General Chemistry Lab ( Determining the Empirical Formula of Zinc Chloride) 0. I

Question

General Chemistry Lab ( Determining the Empirical Formula of Zinc Chloride)

0. In this experiment, you titreated three separate samples of a known mass of zinc chloride which had been dissolved in a known total volume. Explain why this was a better approach to determining the small, whole number ratio of moles Zn to moles Cl than titrating three separate mass samples of zinc chloride, each dissolved to a total volume of 25.00mL.

Assume that before weighing out the sample, zinc chloride used had aborbed atmospheric water.

1, Would the number of moles and mass of Zn determined to be in the titrated sample of zinc chloride be: greater than true/less than true/or ture? Explain the answer***

Answer :

Explain your answer :

2. Would the mass of Cl in the titrated sample be greater than true/less than true/or true?

Answer :

Explain your answer :

3. How would these factors affect the small, whole number ratio of moles Zn to moles Cl being determined?

Answer :

Explain your answer :

Explanation / Answer

1) the number of moles and mass of Zn determined to be in the titrated sample of zinc chloride be less than orginal values.

because percentage error always = (experimental / theoritical ) x 100

so experimental value always less than that theoritical value.

2) less than the actual value.

here also the same above explanation

3) in ZnCl2 ration of moles 1:2 . so the value obtained is also same differs 1:2 ratio

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