Find the concentration of I- in 0.05 M AgNO3 saturated with AgI. Include activity coeffcients in the solubility-product expression. The Ksp of AgI is 8.3x10-17. Refer to the table of activity coefficients at various ionic strengths as needed. Ionic Strength( µ „M)Ionsize| ( αpm)Ion0.0010.0050.010.050.1Charge= +/-1Activity coefficient (y)H9000.9670.9330.9140.860.83(C6H5)2CHCO2", (C3H7)4N*8000.9660.9310.9120.850.82(O2N)3CGH2O",(C;H¬)NH*,CH3O6H4CO2-7000.9650.9300.9090.8450.81Li",C,H5CO2", HOC,H4CO2-, CIC&H4CO2-, CgH5CH2CO2,6000.9650.9290.9070.8350.80CH2=CHCH2CO2-.(CH3)2CHCH2CO2-, (CH3CH2)4N+, (C3H7)2NH2+C12CHCO2", C13CCO2, (CH3CH2);NH", (C3H7)NH3*Na", CdCI", CIO2", I03', HCO3", H2PO4', HSO3", H2ASO4',Co(NH3)4(NO2)2*, CH;CO2', CICH2CO2', (CH3)4N*, (CH3CH2)½NH2",H2NCH2CO2"H3NCH2CO2H,(CH3)3NH+, CH3CH,NH3*5000.9640.9280.9040.830.794500.9640.9280.9020.820.7754000.9640.9270.9010.8150.77OH", F', SCN", OCN", HS`, CIO3 , CIO4", BrO3", IO4 , MnO4", HCO2",H2citrate", CH3NH3", (CH3)2NH2"K*, CI, Br", I, CN", NO2", NO33500.9640.9260.9000.810.763000.9640.9250.8990.8050.755Rb*, Cs*, NH4", TI“, Ag*0.9240.752500.9640.8980.80

Answered: Image /qna-images/answer/5b083af5-c72c-44a8-8184-79366c0567c3.jpg

Find the concentration of I- in 0.05 M AgNO3 saturated with AgI. Include activity coeffcients in the solubility-product expression. The Ksp of AgI is 8.3x10-17. Refer to the table of activity coefficients at various ionic strengths as needed.

Find the concentration of I- in 0.05 M AgNO3 saturated with AgI. Include activity coeffcients in the solubility-product expression. The Ksp of AgI is 8.3x10-17. Refer to the table of activity coefficients at various ionic strengths as needed.

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

BaSO4, an imaging agent, has a Ksp of 1.5 x 10-9. Calculate the molar solubility, s, given the dissociation of the precipitate. BaSO4 Ba2+ + SO42- 3.9 x 10-52.3 x 10-181.5 x 10-96.2 x 10-3
What you expect to observe on mixing 0.1M CuSO4 with 0.1M AgNO3. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?
A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a pink colourNaIO3(aq) added and no precipitate formsflame colour is redNa2CO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a.lithium and manganese(II) b. strontium and cobalt(II) c. strontium and manganese(II) d. lithium and cobalt(II)
Find the minimum concentration of Cr(NO3)3 that must be added to a 0.095M NaF Solution to initiate precipitation of CrF3. The Ksp of CrF3 = 6.6 x10^-11 why is this the minimum concentration needed for precipitation?
Calculate the concentration of dissolved sulfate ion in solution if 75.0 mL of a 0.0250 M Ba(N03)2 aqueous solution is mixed with 25.0 mL of 0.0100 M sodium sulfate aqueous solution and allowed to come to equilibrium. Ksp for barium sulfate is 1.5x10- Answer:
Hi! All necessary information for the below question. Even if you can't finish the problem, please solve as much as you can. I'll be happy if you can at least set the question up well. Thanks!
Add 0.3 M AgNO3 to each of the cold sample solutions until AgCl is observed to coagulate. Determine the approximate amount of needed AgNO3 by calculating the volume that would be required if the unknown were pure NaCl.
A 0.20 M sodium chloride solution is slowly added to a solution containing 0.40 M Pb2* and 0.40 M Ag* ions. What is the remaining concentration of the first ion at the point where the second ion just begins to precipitate? The Ksp of PbCl2 is 1.2x10-5, and the Ksp of AgCl is 1.8x10-10. 1.6x10-6 M 6.0x10-9 M ) 3.1x10-2 M 1.4x10-2 M 3.4x10-5 M
A student does not filter his/her saturated solution before titrating. Will the calculated Ksp probably be too high, too low, or unaffected? Why? Solid substances are not part of equilibrium equations, so their presence would leave the value of Ksp unaffected. The remaining solids would absorb excess H30+ ions during the titration, making the calculated value of [OH ], and thus Ksp, too low. O The remaining solids would dissolve during the titration to give more OH¯. The calculated Ksp would therefore be too high.
At a certain temperature CrF3 has Ksp = 4.9 x 10-9.Calculate the minimum concentration of Cr3+ that must be added to 0.075 M NaF in order for chromium(III) fluoride to precipitate. Neglect volume changes.Provide your answer in E-notation, rounded to 2 significant digits.
15a. Knet needs to be a number