In a solution that is 0.0500M in
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General Chemistry: Principles and Modern Applications (11th Edition)
- At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.arrow_forwardWhat is the approximate concentration of free Aut ion at equilibrium when 1.86x10-2 mol gold(1) nitrate is added to 1.00 L of solution that is 1.430 M in CN. For [Au(CN)₂], Kf = 2.0×10³8 [Au*] = Marrow_forwardWhat is the concentration of Ag+ at equilibrium in the following reaction when carried out at 238 K and [Fe2+] = [Fe3+] = 0.3 M at equilibrium?arrow_forward
- Consider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue 1. A test tube in 2. the to [CuC14]²+ (aq) + 6 H₂O (1) orange COWNIC is color? 14 TOT Châtelie anges to for the color? pic. Dior species diesent 3. The test tube in 2, is put into an ice bath. The solution changes to a light blue color. What is the major species present in the solution responsible for the color? b. Explain the effect of heat in terms of Le Châtelier's principle.arrow_forwardWhat is the approximate concentration of free Ag* ion at equilibrium when 1.78×10-² mol silver nitrate is added to 1.00 L of solution that is 1.170 M in CN. For [Ag(CN)2], Kf = 1.3×1021. [Ag*] = Marrow_forwardWhat is the approximate concentration of free Cu+ ion at equilibrium when 1.91x10-2 mol copper(I) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cu(CN)₂], K = 1.0x1024. [Cut] = M use tine References to access important values ir needed for this question. What is the approximate concentration of free Cd2+ ion at equilibrium when 1.48x10-2 mol cadmium(II) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cd (CN)4]2, K₁= 6.0x10¹8. [Cd2+] = Marrow_forward
- [Fe(H2O)6]3+ (aq) + SCN1- ↔ Fe(H2O)5SCN]2+(aq) + heat yellow red For the above reaction, describe using Le Chatelier’s Principle what changes (color changes and shifts) would occur when each stress is applied to this equilibrium. Explain your answers. a) Add KSCN(aq) b) Decrease temperature c) Add AgNO3, which causes AgSCN to precipitate out.arrow_forwardCalculate the molar concentration of zinc ions in a solution containing 0.200 M [Zn(NH3)4]2+ (K¢ = 4.10x10°) and 0.0116 M NH3 at equilibrium. Give your answer to the correct number of sig. figs. in regular notation (e. g. 0.0123).arrow_forward1.) 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).arrow_forward
- Which of the following expression can be used to calculate the equilibrium constant involving the 3- 2+ 4- 3+ Fe(CN), + Cr = Fe(CN)," + Cr reaction: Select one: log Keq = (E°cr E"(Fe(CN)61)/0.0592 log Keq = {2(E°Fe(CNIGI - E°C, )}/0.0592 Cr· O log Keq = (E°, - E°C, )/0.0592 [Fe(CN)6] log Keq = {2(E°. Cr E"(Fe(CN)6)}/0.0592 E°,arrow_forwardd) Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a total of 1.0 × 10-³ M copper (II) ions and an equilibrium concentration of 0.10 M NH3.arrow_forwardConsider the following reaction. Fe3+ (aq) + SCN (ag) FESCN2*(ag) a) İnitially [Fe3+]=1,0 x 10-3 M and [SCN]= 8,0 x 104 M a solution was prepared. In balance [FESCN2-] = 1,7 x 104 M. Calculate the equilibrium constant Kd.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning