Chapter 4: Molarity, Molarity of Ions, Solubility, and Dilution

Vocabulary and key concepts covering molarity calculations, dilutions, net ionic equations, electrolyte behavior, and selective precipitation from Chapter 4.

Molarity ($M$)

The measure of solute concentration defined as moles of solute divided by liters of solution ($M = \frac{\text{mols}}{L}$).

Dilution Formula

The mathematical relationship $V_1 M_1 = V_2 M_2$ used to determine initial or final concentrations and volumes when a solution is diluted.

Solute Volume Displacement

The phenomenon where dissolving a solid solute displaces liquid volume, requiring water to be added until the final mixture reaches the target volume rather than adding a set volume of liquid first.

Weak Acid Net Ionic Representation

The convention stating that weak acids (such as $\text{HNO}_2$) do not dissociate completely in aqueous solution and must remain in molecular form in net ionic equations.

Non-Electrolyte

A compound, such as methanol ($\text{CH}_3\text{OH}$), that dissolves in water without dissociating into ions and does not conduct electricity.

Qualitative Separation of $\text{Pb}^{2+}$

A laboratory method using hydrochloric acid ($\text{HCl}$) to selectively precipitate $\text{PbCl}_2$ at room temperature, isolating $\text{Pb}^{2+}$ from ions like $\text{Fe}^{2+}$ and $\text{Cu}^{2+}$.

Nitrous Acid Neutralization Net Ionic Equation

The net ionic equation describing the titration of nitrous acid with sodium hydroxide: $\text{HNO}_2 + \text{OH}^- \rightarrow \text{NO}_2^- + \text{H}_2\text{O}$.

Silver Carbonate and Hydrochloric Acid Net Ionic Reaction

The reaction represented by the net ionic equation $\text{Ag}_2\text{CO}_3 + 2\text{H}^+ + 2\text{Cl}^- \rightarrow 2\text{AgCl} + \text{H}_2\text{O} + \text{CO}_2$.