B) Given that Ksp of Al(OH)3 is 1.3X10-33, and the following dissociation : Al(OH)3 =→ Al3+...
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...
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
What is the pH of a saturated solution of Al(OH)3? For Al(OH)3 , Ksp=2.0x10-33.
Determine the molar solubility for Al(OH)3 in pure water. Ksp for Al(OH)3 = 1.3 x 10-33 2.6 x 10-9 M is the answer, but how? Please explain.
A pH 4.88 buffer which was prepared by dissolving 0.10 mol of benzoic acid (Ka=6.3x10-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. A 2.00 mL of 2.00 M HI solution was added to a 70.0 mL aliquot of this solution. a) What was the pH of the new 72.0 mL solution. b) If 0.01 mol A13+ is added to this new solution, will Al3+ ion be separated as Al(OH)3(s) (Ksp =...
Ksp of Al(OH)3 is 4.6 x 10^-33
A solution contains 0.20 M Pb2+ and 0.44 M A1+ Calculate the pH range that would allow Al(OH); to precipitate but not Pb(OH)2. The Kop values for Al(OH); and Pb(OH), can be found in this table. minimum pH: maxiumum pH: TOOLS X10
What is the concentration of Al^3+ when 25 grams of Al(OH)3 is
added to 2.50 L of solution that originally has [OH-] = 1*10^-3
Ksp(Al(OH)3 )=1.3*10^-33
Watch Video Ch15.LO3 and answer the following question about the common ion effect. Common Ion What is the concentration of Al3+ when 25 grams of Al(OH)3 is added to 2.50 L of solution that originally has [OH-] = 1 x 10-3 Ksp(Al(OH)3) = 1.3 x 10-33 2.63 x 10-M - • 1.3 x 10-30...
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
07 6. Determine the molar solubility for Al(OH)3 in pure water. Ksp for Al(OH)3 = 1.3 x 10-33. A) 3.6 x 10-12 M Ol S 7 B) 2.2 x 10-10 M C) 4.8 x 10-35 M (D) 2,6 x 10-9 M E) 6,0 x 10-19 M 29-7 (3 109 21.370-3? 98151.7370-
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.