It is determined that the equilibrium concentrations of Fe3+, SCN and [F e SCN2*] are 5.30 × 10-4 M (5.30 times 10 to the minus 4th power M), 8.30 x 10-4 M (8.30 times 10 to the minus 4th power M) and 2.60 x 10-4M (2.60 times 10 to the minus 4th power M) respectively. What is the value of K? No units, please. Your Answer: Answer

A student prepares an FeSCN2+ experimental sample by mixing:4.0 mL of 0.0025 M Fe(NO 3) 32.0 mL of 0.0025 M KSCN8.0 mL of 0.10 M HNO 3Based on a standard curve, it was determined that the concentration of FeSCN 2+ present in thesample at equilibrium was 2.52 × 10 -5 M. Based on this data, calculate the equilibrium constant forthe reaction of Fe 3+ with SCN– .

4 Calculate the equilibrium constant, K, for the following: A + 2 B 3C +D when the equilibrium concentrations of each species were determined: [A] = 0.010 M, [B] = 0.15 M, [C] = 0.20 M, and [D] = 0.25 M.

In the fictitious reaction below, the equilibrium concentration of A is 0.7140 M, B is 0.1133 M, and A 2B 3 is 0.5984 M. What is the value of the equilbrium constant k for this reaction? 2 A (ag) + 3 В (aq) А 2B з 0.001239 128.1 8.778 7.397 807.1

A student ran the following reaction in the laboratory at 642 K: 2HI=H2+I2 When she introduced 0.368 moles of HI into a 1.00 liter container, she found the equilibrium concentration of I2 to be .0363 M Calculate the equilibrium constant, KC, she obtained for this reaction.

Solid iron(II) carbonate and solid cobalt(II) carbonate are in equilibrium with a solution containing 1.06x102 M iron(II) acetate. Calculate the concentration of cobalt(II) ion present in this solution. [cobalt(II)] M Solid iron(III) hydroxide and solid iron(III) sulfide are in equilibrium with a solution containing 7.85x10-3 M sodium hydroxide. Calculate the concentration of sulfide ion present in this solution. [sulfide] M

At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The resulting equilibrium solution has a pH of 10.18. What is the Kp of the salt at 22 °C? -12 1.4 x10 Ksp = Incorrect

Fe3+ + SCN- <---> FeNCS2+  Given that Keq= 299, the initial concentration of Fe3+ is 0.04 M, and the initial concentration of SCN- is 0.001 M, calculate the final concentrations of each species in the reaction at equilibrium.

Calculate the concentration of Ag+ present in solution at equilibrium when concentrated ammonia is added to a 0.010 M solutionof AgNO3 to give an equilibrium concentration of [NH3] = 0.20 M. Neglect the small volume change that occurs when NH3 isadded.

9. For the reaction Hg²+ (aq) + 4 I- (aq) → [HgI4]²+ (aq) the value of Kc = 1.0 × 1030. If the initial concentration of I- is 0.78 M and Hg2+ is 0.010 M, what will be the equilibrium concentrations of Hg²+?