you test it you will see it is a new compound, therefore a chemical change has occurred.

Answer 4

You should explain it in more depth though.

Answer 5

oh ok.. is that #1?

Answer 6

No I covered all of your questions. Just quickly

Answer 7

ohh okay:) thank you

Answer 8

Im in lecture I got to go