Acid-Base Equilibria and Titrations

How do strong and weak acids differ in ionization, and how does that affect conductivity?

A strong acid dissociates almost completely in water, producing many H+ ions. A weak acid dissociates only partially, producing fewer H+ ions. Therefore, at the same molar concentration, a strong acid has a higher H+ concentration and shows greater electrical conductivity than a weak acid

Two acidic solutions have the same concentration, but the first has higher conductivity. What conclusion can you draw?

The first solution is a stronger acid (or stronger electrolyte) than the second, because it ionizes more and produces more H+ ions, leading to higher electrical conductivity.

In an acidic aqueous solution, what particles carry electric current?

In acidic solutions, H+ ions (along with any other ions present) act as the charge carriers. A higher concentration of H+ ions leads to better electrical conductivity.

What does electrical conductivity in an aqueous solution depend on, and why?

Conductivity depends on the concentration of dissolved ions. More ions in solution means more charge carriers, which allows more electric current to flow, so the electrical conductivity is higher.

A good Lewis acid has an electron-deficient atom containing:

• An incomplete octet (fewer than 8 electrons around the central atom)

• A partial positive charge (δ+) created by neighboring, electronegative atoms pulling electron density away

A good Lewis base has an electron-rich atom containing:

• A negative formal charge

• A lone pair on the central atom

Common Lewis acids to know for the DAT are:

• Metal cations (ex. K⁺, Mg²⁺, Ca²⁺, Fe³⁺)

• Neutral compounds of boron, aluminum

• Other group 13 elements (ex. BF₃, AlCl₃)

• Protons (H⁺