Write a balanced chemical equation based on the following description:
aqueous iridium(III) bromide reacts with aqueous silver acetate to form
solid silver bromide and aqueous iridium(III) acetate

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)  

Explanation:

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate + silver bromide

You have probably learned NAG SAG and "Cats Cradle Old People," Sally Said.

I've listed the rules below.

The PMS group are the exception to the rule that halides are usually soluble.

We can use the solubility rules to decide which product is the precipitate.

Iridium(III) acetate — soluble (Acetate)

Silver bromide — insoluble (PMS,  Silver halide)

So silver bromide is a precipitate.

The word equation becomes

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate(aq) + silver bromide(s)

In symbols, the equation is

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error

the ratio of the conjugate base to the acid required to attain the desired ph.