Problem 2
Water is said to be polar but uncharged. How is it possible? \(4\)
Problem 3
Why are weak bonds important in biochemistry? \(4\)
Problem 4
What are the common types of weak bonds important in biochemistry? How does water affect these bonds? \(4\)
Problem 5
. In liquid water, each molecule is hydrogen bonded to approximately 3.4 molecules of water. What effect would freezing water have on the number of hydrogen bonds? Heating water?
Problem 7
What is an electronegative atom, and why are such atoms important in biochemistry? \(/5\)
Problem 8
Define the hydrophobic effect. 5
Problem 9
How does the Second Law of Thermodynamics allow for the formation of biochemical order?
Problem 10
If an aqueous solution has a hydrogen ion concentration of \(10^{-5} \mathrm{M},\) what is the concentration of hydroxyl ion? \(6\)
Problem 11
If an aqueous solution has a hydroxyl ion concentration of \(10^{-2} \mathrm{M},\) what is the concentration of hydrogen ion? 6
Problem 12
Using the Henderson-Hasselbalch equation, show that, for a weak acid, the \(\mathrm{p} K_{\mathrm{a}}\) is the \(\mathrm{pH}\) at which the concentration of the acid equals the concentration of the conjugate base. \(6\)
