Vhich of the following is a CORRECT charge balance expression for a 0.10 M aqueous solution f[NH2(CH3)2]CI? bof NH(CH3)2 = 5.10 × 10–4 %3D ) [NH2(CH3)2*]+ [H3O*] = [CI]+ [OH'] D (NH2(CH3)2*] + [H3O*] = [OH"] ) [H30*] = [CI']+[OH°] ) [NH2(CH3)2] + [H3O*] = [CI]+ [OH']
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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).# E 80 C Consider the insoluble compound copper(II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+, K₁= 6.8x10¹2. Be sure to specify states such as (aq) or (s). K= Submit Answer $ 4 R F + V 67 20 % 5 [Review Topics] [References] Use the References to access important values if needed for this question. T G Retry Entire Group 9 more group attempts remaining ? Cengage Learning | Cengage Technical Support 6 B MacBook Pro Y H + & 7 N U J * 00 8 ▶ I M ( 9 K € O ) O L ➡ P Previous )) Email Instructor Save and Exit { + . || [ = Next> ? I 12. 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.
- Calculate the [Ag+] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2]1- = 1.0 x 10211) 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.For the aqueous [Ag (CN)₂] complex K=1.26 × 10²¹ at 25 °C. + Suppose equal volumes of 0.0022M AgNO3 solution and 0.48M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M x10 X Ś ?
- 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 M31) 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 MWhich 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
- Silver ions form a complex ion in the presence of cyanide ions, according to the following equation: Ag (aq) + 2 CN (aq) [Ag(CN)₂] M If 0.090 mol of AgNO3 is added to one liter of 1.0 M KCN, what are the equilibrium concentrations of each species in the reaction? [Agt] = [CN] = [[Ag(CN)₂]]= 0.090 M Ke 1.1 x 10¹8 M Question #62+ For the aqueous [Ni(NH3) [Ni(NH3)]²+ complex K₁ = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0078M Ni(NO3), solution and 0.96M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. Round your answer to 2 significant digits. M 0x₁ x10 X ? ŚFor the aqueous [Ag (NH3)2] complex K, =1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0072 M AgNO3 solution and 0.72M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. м x10 X