Question

In: Chemistry

Finding cconcentration from Ksp, advanced topics in chemistry. Find the concentration of I- in 0.0010 M...

Finding cconcentration from Ksp, advanced topics in chemistry.

Find the concentration of I- in 0.0010 M AgNO3 saturated with AgI. In clude aciticity coefficients in your solubility-product expresion. The Kap od AgI is 8.3 x10 -17.

Ans is not:

1.03 x10 -13

9.44 x10 -9

8.3 x 10-14

8.135 x 10 -14

1.028 x10 -13

1.028 x 10 -14

Solutions

Expert Solution

Since this involving the activity coefficients you would have to find the ionic strength then the activity coefficient to solve this problem.
Also note this involves the common ion effect so the answer is going to be really small.
First you get the ionic strength of 0.0010M AgNO3 using this formula...
I=1/2Sum[cz^2) where c is the concentration of the ion times z= the charge squared.
you does this separately for the Ag+ and NO3- then add the values then multiply by 1/2.
Then use the debye-huckel equation, (i suggest you look it up) the a or alpha represents the size of the ion,
in this case Ag+, just do it for Ag+ to get is activity coefficient, which should be around 0.75,
now you need the activity coefficient, look that up also but it should be 0.755

Setup your equlibrium equation AgI <-->Ag+ + I- and do ICE.

Now setup your Ksp=[Ag+]y[I-]y y=activity coefficient corresponding to their ion and solve for x which is your [I-]

it should be 8.3E-17= (x)0.75(0.0010+x)0.755, the second x dont worry about since x is small in this case, so then its now
8.3x10-17= (x)0.75(0.0010)0.755 and just solve for x. And you done


Related Solutions

how do i find ksp
how do i find ksp
ORGANIC CHEMISTRY 1 Assuming that the concentration of concentrated HCl is 12.1 M and that the...
ORGANIC CHEMISTRY 1 Assuming that the concentration of concentrated HCl is 12.1 M and that the synthesis reaction has a 1:1 molar ratio determine the molar excess of HCl to the t-butyl alcohol. Show a calculation. Was t-butyl alcohol actually the limiting reagent? Briefly explain.
Using the appropriate Ksp values, find the concentration of Cu2+ ions in the solution at equilibrium...
Using the appropriate Ksp values, find the concentration of Cu2+ ions in the solution at equilibrium after 600 mL of 0.50 M aqueous Cu(NO3)2 solution has been mixed with 300 mL of 0.20 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find the concentration of OH− ions in this solution at equilibrium. (Enter in M.)
Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium...
Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium after 700 mL of 0.35 M aqueous Cu(NO3)2 solution has been mixed with 350 mL of 0.40 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find the concentration of OH− ions in this solution at equilibrium. (Enter in M.)
Using the appropriate Ksp values, find the concentration of Cu2+ ions in the solution at equilibrium...
Using the appropriate Ksp values, find the concentration of Cu2+ ions in the solution at equilibrium after 650 mL of 0.45 M aqueous Cu(NO3)2 solution has been mixed with 500 mL of 0.25 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19).AND find the concentration of OH? ions in this solution at equilibrium. (Enter in M.)
Find the concentration of I– in 0.050 M AgNO3 saturated with AgI. Include activity coefficients in...
Find the concentration of I– in 0.050 M AgNO3 saturated with AgI. Include activity coefficients in your solubility-product expression. The Ksp of AgI is 8.3× 10–17. A table of activity coefficients at various ionic strengths can be found here.
how do i find the 1st order or 2nd order from this question?? A chemistry graduate...
how do i find the 1st order or 2nd order from this question?? A chemistry graduate student is studying the rate of this reaction H2CO3 -> H2O +CO2 T [H2CO3] 0 0.600 1 0.122 2 0.0682 3 0.0472 4 0.0361 1) Write the rate law for this reaction rate = k () 2) Calculate the value of the rate constant k.
CH4(g)+Cl2(g)=CH3Cl(g)+HCl(g) Kc=4.5*10^3 Initial Concentration of the reactants 0.0010 M calculate the equilibrium concentrations
CH4(g)+Cl2(g)=CH3Cl(g)+HCl(g) Kc=4.5*10^3 Initial Concentration of the reactants 0.0010 M calculate the equilibrium concentrations
Finding the Percent Ionization of a Weak Acid Find the percent ionization of a 0.250 M...
Finding the Percent Ionization of a Weak Acid Find the percent ionization of a 0.250 M HC2H3O2 solution at 25 °C.
Find the solubility of CuI in 0.48 M KCN solution. The Ksp of CuI is 1.1×10−12...
Find the solubility of CuI in 0.48 M KCN solution. The Ksp of CuI is 1.1×10−12 and the Kf for the Cu(CN)2− complex ion is 1×1024.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT