# Question #0e3ac

Aug 8, 2017

Here's what I get.

Citric acid ($\text{H"_3"Cit}$) is a weak tricarboxylic acid with the chemical formula ${\text{C"_6"H"_8"O}}_{7}$.

Although the degree of dissociation depends on concentration, a reasonable rule of thumb is that citric acid is about 8 % ionized.

Thus, if you start with 1 mol of $\text{H"_3"Cit}$, the equilibrium solution will contain about $\text{0.92 mol H"_3"Cit, 0.08 mol H"^"+}$, and $\text{0.08 mol H"_2"Cit"^"-}$.

Thus 1 mol of $\text{H"_3"Cit}$ produces 1.08 mol of "particles".

${\text{K"_2"HPO}}_{4}$ is an ionic substance.

It dissociates completely in solution:

$\text{K"_2"HPO"_4"(aq)" → "2K"^"+""(aq)" + "HPO"_4^"-""(aq)}$

The hydrogen phosphate ion is such a weak acid that we can ignore its ionization.

Thus 1 mol of $\text{K"_2"HPO"_4}$ produces 3 mol of "particles" in solution.