Ammonium sulfate, (NH4)2SO4, is a salt used as a fertiliser. It is made by neutralising ammonia solution with dilute sulfuric acid: 2NH3 + H2SO4 → (NH4)2SO4. The same reaction is used in the laboratory and in industry.
In the laboratory: a fixed volume of ammonia solution is measured into a flask using a pipette. An indicator is added and dilute sulfuric acid is run in from a burette until the colour change shows it has just been neutralised. The volume of acid is noted. The reaction is then repeated with the same volumes but with no indicator, so the crystals are not contaminated. The solution is heated to evaporate some of the water, left to cool so that crystals form, then filtered and dried. This is a small scale, batch process: one portion is made at a time.
In industry: the process is a continuous process on a much larger scale, running all day. Several stages are needed to make the raw materials first. The ammonia comes from the Haber process, using nitrogen from the air and hydrogen from natural gas. The sulfuric acid comes from the contact process (you do not need the details). The ammonia and acid are then reacted in large reactors, and the ammonium sulfate is crystallised and dried.
Comparing: both use the same neutralisation reaction and give the same product. The laboratory method starts with ready-made solutions and uses indicators and a burette to get the amounts exactly right. The industrial method makes its own raw materials and has to control costs, energy use and the supply of raw materials.