a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksn. = 1.4 x 107 at 25 °C b) Will the solubility of Cu(IO3)2 (6) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (20), react with aqueous ammonia to form a complex according Cu²*(a0± 4NH3 (a9) =[Cu(NH3)4]²* (a2) with a formation constant, Ki = 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)

a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksn. = 1.4 x 107 at 25 °C b) Will the solubility of Cu(IO3)2 (6) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (20), react with aqueous ammonia to form a complex according Cu²(a0± 4NH3 (a9) =[Cu(NH3)4]² (a2) with a formation constant, Ki = 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Copper(I) ions in aqueous solution react with NH, (aq) according to Cu*(aq) + 2 NH, (aq) → Cu(NH, )† (aq) K = 6.3 × 1010 Calculate the solubility (in g-L-!) of CuBr(s) (Ksp = 6.3 × 10-º) in 0.86 M NH, (aq). solubility of CuBr(s): g/L
Use the reaction quotient to predict whether a precipitate will form. If 15.0 mL of 9.93×104 M Pb(NO3)2 are added to 22.0 mL of 2.60×105 M (NH4)2SO4 will solid PbS04 (Ksp = 1.8×10) precipitate? If a precipitate will not form, what sulfate ion concentration will cause a precipitate of lead sulfate to form? If a precipitate will form, what is the minimum [SO42] that could have been present without initiating precipitation? Assume the total volume used in the above example. M
تھے Calculate the molar solubility calcium fluoride, CaF₂, given that Its Ksp 15 410 x 10" B. calculate molar solubility of CaF₂ in a 0,45M SOLUTION OF KF (aq) (include ICE chart)
Complete the following solubility constant expression for Co (OH),. K - U sp =
The solubility of silver chloride is 1.3 x 10-5 mol L-1. What is the Ksp for silver chloride at 25 °C?
1. The Ksp for Mg(OH)2 is 5.6 x1012. Determine the molar solubility of Mg(OH)2 in a solution of 0.010 M Ca(OH)2.
After addition of HNO, to the mixture (1st addition), why did the precipitate dissolve? Consider the following equilibria: 2 Ag* (aq) + CO, (ag) = Ag2CO3(s) CO" (aq) +2H*(aq) = H2O(1) + CO2(9)
What is the molar solubility (in M to two decimal places) of cadmium carbonate in water (at 25 °C)? Ksp = 5.2 × 10–12
4.0 mL of 0.20 M HCI is added to 4.0 mL of 0.30 M Pb(NO3)2 to produce a precipitate of PbCl21s)- Water in the amount of 9.0 mL is added to dissolve the precipitate. Based on this data, what is the Ksp of PBCI2(s}? Express answer as a decimal value.
27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2
Will a precipitate form when 100.0 mL of 1.2 × 10- M Mg(NO3), is added to 100.0 mL of 1.2 x 10-4 M NAOH? The ion product for Mg(OH), is Since Q is than Ksp, Mg(OH), v precipitate from the solution.
What is the molar solubility of silver iodide, Agl, in 0.0325 M CH;NH,? For AgI Ksp = 8,52 x 10 "; for [Ag(CH;NH,)2]", Kf= 7.8 x 10°