Consider a receptor (R) that binds two ligands (L & M ) in a sequential fashion. For example, ligand"L" must be present before ligand "M" can bind. In dissociation reactions, it would look like this.R•L•M R•L + M with equilibrium constant KamR•L OR+Lwith equilibrium constant Kaa. Derive an equation that relates the fraction [R•L•M]/[R]tot to the concentrations of free L and freeM.b. In terms of the dissociation constant, Kam, what concentration of ligand "M" will lead to 50% ofthe receptor existing in the R•L•M state when [L] = 10 x Ka?

a receptor equential nple, ligai L" must be present before ligand "M" can bind. In dissociation reactions, it would look like this. R•L•M R•L + M with equilibrium constant Kas with equilibrium constant Kdt R•L OR +L . Derive an equation that relates the fraction [R•L•M]/[R]tot to the concentrations of free L and fre М. . In terms of the dissociation constant, Kam, what concentration of ligand "M" will lead to 50% the receptor existing in the R•L•M state when [L] = 10 x Ka?

a receptor equential nple, ligai L" must be present before ligand "M" can bind. In dissociation reactions, it would look like this. R•L•M R•L + M with equilibrium constant Kas with equilibrium constant Kdt R•L OR +L . Derive an equation that relates the fraction [R•L•M]/[R]tot to the concentrations of free L and fre М. . In terms of the dissociation constant, Kam, what concentration of ligand "M" will lead to 50% the receptor existing in the R•L•M state when [L] = 10 x Ka?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

See similar textbooks

Similar questions

A Boric acid and glycerin form a complex B(OH)3(aq) + glycerin(aq) B(OH)3 glycerin(aq) with an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid is in the form of the complex?
For the aqueous [Ag (NH3)2] complex K, =1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0072 M AgNO3 solution and 0.72M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. м x10 X
If 4.00 g of CuSO4 are dissolved in 8.5 × 102 mL of 0.25 M NH3 solution, what are the concentrations of Cu2+, Cu(NH3)42+, and NH3 at equilibrium? The formation constant for Cu(NH3)42+ is 5.0 × 10^13. Cu2+=..............× 10............M (scientific notation. Cu(NH3)42+=......................M NH3=.........................M
2. Is the following equilibrium reaction homogeneous or hetero- geneous? CaF₂ (s) Ca²+ (aq) + 2F- (aq) + heat 3. Write the equilibrium constant expression for the reaction CaF₂ (s) Ca²+ (aq) + 2F- (aq) + heat. 2
The stock solution at equilibrium used in test tube #4 contains Fe 3+ (aq), SCN- (aq) and [FeSCN]2+ (aq). When NaOH was added to test tube #4 a shift in equilibrium was observed. What chemical species in the stock solution reacted with NaOH? Write the balanced chemical reaction associated with the change observed from the addition of NaOH to test tube #4?
The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is mixed with the thiocyanate ion. A solution containing initial concentrations of M2+ and SCN- are 0.000100 M and 0.000300 M respectively has an equilibrium concentration of M(SCN)2 of 2.00 x 10-5 M. What are the equilibrium concentrations of the two starting ions and what is the value of the equilibrium constant? [M2+] = ___ x 10__ M [SCN-]= ___ x 10__ M Kc = ___ x 10 __
A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) What is Kf, the formation constant, for this complex?
A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) Use your correct answers from #7 to answer this question. What is Kf, the formation constant, for this complex?
for the reaction 4PH ₂3 (9) 6 H₂₂ (9) + P4 (9) the equilibrium concentrations were found to be [PH3] = 0.250M, [#₂] = 0.370 M, and [P4]=0.750 M. what is the equilibrium constant for this reaction?
An experiment was carried out to determine the value of the equilibrium constant, Kc for the reaction.• Total moles of Ag+ present= 3.6 x 10 -3 moles• Total moles of NH3 present = 6.9 x 10-3 moles• Measured concentration of Ag(NH3)2 + at equilibrium = 3.4 x 10-2 M• Total solution volume = 100 mLCalculate the equilibrium concentration of Ag+ and NH3(uncomplexed)
The Kf for the formation of the B(CN)42- is 7.4 × 1039. Calculate the concentration of B2+ at equilibrium in a solution when concentrated KCN is added to a 0.14 M solution of B(NO3)2 to give an equilibrium concentration of [CN] = 0.013 M. Neglect the small volume change that occurs when KCN is added.
Given the equilibrium concentrations of [FeSCN2+] = 6.55 x 10-4 M, [Fe3+] = 8.39 x 10-4 M, and [SCN-] = 2.28 x 10-3 M, calculate the value of Keq.

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS