Question

1.

Using Table 38.3 in the Voyce text, calculate the solubility of Manganese(II) hydroxide at 25^oC

	A.	5.7 x 10-5
	B.	3.6 x 10-5
	C.	4.4 x 10-7

-116- Table 38.3 SOLUBILITY-PRODUCT CONSTANTS FOR COMPOUNDS AT 25° C Name Formula KSP BaCO3 BaF2 Ba(OH)2 Ba3(PO4)2 BaS04 CaCO3 Cd(OH)2 CaCO3 CaF2 Barium carbonate Barium fluoride Barium hydroxide Barium phosphate Barium sulfate Cadmium carbonate Cadmium hydroxide Calcium carbonate Calcium fluoride Calcium hydroxide Calcium phosphate Calcium sulfate Chromium(III) fluoride Chromium(III) hydroxide Copper(11) carbonate Copper(11) hydroxide Copper(II) phosphate Copper(II) sulfide Iron(II) carbonate Iron(II) hydroxide Iron(II) sulfide Iron(II) hydroxide Lanthanum iodate Lead carbonate Lead chloride Lead fluoride Lead hydroxide Lead sulfate Lead sulfide Magnesium hydroxide Manganese carbonate Manganese hydroxide Manganese(II) sulfide Nickel carbonate Nickel hydroxide Silver bromide Silver carbonate Silver chloride Silver chromate Silver cyanide Silver iodide Silver sulfate Strontium carbonate Tin(II) hydroxide Zinc hydroxide Ca(OH)2 Ca3(PO4)2 Ca504 CrF3 Cr(OH)3 Cuco, Cu(OH)2 Cu3(PO4)2 Cuš FeCO3 Fe(OH)2 Fes Fe(OH)3 La(103)3 PbCO3 5.1 X 10-9 1.0 X 10-6 5 X 10-3 3.4 X 10-23 1.1 X 10-10 5.2 X 10-12 2.5 X 10-14 2.8 X 10-9 3.9 X 10-11 5.5 X 10-6 2.0 x 10-29 9.1 x 10-6 6.6 X 10-11 6.3 X 10-31 1.4 X 10-10 2.2 X 10-20 1.3 X 10-37 6.3 X 10-36 3.2 X 10-11 8.0 X 10-16 6.3 X 10-18 4 X 10-38 6.1 X 10-12 7.4 X 10-14 1.6 X 10-5 2.7 X 10-8 1.2 X 10-15 1.6 X 10-8 1.6 X 10-8 1.8 X 10-11 1.8 X 10-11 1.9 X 10-13 1.0 X 10-13 6.6 X 10-9 1.6 X 10-14 5.0 X 10-13 Pbc12 PbF2 Pb(OH)2 Pb504 PbS Mg(OH)2 MnCO3 Mn(OH)2 Mns NICO3 Ni(OH)2 Agor Ag2CO3 Agči Ag2Cros AgCN Agi Ag2S04 Srč03 Sn(OH)2 Zn(OH)2 8.1 X 10-12 1.8 X 10-10 1.1 X 10-12 1.2 X 10-16 8.3 X 10-17 1.4 X 10-5 1.1 X 10-10 1.4 X 10-28 1.2 X 10-17 Send a chat

2.

The pH of a 0.0147M KCN solution is:

	A.	10.7
	B.	5.52
	C.	3.3
	D.	8.48

3.

The pH of a buffer solution composed of 0.020M HCHO₂ and 0.014M NaCHO₂ is:

	A.	3.59
	B.	3.74
	C.	3.90

4.

When 400ml of a 0.01M SnCl₂ solution is mixed with a 300ml if a NaOH solution at pH 9.0, a precipitate will form

True
False

Answer 1

1) Solubility equilibrium: Mn(OH)(s) M na* (aq) + 2OH- (aq) Solubility product, K, = [Mn* [OH-] = 1.9x10-13 Mn(aq) + 2OH- (aq) ICE table for the solubility equilibrium: Mn(OH),(s) Initial concentrations (M): Change: Equilibrium (M): +2s Solubility product, K, =[Mn* [OH-] 1.9x10-13 = (s) (28)* = 45% 1.9x10- Solubility, -= 3.6x10-M Therefore, the molar solubility of Mn(OH), in pure water is 3.6x10M