Write the Ion Product Expression for Silver Sulfide Ag2s
 | Slightly Soluble Salts Examples of |
- 1.
- The solubility product expression for tin(II) hydroxide, Sn(OH)2, is
- (a) [Sn2+][OH - ]
- (b) [Sn2+]2[OH - ]
- (c) [Sn2+][OH - ]2
- (d) [Sn2+]3[OH - ]
- (e) [Sn2+][OH - ]3
- 2.
- The solubility product expression for silver(I) sulfide, using x to represent the molar concentration of silver(I) and y to represent the molar concentration of sulfide, is formulated as:
- (a) xy
- (b) x2y
- (c) xy2
- (d) x2y2
- (e) xy3
- 3.
- Consider the following solubility data for various chromates at 25oC.
Ksp Ag2CrO4 9.0 x 10 -12 BaCrO4 2.0 x 10 -10 PbCrO4 1.8 x 10 -14 - (a) Ag2CrO4
- (b) BaCrO4
- (c) PbCrO4
- (d) impossible to determine
- (e) none of these
- 4.
- The molar solubility of PbBr2 is 2.17 x 10 -3 M at a certain temperature. Calculate Ksp for PbBr2.
- (a) 6.2 x 10 -6
- (b) 6.4 x 10 -7
- (c) 4.1 x 10 -8
- (d) 3.4 x 10 -6
- (e) 1.4 x 10 -5
- 5.
- The solubility of silver sulfate in water at 100oC is approximately 1.4 g per 100 mL. What is the solubility product of this salt at 100oC?
- (a) 5.7 x 10 -8
- (b) 3.5 x 10 -7
- (c) 8.3 x 10 -6
- (d) 4.1 x 10 -5
- (e) 3.6 x 10 -4
- 6.
- What is the molar solubility, s, of Ba3(PO4)2 in terms of Ksp?
- (a) s = Ksp 1/2
- (b) s = Ksp 1/5
- (c) s = [Ksp/27]1/5
- (d) s = [Ksp/108]1/5
- (e) s = [Ksp/4]5
- 7.
- For Cu(OH)2, Ksp = 1.6 x 10 -19. What is the molar solubility of Cu(OH)2?
- (a) 3.4 x 10 -7 M
- (b) 6.4 x 10 -7 M
- (c) 2.7 x 10 -11 M
- (d) 5.1 x 10 -10 M
- (e) 1.7 x 10 -10 M
- 8.
- Many lead salts are often used as pigments. If PbSO4 were used in an unglazed ceramic bowl, how many milligrams of lead(II) could dissolve per liter of water?
- (a) 43
- (b) 35
- (c) 11
- (d) 28
- (e) 53
- 9.
- Ag3PO4 would be least soluble at 25oC in
- (a) 0.1 M AgNO3
- (b) 0.1 M HNO3
- (c) pure water
- (d) 0.1 M Na3PO4
- (e) solubility in (a), (b), (c), or (d) is not different
- 10.
- The molar solubility of PbCl2 in 0.20 M Pb(NO3)2 solution is:
- (a) 1.7 x 10 -4 M
- (b) 9.2 x 10 -3 M
- (c) 1.7 x 10 -5 M
- (d) 4.6 x 10 -3 M
- (e) 8.5 x 10 -5 M
- 11.
- When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if Qsp _____ Ksp, and will continue to precipitate until Qsp _____ Ksp.
- (a) is greater than; equals
- (b) is less than; is greater than
- (c) is less than; equals
- (d) equals; is less than
- (e) equals; is greater than
- 12.
- Which of the following pairs of compounds gives a precipitate when aqueous solutions of them are mixed? Assume that the concentrations of all compounds are 1.0 M immediately after mixing.
- (a) CuBr2 and K2CO3
- (b) HNO3 and NH4I
- (c) BaCl2 and KClO4
- (d) Na2CO3 and H2SO4
- (e) KCl and KNO3
- 13.
- A swimming pool was sufficiently alkaline so that CO2 absorbed from the air produced in the pool a solution which was 2 x 10 -4 M in CO3 2- M. If the pool water was originally 4 x 10 -3 M in Mg2+, 6 x 10 -4 M in Ca2+ and 8 x 10 -7 M in Fe2+, then a precipitate should form of:
- (a) only MgCO3
- (b) only CaCO3
- (c) only FeCO3
- (d) only CaCO3 and FeCO3
- (e) MgCO3, CaCO3 and FeCO3
- 14.
- When equal volumes of the solutions indicated are mixed, precipitation should occur only for:
- (a) 2 x 10 -3 M Mg2+ + 2 x 10 -3 M OH -
- (b) 2 x 10 -1 M Ba2+ + 2 x 10 -3 M F -
- (c) 2 x 10 -3 M Ca2+ + 2 x 10 -2 M OH -
- (d) 2 x 10 -3 M Ca2+ + 2 x 10 -3 M OH -
- (e) 2 x 10 -4 M Pb2+ + 2 x 10 -5 M SO4 2-
- 15.
- At what pH will Cu(OH)2 start to precipitate from a solution with [Cu2+] = 0.0015 M?
- (a) 9.0
- (b) 8.0
- (c) 6.0
- (d) 9.4
- (e) 4.6
- 16.
- What is the pH of a saturated solution of Mg(OH)2?
- (a) 3.5
- (b) 10.1
- (c) 10.9
- (d) 10.5
- (e) 9.2
- 17.
- Which solid will precipitate first if an aqueous solution of Na2CrO4 at 25oC is slowly added to an aqueous solution containing 0.001 M Pb(NO3)2 and 0.100 M Ba(NO3)2 at 25oC?
- (a) BaCrO4(s)
- (b) NaNO3(s)
- (c) PbCrO4(s)
- (d) Pb(NO3)2(s)
- (e) none of these
- 18.
- A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly until the solid AgCl just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 x 10 -10 and for AuCl = 2.0 x 10 -13.
- (a) 2.0 x 10 -10 M
- (b) 4.5 x 10 -7 M
- (c) 1.8 x 10 -7 M
- (d) 3.0 x 10 -4 M
- (e) 1.1 x 10 -6 M
Answers:
1. (c) 2. (b) 3. (a) 4. (c) 5. (e) 6. (d) 7. (a) 8. (d) 9. (a) 10. (d) 11. (a) 12. (a) 13. (d) 14. (a) 15. (c) 16. (d) 17. (c) 18. (e)
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Write the Ion Product Expression for Silver Sulfide Ag2s
Source: https://www.chem.tamu.edu/class/fyp/mcquest/ch20.html
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