What is (the value for Ksp for Ag2 CO3 in this solution? 3.4 x 10-8 6.8 x 10-8 1

Question

What is (the value for Ksp for Ag2 CO3 in this solution? 3.4 x 10-8 6.8 x 10-8 1.7 times 10-8 4.4 times 10-12 8.8 x 10-12 The Ksp for BaCO3 (197.3 g/mol) is 5.1 x 10-9 How many grams of BaCO3 will dissolve in enough water to make 1.000 L of solution? 0.0141 g 7.14 x 10-5 g 0.566 0.00232 g 1.03 g A solution containing CaCl2 is mixed with a solution of L1C2O4 to form a solution that is 3.5 x 10-4 M in calcium ion and 2.33 x 10-4 M in oxalate ion. What will happen once these solutions are mixed? ksp(CaC204) = 2.3x10-9. Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. Nothing will happen since the concentrations of ions present do not exceed the value. A precipitate will form as calcium oxalate is not soluble to any extent. A precipitate will form since the concentrations of calcium and oxalate are higher than the Ksp, will allow. There is not enough information to determine. In the oxidation-reduction titration experiment, potassium permanganate (KMnO4) reacts with oxalate' (C2O42-) to produce CO2 and water in acidic solutions. 5 C2042 (aq) + 2 Mn04 (aq) + 16 W(aq) rightarrow 10 CO2(g) + 8 H20(I) + 2 Mn2+(aq) What serves as a catalyst for this reaction? light H2O Mn2+ a catalyst is not required

Explanation / Answer

32-E

33-B

34-C

35-A

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