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Question 4 of 5 > The generic metal A forms an insoluble salt AB(s) and a complex ACs(aq). The equilibrium conce...
Find Ksp The generic metal A forms an insoluble salt AB(s) and a complex ACs(aq). The equilibrium concentrations in a solution of ACs were found to be (A) = 0.100 M, [C] = 0.0140 M, and [ACs) = 0.100 M. Determine the formation constant, K, of AC5. Number K,= 1.86 x 10 The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.175 M. What is the Ksp of AB? Number
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A] 0.100 M, [C] 0.0210 M, and [ACSl0.100 M. Determine the formation constant, K, of AC5 Number The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.116 M. What is the Ksp of AB? Number sp
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M[A]=0.100 M, [C]=0.0260 M[C]=0.0260 M, and [AC5]=0.100 M[AC5]=0.100 M. Determine the formation constant, Kf, of AC5. ?f= The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.1310.131 M. What is the Ksp of AB? ?sp=
can someone please help me answer these, for some reason theh are both wrong and i cant get them right, will rate you good if you can help get both correct answers! thanks The formation constant of M(CN)61 is 2.50 x 10'7, where M is a generic metal. A 0.130 mole quantity of M(NO3) is added to a liter of 1.180 M NaCN solution. What is the concentration of M2+ ions at equilibrium? [M ] = 4.6 x10-19 The generic...
Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) The generic metal hydroxide M(OH)2 has Ksp = 6.85×10−12. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.) 1. Le Châtelier's principle tells us that an increase in either [A+] or [B−] will shift this equilibrium to the left, reducing the solubility of AB. In other words, AB...
At 25 °C, only 0.0450 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB(s) 7 A+ (aq) +B+ (aq) Ksp = At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.18. What is the Ksp of the salt at 22 °C? ot a generic metal hydroxide, M(OH), is mixed...
A metal ion M forms a stable complex with the ligand X: M + (aq) + 4 X (aq) ⇌ M (X) 4+ (aq) Kf = 1.0 ∙ 10^20 In a solution where [M +] = 0.100 M and [X] = 0.800 M before reaction, what is [X] at equilibrium?
Consider an amphoteric hydroxide, M(OH),(s), where M is a generic metal. M(OH),(s) M2+ (aq) + 2OH-(aq) M(OH),(s) + 2OH(aq) = M(OH)2-(aq) Ksp = 2 10-16 M3 Ke=0.02 M- Estimate the solubility of M(OH), in a solution buffered at pH = 7.0, pH = 10.0, and pH = 14.0. solubility at pH = 7.0 solubility at pH = 10.0 Enter numeric value solubility at pH = 14.0
Precipitation is the formation of an insoluble substance. For the equation AB(s)⇌A+(aq)+B−(aq), precipitation represents a shift to the left and the production of a solid. From Le Châtelier's principle, we know that when the product of the concentrations of A+ and B− gets above a certain level, the reaction will respond by shifting left to decrease the concentrations of A+ and B−. This critical level, Ksp, is a constant at a certain temperature. In this case, Q=[A+][B−], where Q is...
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...