Metallic cadmium is added to 0.350 L of an aqueous solution in which [Cr³+]o is 1.00 mol/L. What is the [Cr³+] eq concentration of the chromium(III) species at equilibrium? Kc=0.288  2Cr3+(ac)+Cd(s)<------->2Cr2+(ac)+Cd2+

What 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+] = M

Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH", the A1³+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.97x10-2 mol AI(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.50). For Al(OH)4, Kf = 1.1x1033. [A1³+] = M

Calculate the Ksp for the slightly soluble salt Ce(IO3)4, if at equlibrium, the salt has measured concentration shown: [Ce4+] = 1.8 x 10-4 M  [IO3-] = 2.6 x 10-13 M

[Review Topics] [References] In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+ (aq) is pink and CoCl42 (aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilibrium as: CoCl42 (aq) Co2+ (aq) + 4Cl(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. Next - - - ) SONY DISPLAY WEB OFF One Touch Web Access Without Booting Up F11 F12 Num Lk Scr LK Prt Sc Sys Rg F10 Other Bookmarks THE 4:16 AM 4/30/2022 VGN-NW350F Pause Delete Break

Answer questions 3-6 in the following image

Silver and ammonia may react to form Ag(NH3)2+ complex (​K​f = 1.66 x 10​7). A 500 mL of 0.20mol Ag+ and 500 mL of 0.80 mol NH3 are mixed together.a. Write the complexation reaction.b. Write the formation constant expression.c. What is the concentration of the complex at equilibrium?d. What is the concentration of the metal at equilibrium?

What 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?

6. What is the concentration of the Cd+2 (aq) ion in a 0.010M Cd(NO3)2 solution that is also 1.0 M NH3? (Kf for Cd(NH3)4+2 = 1.0 x 107) A) 5.6 x 103 M D) 1.0 x 102 M B) 1.1 x 109 M C) 7.2 x 10-12 M E) 1.0 x 10-5 M

Write the chemical equation for the disproportionation of Cr(OH)3Cr(OH)3 in basic solution. Chromium(III) hydroxide and chromium(II) hydroxide are poorly soluble salts.