Enter the solubility-product expression for Al(OH)3(s).
Solubility is defined as the maximum amount of solute dissolved in a given amount of solvent to make a saturated solution at a particular temperature.
Molar solubility is the number of moles of solute that will dissolve in a liter of a solution. It is expressed as mol/L or M (molarity).
Solubility product: The equilibrium constant which defines the solubility of an ionic substance in water is known as a solubility product. The solubility product is denoted by.
For a saturated solution, the solubility product is the product of activities of the ions each raised to its coefficients (powers).
Consider a general reaction:
The solubility product is expressed as follows:
Where,
Solubility product =
Molar solubility of M ion =
Molar solubility of X ion =
The powers raised to the ions =
The equation is as follows:
The solubility product expression is as follows:
Solubility-product expression for is
.
Question 1 The solubility product for Al(OH)3 is written as a. K- [A1*] s[on-) [Al(OH)] Ob. Ko - (A1*) 3[on] OCK, -[A1*](OH-] [A14] (0H-] d. Ko Al(OH),] OeKq - [Al] + [OH-] Moving to another question will save this response.
Enter the solubility-product expression for AIOH),(s).
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.
Write the solubility product constant expression for the solubility of Chromium (III) Hydroxide, Cr(OH)3. What would the solubility in g/100 mL of this salt be in water given the solubility product is 6.1 x 10 ^-31
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...
Q1 The solubility product, Kps, of Al (OH) 3 (s) is 1.0 x 10-33. What is its solubility (in g / L) in an aqueous solution of NaOH with a pH of 12.21? Q2 The formation constant, Kf, of PbCl42- (aq), Pb2 + (aq) + 4 Cl- (aq) ⇌ PbCl42- (aq), is 2.5 x 1015. What are the equilibrium concentrations of Pb2 + (aq) , Cl- (aq), and PbCl42- (aq) if we add 0.103 mol of Pb (NO3) 2 to...
Enter the solubility expression for Mg 3 ( PO 4 ) 2 ( s ) . K sp =
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)
1) Write the solubility product equilibrium and the solubility product constant expression for barium fluoride. al 2) A solution is made by placing solid barium fluoride into pure water. The barium ion concentration in this solution was found to be 1.1 x 10-8 M, what would the numerical value of Ksp be for calcium fluoride? 3) A solution is made by diluting 10.0 mL of 0.021 M potassium dichromate to 200 mL. What is the molarity of the diluted solution?
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...