How can I tell whether something is a weak, strong, or non-electrolyte?

I know non-electrolytes do not ionize, strong almost completely ionize and weak only partially.

But how would I be able to tell? Like, something like KOH is a strong electrolyte because it can ionize into OH^- and K^+ ions, but why is something like water a weak electrolyte, even though it can ionize into OH^- an H^+ ions.

We talk mostly about acids in water solution; therefore, the strength of an acid or base depends upon how it reacts with water. For example,

HCl(g) + H2O ==> H3O^+ + OH^-
In this case, the extra pair of electrons on the H2O molecule (remember it has two unshared pairs) attract the H^+ from HCl to form H3O^+ and that leaves the Cl^- to stand alone. Said another way, H2O is a stronger base than Cl^-; that is, the H2O molecule to H^+ bond formed is stronger than the
H-Cl bond. So whether an acid or a base is strong or weak depends upon the H-X bond strength versus the H-O-H bond strength. From a practical point, just keep a chart of ionization constants for acids and bases (Ka and Kb) handy. If the compound has a Ka or Kb it is week. If not, it is strong (or it could be insoluble in water).

what are the non-electrolytes of ORS

To determine whether a substance is a weak, strong, or non-electrolyte, you need to consider its ability to ionize in water.

Non-electrolytes are substances that do not ionize when dissolved in water. Examples of non-electrolytes include most organic compounds, such as sugar (C12H22O11) or ethanol (C2H5OH). When these substances dissolve in water, they remain as intact molecules and do not produce any ions.

Strong electrolytes are substances that completely ionize when dissolved in water, producing a large number of ions. Examples of strong electrolytes include ionic compounds that readily dissociate into ions, such as sodium chloride (NaCl) or potassium hydroxide (KOH). When these substances dissolve in water, they break apart into their constituent ions, resulting in a high concentration of ions in the solution.

Weak electrolytes are substances that only partially ionize when dissolved in water, producing a small number of ions. Examples of weak electrolytes include weak acids (e.g., acetic acid, CH3COOH) or weak bases (e.g., ammonia, NH3). When these substances dissolve in water, only a fraction of the molecules ionize, leading to a lower concentration of ions in the solution compared to strong electrolytes.

Now, let's use water as an example to understand why it is considered a weak electrolyte despite its ability to ionize into H+ and OH- ions. Water undergoes a process called autoionization, where a small fraction of water molecules dissociate into H+ and OH- ions. However, the concentration of these ions is very low compared to a strong electrolyte. Most water molecules remain intact, making the overall ionization of water relatively weak. Therefore, water is classified as a weak electrolyte.

To summarize, the classification of a substance as a weak, strong, or non-electrolyte depends on the extent to which it ionizes in water. Non-electrolytes do not produce ions, strong electrolytes completely ionize, and weak electrolytes only partially ionize.