Chemistry on a lab i did ?

oh ops lol. 2. below are the balanced equations for the reactions in parts 1–3. review the results of your experiments and look closely over the mole ratios of the chemical reactions. do your experiments reflect the stoichiometric, molar amounts indicated by the reactions? discuss this using the evidence from your experiments.
cu(no3)2 (aq) + 2naoh (aq)  cu(oh)2 (s) + 2nano3 (aq) note: cu(oh)2 is a blue precipitate.
feso4 (aq) + 2naoh (aq)  fe(oh)2 (s) + na2so4 (aq) note: fe(oh)2 is a dark green precipitate.
fe(no3)3 (aq) + 3naoh (aq)  fe(oh)3 (s) + 3nano3 (aq) note: fe(oh)3 is a red-orange precipitate

Well #        # Drops of Iron Sulfate             # Drops of Sodium Hydroxide
  A1         5     45
  A2        10    40
  A3        15     35
  A4        20     30
  A5        25     25
  A6        30     20
  B1        35     15
  B2        40     10
  B3        45      5

that's for B, because it says "Iron Sulfate".
which is this equation: FeSO4 (aq) + 2NaOH (aq)  Fe(OH)2 (s) + Na2SO4 (aq)

FeSO4 (aq) + 2NaOH (aq)  Fe(OH)2 (s) + Na2SO4 (aq)
ratio of FeSO4:NaOH is 1:2,
so you need to moles of NaOH for every mole of FeSO4.

A1-A6 had precipitate, though less ppt every time. This corresponds to the decrease in the number of NaOH drops At A2 10/1:40/2 the stoichiometric ratio is equal, so you should've seen the post ppt present. But looking at the picture it doesn't look right. I think you might've labelled them wrong, or there is an error somewhere. This fits micro-plate A better.