P16B.9* (a) A dilute solution of a weak electrolyte AB, which dissociates to A* +B, is prepared with an initial concentration c. Suppose that a fraction a of AB dissociates. Assuming that activities can be approximated by concentrations, show that the equilibrium constant K for dissociation may be written a'cA K=- AB (1-a)c (b) The conductivity of the solution described in (a) is measured as K, and the molar conductivity is then calculated as A = x/CAg. However, because the degree of dissociation, and hence the concentration of the ions, varies strongly with the initial concentration cAB» values of A calculated in this way also vary strongly with cA. Given that K can be expected to be proportional to the concentration of the ions, explain why a = AIAm where Am, is the molar conductivity in the limit of complete dissociation of AB. (c) Substitute this expression for a into the above expression for K. You now have two expressions for K: one in terms of a and one in terms of A/Am1- Equate these two expressions and hence show (by rearranging your expression) that *m,l 1 A_(1-a) 1 !! m 'm,l

P16B.9* (a) A dilute solution of a weak electrolyte AB, which dissociates to A* +B, is prepared with an initial concentration c. Suppose that a fraction a of AB dissociates. Assuming that activities can be approximated by concentrations, show that the equilibrium constant K for dissociation may be written a'cA K=- AB (1-a)c (b) The conductivity of the solution described in (a) is measured as K, and the molar conductivity is then calculated as A = x/CAg. However, because the degree of dissociation, and hence the concentration of the ions, varies strongly with the initial concentration cAB» values of A calculated in this way also vary strongly with cA. Given that K can be expected to be proportional to the concentration of the ions, explain why a = AIAm where Am, is the molar conductivity in the limit of complete dissociation of AB. (c) Substitute this expression for a into the above expression for K. You now have two expressions for K: one in terms of a and one in terms of A/Am1- Equate these two expressions and hence show (by rearranging your expression) that *m,l 1 A_(1-a) 1 !! m 'm,l

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

What is the solubility of Mg(OH)2 ( Ksp 1.80 x 1011) in 0.0862 M Mg(NO3)2(aq), Leave answer in exponential form with 3 significant figures. Example on how you will write your answer : 2.32x10-5 OR 2.32E-5
The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)
A lake has a pH of 6.35 and a measured alkalinity of 5.0 x 103 eq/l. What is the concentration of CO2, HCO;, CO;-, H*, OH , assuming no interaction with the atmosphere or the bottom matrix or any biological processes?
Complete the following solubility constant expression for Ag2CrO4. Ksp = ☐ == ✗
Can you show the calculations step by step? Where did 3.1e-5 came from
Calculate the solubility of CaSO4 (in g·L-1) in the following media. The solubility product of CaSO4 is 4.9×10-5. Assume ideal behavi (a) water I-7.6 (b) a 7.8x10-5 M SrSO4 solution g•L-1
Consider the table of equilibrium constant values given below for a given set of conditions. What will be the concentration of [HCO3-] in water that is in equilibrium with both CaCO3 (s) and 225 ppm CO2 (g) under these conditions? Equation Type Value CO2 (g) H2CO3 (aq) KH 1.7 x 102 H2CO3 (aq)=HCO3(aq) + H (aq) Kat 6.44 x 107 HCO3 (aq) CO32 (aq) + H* (aq) Ka2 8.43 x 10-11 CaCO3 (s) Ca2+ (aq) + CO2 (aq) Ksp 8.4 x 10-9 H₂O (1) H(aq) + OH (aq) Kw 7.6 x 10-14 O 1.6 x 103 M O 8.1 x 10-3 M O 5.6 x 104 M O 3.9 x 104 M O 7.9 x 104 M
Assuming 100% dissociation, calculate the freezing point (?f) and boiling point (?b) of 3.29 ? AgNO3(aq).
TUOv to lls worla taum uo 1o9TIOoni bolam od lliw elimu iboo lut o 19 4. Given the Borax reaction below, what would be the solubility product (Ksp) of borax at 40 °C, if the solubility of borax is 0.8 mol L¯1 at 40 °C? Na,B4O5 (OH)4 · 8H,O(s) = 2Na+ (aq) + B405(OH) (aq) +8H,O(1) sr vol (A) gnsb vgotino brrbae ar bo CHO)gab xglerino bisbasie orb il S
ST5G.2 - Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.716 molar CaCl2(aq). Type your answer...