A chemist at a pharmaceutical company is measuring equilibrium constants for rea

Question

A chemist at a pharmaceutical company is measuring equilibrium constants for reactions in which drug candidate molecules bind to a protein involved in cancer The drug molecules bind the protein in a 1:1 ratio to form a drug-protein complex. The protein concentration in aqueous solution at 25 degree C is 1.60 times 10-6M. Drug A is introduced into the protein solution at an initial concentration of 2.00 times 10-6M. Drug B is introduced into a separate, identical protein solution at an initial concentration of 2.00 times 10-6M. At equilibrium, the drug A-protein solution has an A-protein complex concentration of 1.00 times 10-6M. and the drug B solution has a B- protein complex concentration of 1.40 times 10-6M. Calculate the Kc value for the A-protein binding reaction. Express your answer using two significant figures. Calculate the Kc value for the B-protein binding reaction. Express your answer using two significant figures. Assuming that the drug that binds more strongly will be more effective, which drug is the better choice for further research? Drug B is the better choice for further research. O Drug A is the better choice for further research.

Explanation / Answer

Part A) K= [protein-A complex]/[proetin][A] = 10^-6/(1.6 x10^ -6 x 2 x10^ -6) = 3.125 x10^ -7 M-1 Part B) K = 1.4 x10^ -6/( 1.6 x10^ -6 x2 x10^ -6) = 4.375 x10^ -7 M-1, Part C) Drug B is better choice for research

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