What are some ways to predict that a double replacement reaction will occur? [duplicate]

This question already has an answer here:

For instance, say:

$\ce{2KOH + Pb(NO3)2 -> 2KNO3 + Pb(OH)2}$

How would I even go about beginning to predict this?

marked as duplicate by ringo, bon, pentavalentcarbon, paracetamol, ButtonwoodJun 13 '17 at 12:58

Look at the double replacement reaction chart. The rules are followed in order. Let's look at $\ce{KNO3}$ first. The first rule states that alkali metal salts are soluble. Potassium is an alkali metal, therefore potassium nitrate is soluble. The second product is $\ce{Pb(OH)2}$. Looking through the rules, none of them apply until the 5th rule which states that hydroxides are insoluble. Therefore lead hydroxide is insoluble.
First reduce the equation into it's respective ions. $$\ce{2KOH(aq) + Pb(NO3)2(aq) -> 2KNO3(aq) + Pb(OH)2(s)}$$ ...becomes... $$\ce{2K+(aq) + 2OH-(aq) + Pb^2+(aq) + 2NO3-(aq) -> 2K+(aq) + 2NO3-(aq) + Pb(OH)2(s)}$$ However, keep in mind that $\ce{Pb(OH)2}$ does not break down into ions because it is insoluble, as we discovered earlier. Therefore it stays in it's full formula. At this point you do the "cancelling out" by removing duplicate ions on each side of the equation. The cancelled ions are also known as spectator ions because they do not actively participate in the synthesis of the product. $$\ce{2OH-(aq) + Pb^2+(aq) -> Pb(OH)2(s)}$$ The potassium and nitrate ions are removed because they appear on each side of the equation in the same quantity. These cancel out leaving the net ionic equation show above.