Answer:
215 mL of silver nitrate are needed.
Explanation:
Let's think the reaction:
Na₂CrO₄(aq) + 2AgNO₃(aq) → Ag₂CrO₄ (s) ↓ + 2NaNO₃(aq)
First of all, we determine the moles of chromate we have available.
Molarity = mol / volume(L)
We convert volume to L → 75mL . 1L / 1000mL = 0.075 L
Molarity . volume(L) = moles → 2.50 M . 0.075L = 0.1875 moles
Ratio is 1:2. For 1 mol of chromate I need the double of moles of nitrate.
So, for 0.1875 moles of chromate I would need (0.1875 . 2) = 0.375 moles of nitrate. Let's determine volume of solution
Molarity = mol/ volume(L) → volume (L) = mol / Molarity
volume (L) = 0.375mol / 1.74M → 0.215L
We convert the value to mL → 0.215L . 1000mL/ 1L = 215 mL
