Hemoglobin (Hb) and oxygen are in equilibrium with the...

Hemoglobin (Hb) and oxygen are in equilibrium with the hemoglobin-oxygen complex, HbO2. Which of the equations below shows the correct setup for calculating the equilibrium constant, $K_{eq}$? $K_{eq} = \frac{[HbO_2]}{[Hb]}$ $K_{eq} = [HbO_2]$ $K_{eq} = \frac{[O_2][Hb]}{[HbO_2]}$ $K_{eq} = \frac{[HbO_2]}{[O_2][Hb]}$

The Keq for imidazole binding to hemoglobin can be determined from the following linear equation. It is used mainly because we will never be directly measuring A100. For the plot of the reciprocal of the change in absorbance versus the reciprocal of the imidazole concentration, identify the equivalent of the slope and the y-intercept in the above equation. Copy the equation in your notebook, and clearly mark a circle around the term equivalent to slope and a square around the y-intercept. If the best-fit line determined for a set of data gives a slope of 0.112 M and an intercept of 21.4, what is the value of ΔA100 and Keq? For the reaction, Hb·Fe+(aq)+Im(aq)⇌Hb·Fe-Im+(aq), what does the calculated value of Keq from question 3b imply about this reaction? Given the Keq your calculated in part c above, if the [Im] = 0.075 M, what is the predicted ratio of bound to unbound ferrihemoglobin?

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