We have a blue colored solution of CuSO4 in a concentration of 0.1 M. What is the necessary concentration of chlorides that must be added to 1 L of solution so that it becomes yellow?   [Cu(H2O)4]2+ + 4Cl-  ⇄ [CuCl4]2-  + 4 H2O     Kf = 4.2 × 105       Blue                               yellow   For the yellow color to be visible, we consider that 99% of [Cu(H2O)4]2+ is in the form of [CuCl4]2-

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Write the equilibrium expression for each of the following reactions. Be sure to pay attention to physical states: a)2 O3 (g)  3 O2(g)                                            b)5 Fe+2(aq) + MnO4-(aq) + 8 H+(aq)  5 Fe+3(aq) + Mn+2(aq) + 4 H2O(l)

The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if 2.21 g of CuCl2 is dissolved in 1.000 L of a 0.926 M solution by NaCN. The addition of CuCl2 does not affect the volume (the final volume is always 1,000 L).

"the complex ion Cu(NH3)4^2+ is formed in a solution made of .0500 M Cu(NO3)2 and .500 M NH3. What are the concentrations of Cu2+, NH3, and Cu(NH3)4^2+ at equilibrium? the formation constant*, Kf, of Cu(NH3)4^2+ is 1.70x10^13

If a solution containing 0.10 M Cl-, Br, I-, and CrO2 is treated with Ag+, in what order will the anions precipitate? Salt AgCI AgBr Agl Ag₂ CrO 4 Ksp 1.8 × 10-10 5.0 × 10-13 8.3 × 10-17 1.2 × 10-12

Determine the equilibrium concentration of chloride ions when solid AgCl is dissolved in 0.10 M NH3. Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(NH3)2+ is 1.7 × 107. 1.3 x 10-5 M O 5.0 × 10-8 M 5.5 x 10-2 M 5.5 x 10-3 M

The molecular complex between silver ion and cyanide ion forms by the reactionAg+(aq) + 2 CN-(aq) ⇌ Ag(CN)2-(aq) Kf = 1.0 x 10^21A solution initially has [Ag+] = 2.0 x 104 M, and [CN-] = 0.0400 M. What will be the concentration ofAg+ ion at equilibrium?

A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value