Smallers 23) (15 pts.) A saturated solution of zinc hydrokide is prepared at 25°C. Calculate, then...
6 6. Zinc hydroxide, Zn(OH)2. is practically insoluble in pure water. (Kap 3.0 x 10-16) a) Determine the pH of a saturated aqueous solution of Zn(O1H)2. (You should assume that all hydroxide ions in the solution come from the Zn(OH)2: you can ignore the autoionization of water.) (4 pts) b) Zn(OH)2 is less soluble in even very dilute solutions of Zn(NOs)2 due to the common ion effect. Determine the molar solubility of zine hydroxide in a 1.0 x 10-4 M...
A) Consider the insoluble compound zinc hydroxide, Zn(OH)2. The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Zn(OH)2(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)42+, Kf = 2.9×109. Specify states such as (aq) or (s) and provide K. K = ______ B) Consider the insoluble compound nickel(II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions....
5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions. Given the equilibria below, calculate the concentration of each zinc species in a solution saturated with Zn(OH)2 and [OH') fixed at 3.2 x 107M Zn(OH)2(8) Ksp = 3 x 10-16 Zn(OH)* K= 1 x 104 Zn(OH)2(aq) K = 2 x 1010 Zn(OH)3 K = 8 x 1013 Zn(OH)42 K= 3 x 1015
1) A saturated solution of copper (II) iodate in pure water has a copper ion concentration of 2.7X10^-3 M. a) whar is the molar solubility of copper iodate in a 0.35 M Potassium iodate solution B) what is the molar solubility of copper Iodate in 0.35 M copper nitrate solution 2) a)consider the slightly soluble salt, silver chloride, Agcl. If you had 10.0 g of silver chloride, what volume of water would be required to completely dissolve this amount b)...
4. The pH of a saturated aqueous solution of zinc ammonium phosphate (ZnNH4P04) is 7.20, whereas the concentration of the zinc ion in the solution is 8.4 x 10-5 M. Calculate the solubility product of ZnNH4PO4. 5. What is the minimum concentration of excess Agt required to quantitatively precipitate (99.9%) oxalate from a 0.0303 M NaC204 solution buffered at pH 4.00 6. Calculate the molar solubility of Ag2CrO4 in a) water, b) 0.050 M Na2CrO4, c) 0.050 M AgNO3. (Disregard...
A saturated solution is prepared by dissolving Al(OH)3 (Ksp = 2*10^-32) in pure water at 25 C. Which of the following could to add to the solution to dissolve more Al(OH)3? A. Ar B. KCl C. HBr D. NaOH E. NH3 NOTE: I know the answer is C, I need the reasoning to get there.
a saturated solution of mg(oh)2is prepared and allowed to equilibriate at 25 C. a 25 mL sample of the 25 C solution is titrated with .00508M HCL solution. 1.38 mL of the HCL solution are required to fully react the solution sample A. Determine the molar solubility of mg(oh)2 B. Calculate Ksp for mg(oh)2 C. Calculate ∆G for mg(oh)2 D. what additional measurements would be required in order to determine ∆H and ∆S for mg(oh)2
Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 1.94 x 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 6.24 x 10-6 M. (a) What is the concentration of chloride ions, [CI – ], in the resulting solution? XM (b) What is the molar solubility of silver chloride, AgCl, in 1.94 x 10-5 M NaCl? 4.9 6.24e-6...
Write a solubility product constant expression, K_sp, for an equilibrium in a saturated aqueous solution of the slightly soluble salts Magnesium fluoride, MgF_2 Zinc phosphate, Zn_3(PO_4)_2 Chromium(II) hydroxide, Cr(OH)_3 Strontinum sulfate, SrSO_4. Calculate the solubility in g/L for calcium carbonate, CaCO_3, in pure water given the K_sp = 2.8 times 10^-9. Calculate the solubility in g/L for CaCO_3, in 0.050 M Na_2CO_3.
a Saturated solution of magnesium hydroxide is prepared and the excess solid magnesium hydroxide is allowed to settle. A 25ml aliquot of the saturated solution is withdrawn and transferred to an Erlenmeyer flask, and two drops of methyl orange indicator are added. A 0.00053 M HCl solution(titrant) is dispensed from a buret into the solution (analyte). The solution turns from yellow to a very faint red-orange after the addition of 13.2ml a. How many moles of hydroxide ion are neutralized...