Electrolytes and non-electrolytes

Introduction to Electrolytes

Think about how electricity moves through your house to turn on the bulb. Metals like copper wire carry current. But did you know some liquids can also carry electricity? These liquids act like a bridge for current to pass through them.

What is an Electrolyte

Imagine salt dissolved in water. If you dip two wires connected to a battery inside, the bulb will light up. This liquid is an electrolyte. It can conduct electricity because it has free-moving ions inside it.

Simply put, an electrolyte is a liquid or melted substance that carries electricity and changes chemically while doing so.

Examples of Electrolytes

Common examples include dilute acids like H_2SO4, alkalis like NaOH, and salts dissolved in water like NaCl (table salt). Even molten (melted) lead (II) bromide, PbBr₂, is an electrolyte.

Non-electrolytes Explained

Not every liquid can carry electricity. If you try to pass current through pure water, kerosene, or sugar syrup, the bulb will stay off. These substances do not have ions to carry the charge.

Basically, non-electrolytes are 'stubborn' liquids that do not let electricity pass through them at all.

Strong and Weak Electrolytes

Some electrolytes are like a bright NEPA light, while others are like a dim candle. Strong electrolytes like HCl or NaOH ionize completely in water. Weak electrolytes like ethanoic acid (vinegar) or ammonia only ionize slightly.

Comparing Electrolytes and Metals

Metals carry electricity using electrons, but electrolytes use ions. In a metal like copper, nothing changes chemically. In an electrolyte, the substance actually breaks down at the electrodes.

Differences between conductors and electrolytes:

Metals conduct in solid state, but electrolytes must be liquid or molten.

Metals use electrons, electrolytes use mobile ions.

Metals do not decompose, but electrolytes break down into new substances.