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What is the solubility of Cr(OH)3 in g/l at pH 9.55? Ksp for Cr(OH)3 = 6.30 x 10-31?
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- 1) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, i.e., -log[Cu2+], in an aqueous NaOH solution that has a pH of 12.86 and is saturated with Cu(OH)2. 2) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, i.e. -log[Cu2+], if 2.46 g of CuCl2 is dissolved in 1.000 L of a 0.938 M NaCN solution. The addition of CuCl2 does not affect the volume (the final volume is always 1.000 L).1.) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)2. 3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).If Cu3(AsO4)2 has a Ksp=8.0x10-36, then what is the solubility of [Cu2+] in a saturated solution?
- Ks for Ca(OH)2(6) is 10-5.19. Please write out the reaction and K for the dissolution of this solid. Now write the equilibrium expression for this solid. What is the IAP? If [Ca2+1 = 10-2 M and pH is 8, will this solid form? Is there a range in pH where this will form?1) The following reaction was allowed to reach equilibrium at 25oC. Enclosed with the phase of each species is the equilibrium concentration. Calculate the equilibrium constant (Kc and Kp) for this reaction. 2 NOCl(g, 2.6 M) = 2 NO(g, 1.4 M) + Cl2(g, 0.34 M) 2) Calculate the pH of a 0.10 M hypochlorous acid solution. Ka = 3.5 x 10-8.1.) The solubility product, Ksp, of Cd3(PO4)2 is 2.5 x 10-33. What is the solubility (in g/L) of Cd3(PO4)2 in pure water? 2.) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)2. 3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).
- 31) Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003 M, [CO32−][CO32−] = 0.003 M (b) Co(OH)2: [Co2+] = 0.01 M, [OH–] = 1 ×× 10–7 M (c) CaHPO4: [Ca2+] = 0.01 M, [HPO42−][HPO42−] = 2 ×× 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01 M, [PO43−][PO43−]= 1 ×× 10–13 M2. Given that KspNi(OH)2] = 5.50 x 10-16, Ksp[Mg(OH)2] = 8.9 x 10-12, and Kp[Ca(OH)2] = 4.7 x 10“, a saturated solution of which of the following salts would have the highest pH? %3D (a) Ni(OH)2 (b) Mg(OH)2 (c) Ca(OH)2 (d) They would all be the same.Which of the following is the expression for the solubility product of Fe2(CrO4)3? Ksp 2[Fe2+13 +3[CrO4³-1² O O Ksp=3[Fe2+]2[CrO4³-] OKsp=[2x Fe2+13[3 x CrO4³-12 Ksp [Fe2+]³[CrO43-1² Ksp=[Fe3+12[CrO4²-1³
- If 150 mL 0.0180 M Ni(NO3)2 and 125 mL of 0.25 M ammonia (NH3) are diluted to 500 mL with deionized water. What is the concentration of Ni(NH3)42+ in solution assumed to be at equilibrium? Kr for [Ni(NH3)4²+] is 3.7 x 1016 O 724 x 102 M O 6.9 x 10¹ M O 0.018 M O 5.4 x 10-3 MWhat is the minimum pH at which Cr(OH)3 will precipitate from a solution that is 0.086 M in Cr3+ (aq). (Ksp = 7.0 x 10-31)Given that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.