CHEM134 Week 10 Lesson 5 QuizScore 95%
Course : American Public
Contributed : Hennah Gill
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- Question: For PbCl2 (Ksp = 2.4 × 10–4), will a precipitate of PbCl2 form when 0.10 L of 3.0 × 10–2 M Pb(NO3)2 is added to 400 mL of 9.0 × 10–2 M NaCl?
- Question: How many moles of CaF2 will dissolve in 3.0 L of 0.052 M NaF solution? (Ksp for CaF2 = 4.0 x 10–11)
- Question: Which of the following compounds is more soluble in acidic solution than in pure neutral water?
- Question: Calculate the solubility of Ag2CrO4 (Ksp = 9.0 x 10–12) in a 0.028 M AgNO3 solution.
- Question: The two salts AgX and AgY exhibit very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?
- Question: What is the molar solubility of AgCl in 0.20 M NH3? Ksp for AgCl is 1.8×10-10 and Kf for Ag(NH3)2+ is 1.7×107.
- Question: The solubility product for chromium(III) fluoride is Ksp = 6.6 × 10–11. What is the molar solubility of chromium(III) fluoride?
- Question: What is the most soluble salt of the following set?
- Question: What is the equilibrium constant expression for the Ksp of Ca3(PO4)2?
- Question: What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN)2- forms? Ksp for AgCl is 1.8 × 10- 10 and Kf for Ag(CN)2- is 1.0 × 1021.
- Question: What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.
- Question: What is the pH of 0.701 M Na2SO3(aq) at 25 °C? (Ka1 = 1.2 x 10-2, Ka2 = 6.2 x 10-8)
- Question: The best explanation for the dissolution of ZnS in dilute HCl is that:
- Question: Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 7.48. (Ksp = 1.6 x 10–19)
- Question: Will a precipitate of magnesium fluoride form when 300. mL of 1.1 × 10–3 M MgCl2 are added to 500. mL of 1.2 × 10–3 M NaF?
- Question: Which of the following would decrease the Ksp for PbI2?
- Question: A solution may contain the following ions Ag+, Cu2+, Cd2+, Mn2+, Ni2+ and Na+. A white precipitate formed when 0.10 M NaCl was added and after this was removed the solution was treated with H2S gas under acidic conditions and no precipitate formed. When the solution was made basic and again treated with H2S gas a dark colored precipitate formed. If no further tests were made then what conclusions can you draw?
- Question: Calculate the molar solubility of thallium(I) chloride in 0.30 M NaCl at 25°C. Ksp for TlCl is 1.7 × 10-4.
- Question: Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI. [For PbI2, Ksp = 1.39 × 10–8]
- Question: The solubility of strontium carbonate is 0.0011 g/100 mL at 20 oC. Calculate the Ksp value for this compound.
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