Problem: A student was given a solid containing a mixture of nitrate salts. The sample completely dissolved in water, and upon addition of dilute HCl, no precipitate formed. The pH was lowered to about 1 and H2S was bubbled through the solution. No precipitate formed. The pH was adjusted to 8 and H2S was again bubbled in. This time, a precipitate formed. Which compounds might have been present in the unknown?a) Ca(NO3)2b) AgNO3c) Fe(NO)3d) Cr(NO3)3e) Cu(NO3)2f) Bi(NO3)2g) Co(NO3)2h) KNO3
FREE Expert Solution
Solubility Rules:
•Soluble Ionic Compounds:
▪ Group 1A ions (Li+, Na+, K+, etc.) and Ammonium ion (NH4+) are soluble
▪ Nitrates (NO3-), Acetates (CH3COO- or C2H3O2-), and most Perchlorates (ClO4-) are soluble
▪ Cl-, Br-, and I- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+
▪ Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+
• Insoluble Ionic Compounds:
Problem Details
A student was given a solid containing a mixture of nitrate salts. The sample completely dissolved in water, and upon addition of dilute HCl, no precipitate formed. The pH was lowered to about 1 and H2S was bubbled through the solution. No precipitate formed. The pH was adjusted to 8 and H2S was again bubbled in. This time, a precipitate formed.
Which compounds might have been present in the unknown?
a) Ca(NO3)2
b) AgNO3
c) Fe(NO)3
d) Cr(NO3)3
e) Cu(NO3)2
f) Bi(NO3)2
g) Co(NO3)2
h) KNO3
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