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Help with a few Chemistry questions?
I'm totally stumped. Any help would be greatly appreciated :)
1. Which of the following describes the correct net ionic equation for the reaction of copper (II) chloride solution with potassium phosphate solution?
Answer
CuCl2 (aq) + K3PO4 (aq) arrow Cu3(PO4)2 (s) + KCl (aq)
3CuCl2 (aq) + 2K3PO4 (aq) arrow Cu3(PO4)2 (s) + 6KCl (aq)
3Cu2+ (aq) + 6Cl- (aq) + 6K+ (aq) + 2PO43- (aq) arrow 6K+ (aq) + 6Cl- (aq) + Cu3(PO4)2 (s)
3Cu2+ (aq) + 2PO43- (aq) arrow Cu3(PO4)2 (s)
2. Lead (II) acetate solution reacts with sodium sulfide solution. Which precipitate or precipitates will form?
Answer
PbS
NaC2H3O2
PbS and NaC2H3O2
no precipitates will form
3. Sodium carbonate solution reacts with strontium chloride solution. Predict whether the reaction will produce a precipitate.
Answer
No, all products are soluble because all reactants are soluble.
No, all products are soluble because they each contain metal and nonmetal components.
Yes, strontium carbonate will precipitate because each ion is polyvalent.
Yes, both sodium chloride and strontium carbonate will precipitate because they both contain metals.
2 Answers
- pisgahchemistLv 77 years ago
Q1
Net ionic equation:
3Cu2+ + 2PO4^3- --> Cu3(PO4)2(s)
Q2
Only lead(II) sulfide, PbS, will precipitate
Q3
Reacting sodium sulfate, Na2SO4, and strontium chloride, SrCl2, will produce a precipitate of strontium carbonate, SrCO3. SrCO3 is insoluble in water.
All of the possible answers are nonsense. SrCO3 precipitates because it is insoluble in water, not because the ions are "polyvalent". The solubility of SrCO3 at 20 C is about 0.0011g/100mL
========== Follow up ===========
Deadpool got the first two without difficulty, but not the third question. "Option 1" makes no sense. The reactants are soluble in water, but one of the products is not.
- 7 years ago
1. Option D. In the net ionic equation K+ and Cl- cancel each other as they are same on both sides
2. PbS
3. Option 1
