The first step in the preparation of magnesium metal is the precipitation of Mg(OH)2 from sea water by the addition of Ca(OH)2. The concentration of Mg2+(aq) in sea water is 5.37 x 102 M. Calculate the pH at which [Mg2+] is decreased to 1.0 x 105 M Mg(OH)2(s) Mg2+ (aq) + 20H(aq) ksp =8.9 x 10-12

The first step in the preparation of magnesium metal is the precipitation of Mg(OH)2 from sea water by the addition of Ca(OH)2. The concentration of Mg2+(aq) in sea water is 5.37 x 102 M. Calculate the pH at which [Mg2+] is decreased to 1.0 x 105 M Mg(OH)2(s) Mg2+ (aq) + 20H(aq) ksp =8.9 x 10-12

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A highly acidic (pH< 0.5) industrial wastewater has an initial AlP" concentration of 10 ppm. An engineer decides that strong base should be added to the wastewater in order to raise the pH so that most of the aluminum will precipitate and be removed from solution. The pertinent solubility reaction from Appendix A of our text is: Al(OH)3 (s) → Al* + 30H¯ with pK, = 32.9 a. What is the lowest pH needed to precipitate all but 50 ppb of the aluminum from the wastewater? Assume equilibrium conditions can be achieved. b. Suppose the engineer decides that the pH should be raised to 7. What equilibrium concentration of aluminum would be left in solution? Report your answer in ppb and moles per liter.
Consider the following reaction, which is endothermic in the forward direction Fe+3(aq) + NCS-(aq) ↔ FeNCS+2 (aq) yellow. colorless blood red If Fe+3 can make complex ions with chloride ions and hydrogen phosphate ions, can be reduced by Sn2+ ions, and can precipitate with hydroxide ions (becoming colourless in all cases), what would be the colour of the equilibrium under the condition of the following stressors? (ie. Which way would it shift) The addition of HCl The addition of strong base The addition of Fe(NO3)3 Heating the solution Increasing the pressure surrounding the solution
Consider the following equilibrium: 4Ag(s) + O2(g) ---> 2Ag2O(s). At 298 K, the equilibrium constant for this reaction is K = 8.44 X 10^3. What is the change in Gf under standard state conditions for Ag2O(s)?
Write the equilibrium constant expression for the formation of FeSCN2+.
7. Given the following equilibrium constants, Cd(103)2 Ksp = 2.3 × 10¬8 Cd(NH3)4* Kr = 1.0 × 10' ( Cd²*(aq) + 4NH3 (aq)→ Cd(NH3)a²* (aq)) determine the equilibrium constant K for the dissolution of the sparingly soluble salt Cd(IO3)2 in aqueous ammonia (shown below): Cd(1O3)2(s) + 4NH3(aq) %3D %3D - Cd(NH3)42*(aq) + 2103-(aq) a) 0.23 b) 2.3 x 1015 c) 4.3 x 1014 d) 4.3 e) 1.0 x 107 f) none of the above
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
At 25 °C, only 0.0110 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB, (s) = A2+(aq) + 2B¯(aq)
The solubility of Mg(OH)2 in water is 1.4 x 10^-4 at 25C. What is the Ksp?
Upon analyzing a seawater sample, it was found that the concentration of bicarbonate ions (HCO3-) is 0.09 m, the activity of calcium ions (Ca2+) is 10^-6, and the pH of the seawater sample is 8.0. (a) Will calcite precipitate in this seawater sample? (b) Calculate the required activity of Mg2+ ions for dolomite to precipitate.
The Ksp of Ca(OH)2 is 5.066 × 10–5 at 25 °C. What is the concentration of OH–(aq) in a saturated solution of Ca(OH)2(aq)?
Consider the insoluble compound aluminum phosphate , AIPO4. The aluminum ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of AIPO4 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Al(OH)4 , Kf = 7.7×1033. Be sure to specify states such as (aq) or (s). + Rectangular Snip K =
Copper(I) ions in aqueous solution react with NH₂ (aq) according to Cu+ (aq) + 2NH₂ (aq) → Cu(NH3)2(aq) Kf6.3 x 10¹0 x Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 × 10%) in 0.88 M NH₂ (aq). solubility of CuBr(s):