What is the solubility of Mg(OH)2(s) in an aqueous solution of pH 13.00 at 25oC? The...

What is the solubility of Mg(OH)₂(s) in an aqueous solution of pH 13.00 at 25^oC? The solubility product of Mg(OH)₂(s) at this temperature is 1.2 x 10^-11. (Answer: 8.7 x 10^-8 g/L)

Expert Solution

queen_honey_blossom answered 3 years ago

What is the solubility of Mg(OH)2 in an aqueous solution buffered to a pH of 13.13?...

What is the solubility of Mg(OH)2 in an aqueous solution buffered to a pH of 13.13? The Ksp of Mg(OH)2 is 1.8 x 10-11. Hint: Determine the [OH-] from the pH then deal with solubility with common ion. Determine if adding each of the following to a saturated Ca3(PO4)2 solution will increase, decrease, or have little to no effect on it ssolubility. - A. B. C. HCl - ...

Compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH...

Compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH of 9.3. water M buffered solution M

What is the pH of a saturated solution of Fe(OH)2 at 25oC? For Fe(OH)2, Ksp=7.9x10-16. Give...

What is the pH of a saturated solution of Fe(OH)2 at 25oC? For Fe(OH)2, Ksp=7.9x10-16. Give three digits in your answer (e.g. 8.47, 12.6, 3.75, etc.)

Assuming complete dissociation, what is the pH of a 4.21 mg/L Ba(OH)2 solution? pH=

Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in...

Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.160 M NaOH? Express your answer with the appropriate units. Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Ksp, calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.160 M NaOH solution. Express your answer numerically to three significant figure Ksp, of 5.61×10−11.

The pH of a saturated solution of Mg(OH)^2, whose Ksp is 7.1x10^-12, is__________.

Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 11.11. Express...

Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 11.11. Express your answer using two significant figures. [Ca(OH)2] = M SubmitMy AnswersGive Up

What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.52? (See...

What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.52? (See the appendix.) M What is the molar solubility at pH = 8.16? M Substance Ksp at 25 oC Aluminum Al(OH)3 1.9 x 10-33 Barium Ba(OH)2 5.0 x 10-3 BaCO3 8.1 x 10-9 BaSO4 1.1 x 10-10 Ba3(PO4)2 3.4 x 10-23 Cadmium Cd(OH)2 2.5 x 10-14 CdCO3 5.2 x 10-12 CdS 8.0 x 10-27 Calcium Ca(OH)2 5.5 x 10-6 CaCO3 4.8 x 10-9 Ca3(PO4)2 1.0...

Mg(OH ) 2 is a sparingly soluble compound, in this case a base, with a solubility...

Mg(OH ) 2 is a sparingly soluble compound, in this case a base, with a solubility product, K sp , of 5.61× 10 −11 . It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Part C - Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Ksp , calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2...

1. Determine the molar solubility of Cr3+& OH- ions in the compound Cr(OH)3 at 25oC at:...

1. Determine the molar solubility of Cr3+& OH- ions in the compound Cr(OH)3 at 25oC at: a pH of 7.9 b.0.010 M chromium (III) nitrate c.Distilled water The Ksp is 6.30 x 10-31 2.A solution is prepared by mixing 0.050 M Pb(NO3)2 with 0.00350 M KBr. a. Determine where this solution will be unsaturated,saturated or super saturated. b. Write a balanced net ionic equation for this chemical reaction. 3) The Ksp for PbBr2is 6.6 x 10-63.Calculate the solubility Ag2CrO4(s) in...

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