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Al(OH), (s) $ Al3+ (aq) + 3 OH+ (aq) How would the solubility of Al(OH), change...
Draw a pC-pH solubility diagram for gibbsite, Al(OH)3 (s) Al(OH)3 (s) ⇌ Al3+ + 3OH- LogKs0 = -34.0 Al3+ + H2O ⇌ AlOH2+ + H+ LogKs1 = -5.0 AlOH2+ + H2O ⇌ Al(OH)2 - +2H+ LogKs2 = -10.1 Al(OH)3 0 + H2O ⇌ Al(OH)3 0 +3H+ LogKs3 = -16.9 Al3+ + 4H2O ⇌ Al(OH)4 - + 4H+ LogKs4 = -22.7 Graph the pH on the x-axis and the concentration of the aluminum species on the y-axis. Assume gibbsite dissolves in...
Al(OH)3(s) → Al3+(aq) + 3OH−(aq) ΔfH∘/kJ⋅mol−1 −1284 −538.4 −230.02 S∘/J⋅mol−1⋅K−1 85.4 −325 -10.9 Part A Compute ΔrS (answer in J⋅mol−1⋅K−1) Part B Compute ΔrG∘ at 298 K (answer in kJ⋅mol−1) Part C Determine the equilibrium constant for the dissolution of Al(OH)3 at 298 K. Part D Determine the Gibbs energy change for the dissolution of Al(OH)3 when the concentrations of Al3+ and OH− are both 2.60×10−7mol⋅L−1.(answer in kJ⋅mol−1) Part E At what temperature will Al(OH)3(s) be at equilibrium with...
19. Predict how the following will affect the solubility of Al(OH)s a. In solution of 0.1 MA b. pH of 4.0 c. pOH of 4.0-Al(OH)s is amphoteric-Al(OH)s (aq) + OH, (aq)-→ [Al(OH) (aq) 20. Predict how the following will affect the solubility of AgBr a. Addition of Na S2Os complex forms in Ag' (a) 2S20 (aq) [Ag(S 0s)2l (aq) 21. Calculate the molar solubility for the following solutions of LiF (Ksp 3.8 103) a. In 0.1 M NaF . In...
In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of free Al3+ ion when 1.32×10-2 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 13.00). For Al(OH)4-, Kf = 1.1×1033. [Al3+] = ?M
Identify the reducing agent. 2 Al3+(aq) + 2 Fe(s) = 2 Al(s) + 3 Fe2+(aq) A) Fe B) Al C) Fe2+ D) Al3+ E) This is not an oxidation-reduction reaction.
4. Consider the following standard reduction potentials, Al3 (aq)+3 e Al(s) 12(s)2 e2 1(aq) E = -1.66 V +0.54 V iT E Under standard conditions: A. Al3(aq) is a stronger oxidizing agent than 12(s), and I(aq) is a stronger reducing agent than Al(s). B. 12(s) is a stronger oxidizing agent than Al3*(aq), and Al(s) is a stronger reducing agent than I'(aq). C. Al(s) is a stronger oxidizing agent than I-(aq), and Al3 (aq) is a stronger reducing agent than l2(s)....
Total lonic Equation 2 Al(OH)3(s) + [6 H* + 3 SO, 2-l(aq) → [2 Al3+ + 3 SO_2-(aq) + 6 H,0() Net Ionic Equation Reaction Type(s)
Al(OH)3 + 3 H+ <--> Al3+ + 3 H2O You find that the solution pH = 5, and that [Al3+] = 10-2 mol/L. Assuming the activity coefficient = 1 for Al3+, what is the log(Keq) of the Al(OH)3 dissolution written above assuming the system is at equilibrium? If you got stuck on a, assume that log(Al3+)=log(Keq)-3pH + 30.
B) Given that Ksp of Al(OH)3 is 1.3X10-33, and the following dissociation : Al(OH)3 =→ Al3+ + 30H Calculate : 1- The concentration of Al ions in pure water. 2- The pH value of the suspension of Al(OH)3 in water.
28. Al(OH)3 has a solubility product constant of 3.95 x 10-'1. A water sample containing aluminum has a pH of 8.9. Which species will dominate in this water sample? a) Al+(aq) b) Al(OH)3 (S) c) A12+(aq) d) Al(s)