Quick questions on Strong vs weak acids and bases (degree of ionisation) explained: HSC Chemistry Module 6

These properties are independent: you can have a dilute strong acid or a concentrated weak acid.

Strong acids are essentially fully ionised in water. The common examples for HSC:

A weak acid only partially ionises, setting up an equilibrium:

Electrical conductivity of a solution depends on the total concentration of ions. At equal acid concentration, a strong acid produces many more ions than a weak acid, so it conducts much better.

For two solutions of equal concentration:

A strong acid reacts faster initially because more $H^+$ is present at any instant. However, a weak acid reacts to the same final extent with a stoichiometric excess of, for example, magnesium, because as $H^+$ is consumed the equilibrium shifts right (Le Chatelier) and more weak acid ionises.

When a weak acid is diluted, the percent ionisation increases. Mathematically, if $K_a$ is fixed and $c$ decreases, then $x/c = \sqrt{K_a/c}$ grows. In the limit of infinite dilution every weak acid becomes 100 percent ionised. This is a Le Chatelier consequence: dilution favours the side with more particles.

"Strong" refers to degree of ionisation; "concentrated" refers to mol/L. Both terms describe the acid, but they describe different things. Concentrated and dilute apply equally to strong and weak.

It is less reactive initially per mole of dissolved acid. Given time and excess reactant, the total chemistry can be the same.

Dilution does not turn a weak acid into a strong one, but it does increase the fraction ionised.

For dilute solutions HSC typically treats both protons as fully ionised. For concentrated solutions the second $K_a$ matters. State your assumption.

Pure water has very low conductivity but is not "weakly acidic" (its $[H^+] = 10^{-7}$ comes from auto-ionisation). Always relate conductivity to total ion concentration, not to acidity alone.