Tasks and exercises
1.
A 0.10 mol sample of AgNO3 is dissolved in 1.00 L of 1,00
M NO3. If 0.010 mol NaCl
is added to this solution, will AgCl(s) precipitate?
2.
What is the minimum
concentration of NO3 needed to prevent AgCl(s) from
precipitating from 1.00 L of a solution containing 0.10 mol AgNO3 and
0.010 mol NaCl?
3.
What [NH3]tot is necessary to keep AgCl from
precipitating from a solution that is 0.13 M AgNO3 and 0.0075 M
NaCl?
4.
What minimum concentration of thiosulfate ion,
S2O32- should be present in 0.10 mol
AgNO3(aq)so that AgCl(s) does not precipitate when the solution is
also made 0.010 M in Cl-? For AgCl, Ksp = 1.8 ×
10-10; for
[Ag(S2O3)2]3-, Kf = 1.7 × 1013.
5.
What is the molar solubility of AgCl in 0.100 mol
NH3(aq)?
6.
What is the molar solubility of Fe(OH)3 in a solution
containing 0,100 M C2O42- ? For, [Fe(C2O4)3]3- , Kf = 2 ×
1020.
7.
Calculate [Cu2+] in 10 M CuSO4(aq) a solution
that is also 6.0 M in free NH3.
Cu2+(aq) + 4 NH3(aq) ↔
3[Cu(NH3)4]2+(aq) Kf = 1.1 ×
1013
8.
Determine the name of the following complexes and give the
coordination number of the central metal atom.
a)
Na2[PtCl6]
b)
K3[Fe(C2O4)3]
c)
[Co(NH3)5Cl]Cl2
9.
Calculate the molar solubility of Mg(OH)2 in 1,00 M
NH4Cl(aq).
10. What is the minimum pH of a solution that is 0.015 M
Fe2+and saturated in H2S (0.10 M) from which FeS(s) (Kspa = 6 × 102) can
be precipitated?