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 2 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

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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...

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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...

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

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The solubility of Mg(OH)2 in water is approximately 9 mg/L. (a) Calculate the Ksp of magnesium...

The solubility of Mg(OH)2 in water is approximately 9 mg/L. (a) Calculate the Ksp of magnesium hydroxide. (b) Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg/L Mg2+ remains in solution. (c) Calculate the maximum concentration of Mg2+ (as M) that can exist in a solution of pH = 12.

1. An aqueous solution is prepared such that pH = 8.2. Determine the [H+] [OH–], and...

1. An aqueous solution is prepared such that pH = 8.2. Determine the [H+] [OH–], and pOH of this solution. Show work. 2. Below are the relative fraction of species versus pH curves for different acids. Based on these curves, rank the acids (carbonic acid (H2CO3), bicarbonate (HCO3 –), phenol (C6H5OH), hydrofluoric acid (HF)) in order of increasing acid strength. Briefly describe reasoning. 3. According to the list of bases in order of increasing base strength up the page, which...

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