1) Use systematic treatment of equilibrium to find the concentrations of Mg2t, F, and HF in a saturated solution of MgF2 held at pH 3.5. Ksp of MgF2 is 6.5 x 10-9
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- Calculate the pH of a carbonate buffer system that contains 0.0065 M HCO3 and 0.0084 M CO32-. The Ka of HCO3- is 4.7 X 10-11.Prepare 500 mL of 0.1 M bicarbonate buffer solution, pH = 6, from 0.1 M stocksolutions of carbonic acid acid and its solution. Ka = 4.27 x 10-7A buffer solution was prepared by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.00 M acetic acid. Assuming the change in volume is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. (The Ka for acetic acid is 1.7 x 10-5).
- A chemist adds enough of the theoretical ionic compound MX3 to form a saturated solution. She knows X- is a weak base, so she titrates the solution and finds that [X-] = (1.0x10^-4) M. What is the value for Ksp of MX3? Note: Your answer is assumed to be reduced to the highest power possible.consider the reaction Ag2O(s) + H2O -> 2Ag+ + 2OH- Ksp = 3.8 x 10-16 If Ag2O forms to an appreciable extent what effect will this equilibrium have on the solubility of AgCN? Explain your reasoning. Judging by the equilibrium reaction shown, would you expect the effect of this equilibrium on the solubility of AgCN to be pH dependent?The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?
- For ferrous hydroxide, Fe(OH)2, KSP = 1.4x10-15, corresponding to a solubility of about 0.6 mg/L. To what pH must a solution in equilibrium with solid Fe(OH)2 be adjusted to reduce the concentration of Fe2+ to 1.0 μg/L?At what pH is the concentration of [Pb2+] 2.5 x 10-4 M in a saturated solution of Pb(OH)2(s), given that Kso for Pb(OH)2(s) is 10-14.9?if the Ksp of AgCl is 1.5 x 10 -8, calculate the molar concentration (M) of AgCl in a saturated solution.
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