A 1.00L sample contains the following ionic compounds: Ba3(PO4)2 CdS AgNO3 NH CI ZnS a. Upon the addition of 50.0 mL of 2M HCI - what is the precipitate? b. The precipitate is then removed from the solution and 50.0 mL of 0.1M NH, solution is added. What happens? C. What is the new molar solubility for the precipitate?

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Chapter1: Chemical Foundations
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Please help with parts A B and C

**Sample Analysis of Ionic Compounds**

A 1.00 L sample contains the following ionic compounds:

- \( \text{Ba}_3(\text{PO}_4)_2 \)
- \( \text{CdS} \)
- \( \text{AgNO}_3 \)
- \( \text{NH}_4\text{Cl} \)
- \( \text{ZnS} \)

**Questions:**

a. Upon the addition of 50.0 mL of 2M HCl, what is the precipitate?

b. The precipitate is then removed from the solution and 50.0 mL of 0.1M \( \text{NH}_3 \) solution is added. What happens?

c. What is the new molar solubility for the precipitate?
Transcribed Image Text:**Sample Analysis of Ionic Compounds** A 1.00 L sample contains the following ionic compounds: - \( \text{Ba}_3(\text{PO}_4)_2 \) - \( \text{CdS} \) - \( \text{AgNO}_3 \) - \( \text{NH}_4\text{Cl} \) - \( \text{ZnS} \) **Questions:** a. Upon the addition of 50.0 mL of 2M HCl, what is the precipitate? b. The precipitate is then removed from the solution and 50.0 mL of 0.1M \( \text{NH}_3 \) solution is added. What happens? c. What is the new molar solubility for the precipitate?
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