Mg(OH)
Mg2+ + 2OH-
x 2x
Ksp of Mg(OH)2 = 1.7*10-11
[Mg2+] = 1.0*10-10 M
Ksp = [Mg2+][OH-]2
1.7*10-11 = 1.0*10-10 [OH-]2
[OH-]2 = 0.17
[OH-] = 0.412 M
Assume the solubility product of Mg(OH)_2 is 1.7 times 10 -^11 at a certain temperature. What...
The solubility products for Mg(OH)_2 and Ca(OH)_2 are 8.9 times 10^-12 and 1.3 times 10^-4, respectively Suppose a solution contains both Mg^2+ and Ca^2+ ions, each at 0.10 M in concentration (a) At what pH Mg(OH)_2 starts to from a precipitate? (b) At what pH Ca(OH)_2 begins to from a precipitate? (C) What is the concentration of Mg^2+ when Ca(OH)_2 begins to from precipitate?
Calculate the molar solubility of Mg (OH)_2 in: given: Ksp = 1.80 times 10^-11 a - Aqueous solution b - In aqueous of pH = 10.25 Mg (OH)_2 Mg^+2 + 2OH^-1
Hydroxylapalite. Ca_10(PO_4)_6(OH)_2, has a solubility constant of K_sp = 2.34 times 10^-59, and dissociates according to Solid hydroxylapalite is dissolved in water to form a saturated solution. What is The concentration a Ca2* in this solution if [OH^-] is somehow fixed at 6.80 times 10^-6 M?
The solubility product of lead (II) chromate is 2.0 times 10^-16. Calculate the solubility in moles per liter of lead (II) chromate in each of the following solutions: Saturated lead (II) chromate in 0.10 M Na_2 CrO_4 solution. Saturated lead (II) chromate in water Saturated lead (II)chromate in 0.001 M Pb(NO_3)_2 solution
1. Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in pure H2O? Answer = Mol Solubility = 2.41 x 10^-4 2. Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2...
The solubility product of Mg(OH)2 at 250 C is 1.6 x 10-11. What is the solubility of Mg(OH)2 in moles per liter?
Based on the given value of the Ksp (5.61*10^-11), what is the molar solubility of Mg(OH)2 in 0.110 M NaOH? What is the pH change of a 0.220 M solution of citric acid (pKa=4.77) if citrate is added to a concentration of 0.125 M with no change in volume?
1. Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is used to control the pHand provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.160 mol L−1NaOH solution. 2. What is the pH change of a 0.220 mol L−1solution of citric acid (pKa=4.77) if citrate is added to a concentration of 0.140 mol L−1with no...
The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of Al(OH)3 in 0.000010 M NaOH? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).
16 A) Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams.Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in pure H2O? Answer is molar solubility = 2.41×10−4 M 16 B) Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2...