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 byKsp 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+) = 0.14Show 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.

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Answered: Use the systematic treatment of…

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...

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The solubility of CaCO3 is pH dependent. Calculate the molar solubility of CaCO3 (Ksp = 4.5 * 10-9) neglecting the acid–base character of the carbonate ion.
Determine the pH during the titration of 39.6 mL of 0.226 M trimethylamine ((CH3)3N, Kp = 6.3x10-5) by 0.226 M HNO3 at the following points. (Assume the titration is done at %3D 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HNO3 (b) After the addition of 15.8 mL of HNO3 (c) At the titration midpoint (d) At the equivalence point (e) After adding 57.8 mL of HNO3
Given the values of K and Kb below, which of the systems given would be most suitable to use to construct a buffer of pH 97 HCOOH, K, = 1.8 x 104 CH3COOH, K3=18x105 H3ASO4. Ka1 = 6.0 x 10, Ka2 = 1.1 x 10, Ka3 = 3 x 1012 C5H5N, Kp = 1,7x10-9 NH3 КЬ - 1.3 х. 10-5 OA H3ASO4/NaH2As04 eB. HCOOH/NAHCOO OC. C5H5N/ C5H5NHCI OD.CH3COOH/KCH3CO0 FOE NH4C/NH3
2. You are studying an unusual enzyme that produces hydronium ions (H3O+) during the courseof the reaction.You wish to maintain pH = 8.5 for the enzyme-catalyzed reaction. Which weak acid will serveas the better 0.1 M buffer for the reaction: HEPPS with pKa = 8.0, or, AMPSO with pKa = 9.0?Justify your answer by describing how the buffer “resists” change in pH and the chemical logicof why you chose the buffer you did.
1. Which of these statements about the common-ion effect is most correct? (A) the solubility of a salt MA is decreased in a solution that already contains either M+ or A- (B) common ions alter the equilibrium constant for the reaction of an ionic solid with water. (C) the common ion effect does not apply to unusual ions like SO32-. (D) the solubility of a salt MA is affected equally by the addition of either A- or an uncommon ion. Group of answer choices Statement (C) is most correct. Statement (A) is most correct. Statement (B) is most correct. Statement (D) is most correct.
The dissolution of CaCO3 in water is also affected by the equilibrium between the carbonate species. What is the solubility of CaCO3 in a water sample at 25°C initially without carbonate species (HCO3 and CO3?) at pH =10? The equilibrium constant for carbonate species is: HCO3 = H+ + Co,?- [H*][C0;²-] [HCO3¯] 3. K = 10-10.3 The solubility product of CaCO3 is Ksp = 10-6.4 at 25°C.
In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H,O, at 20 – 25°C) co so Cro C,0; OH- Mg?+| 0.00069 0.18 35.7 54.8 0.038 Са2+ 0.16 0.00066 0.205 13.2 0.00061 Sr2+ 2.25 0.00034 0.135 0.106 0.005 Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075 For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate. Mg(NO,), and (NH,),CO, : MGCO, Incorrect ВаCl, and NaОН: Ba(ОН), Incorrect AgNO, and NaBr : AgBr Ca(NO,), and KCI : СаCl Incorrect SDECIAI ASO 1..
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?
At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?
Express Ksp in terms of molar solubility, x, for the salts with the given formulas. AB(s) Ksp = AB₂ (s) Ksp = AB 3 (s) Ksp = A3B₂ (s) Ksp =
C
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