Chapter 13, Problem 31P

Please correct answer and don't used hand raiting

Please correct answer and don't used hand raiting

Please correct answer and don't used hand raiting

Use the systematic treatment of equilibrium to determine the pH and the concentrations of all species in a saturated aqueous solution of SrF2. Do not include activity coefficients. The solubility of SrF2 is governed by Ksp for the salt, hydrolysis of F- and of Sr2+, and by ion pairing between Sr2 + and F-. PK(SrF2) = 8.58, PK(HF) = 3.17, pkw = 14.00, pk for the formation of (SrOH+) = 13.18, pk for the formation of (SrF+) = 0.14 Show all your work and upload your answers here. 1 - Write the pertinent reactions. 2 - Write mass balance and charge balance equations. 3 - Write the equilibrium constant expressions. 4 - Count the equations and unknowns. 5- If the problem is solvable make suitable approximations and find the concentrations and the pH.

Please correct answer and don't use hand rating

How might you prepare each of the following using a nucleophilic substitution reaction at some step? (a) (b) (c) (d) CH3 CH3C CCHCH3 CH3 CH3 0 CCH3 ☐ CH3 CH3CH2CH2CH2CN CH3CH2CH2NH2

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Manganese(II) Arsenate is insoluble in water at room temperature. (Note: Arsenate = AsO4³-) In the presence of aqueous ammonia, solid Manganese(II) Arsenate becomes more soluble and aqueous tetraamminemanganese (II) ion forms. When solid Manganese(II) arsenate was placed in a 2.00 M solution of ammonia, at equilibrium, 0.308 M of ammonia remains. If the Kf of tetraamminemanganese (II) ion is 250.0, Determine the Ksp of Manganese(II) arsenate Hint: You will have to figure out the Kspf of the overall chemical equation first, then solve for Ksp by using Kf and Kspf

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