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.
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...
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
The Ksp of Al(OH)3 is 2 × 10–32. At what pH will a 0.4 M Al3+ solution begin to show precipitation of Al(OH)3? 6.1 1.0 3.6 3.1 10.4
Al(OH), (s) $ Al3+ (aq) + 3 OH+ (aq) How would the solubility of Al(OH), change if the pH of this system were increased? a) The solubility of Al(OH), would increase. b) The solubility of Al(OH); would decrease. c) The solubility of Al(OH); would remain unchanged. d) There is not enough information provided to determine how the solubility would change.
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)
1-If the [H+] in an aqueous solution is 5.00 x 10-3 M find the [OH-]. Record your answer to 2 decimal places. Note: Use "E-notation" for very large or very small numbers. [OH-]=____mol/L [H+]=____mol/L 2-The equilibrium between a solid and the associated ions in a solution is Ksp. True or False? 3- [H+] = -log pH True or False?
Phenol (C,H,OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(l) = C, H50- (aq) + H2O + (aq) K. -1.3 x 10-10 If you dissolve 0.157 g of the acid in enough water to make 253 mL of solution, what is the equilibrium hydronium ion concentration [Bot]- What is the pH of the solution? pH-
What is the pH of a saturated solution of Al(OH)3? For Al(OH)3 , Ksp=2.0x10-33.
Aluminium sulfate (alum) is the most widely used aluminium-based coagulant in water and wastewater treatment. a) Briefly describe how alum (Al2(SO4)3) addition assists in water and wastewater treatment. b) Draw a logC-pH diagram for the aluminium species at equilibrium with Al(OH)3(s). c) For the recipe [Al2(SO4)3] = 2 x 10-3 M, what are the pH and the composition of the system, assuming equilibrium with Al(OH)3(s)? d) For what total concentration(s) (minimum and/or maximum) of Al2(SO4)3 is aluminium entirely soluble? Assume...