Solutes throw off a water molecule's "groove".
Fewer degrees of freedom means drop in entropy.
Drop in entropy makes the dissolving the compound less favorable.
$$\Delta G = \Delta H - T \color{red}{\Delta S}$$
Causes molecules to cluster together to maximize $\Delta S$
What happens when you create an amphipathic molecule (has both hydrophobic and hydrophilic character)?
How hydrophobic is the molecule?
What interactions can it make?
What sorts of biological functions might it fulfill?
To convert protonation to charge, you need to know chemistry of the group. For example:
$\color{blue}{R-NH^{+}_{3}} \rightleftharpoons R-NH_{2} + \color{blue}{H^{+}}$
$R-COOH \rightleftharpoons \color{red}{R-COO^{-}} + \color{blue}{H^{+}}$
A few protons can have a huge effect in biochemistry by linking to other equilibria.
Biochemists usually describe proton tirations using the Henderson-Hasselbalch equation:
$$pH = pK_{a} + log \Big (\frac{[A]} {[HA]} \Big ) $$
The fractional protonation on a group is described by $\theta$:
$$\theta = \frac{1}{1 + 10^{pH - pK_{a}}}$$
The $pK_{a}$ is the $pH$ at which a titratable group is half-protonated.
To convert protonation to charge, you need to know chemistry of the group. For example:
$\color{blue}{R-NH^{+}_{3}} \rightleftharpoons R-NH_{2} + \color{blue}{H^{+}}$
$R-COOH \rightleftharpoons \color{red}{R-COO^{-}} + \color{blue}{H^{+}}$