CHM135H1 Lecture : Understanding Solubility Product Expression (Easy)
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A) Look up the solubility of each of the following compounds in water and complete the table below. Use this information to explain why we first precipitate the Group I ions with HCl before precipitating the Group III ions with (NH4)2S.
Compound | Solubility (g/L) | Compound | Solubility (g/L) |
silver(I) chloride | .002 | silver(I) sulfide | 6.21*10^-15 |
lead(II) chloride | 10.8 | lead(II) sulfide | 4.4*10^-12 |
iron(II) chloride | 64.4 | iron(II) sulfide | insoluble |
nickel(II) chloride | 67.5 | nickel(II) sulfide | 1.815*10^-8 |
B) Why do we wait until the very end of our analysis scheme to perform a flame test for Ba2+ and Ca2+? Why are we able to get away with performing a flame test for Na+ on the initial unknown solution?
C) Why do we perform our test for NH4+ on the initial unknown solution instead of testing for it after separating the other groups of ions? Why do we add NaOH to our solution during the NH4+ test?
A solution contains 0.20 M potassium sulfide and 0.20 M potassium carbonate. Solid nickel(II) nitrate is added slowly to this mixture. What ionic compound precipitates first from the solution? Solubility product constant data is found in the Chemistry References.
Formula of first precipitate = |
Hint: It is not necessary to do a calculation here. please somebody help me!!!