How many milliliters of 0.150 M are required to react completely with 175 mL of 0.0855 M K2CrO4? What mass of Ag2CrO4 is formed? AgNO3?

No. of moles of K₂CrO₄ = (0.0855 mol/L) × (175/1000 L) = 0.01496 mol

K₂CrO₄(aq) + 2AgNO₃ → Ag₂CrO₄(s) + 2KNO₃(aq)
Mole ratio K₂CrO₄ : AgNO₃ = 1 : 2
No. of moles of AgNO₃ = (0.01496 mol) × 2 = 0.02992 mol
Volume of AgNO₃ = (0.02992 mol) / (0.150 mol/L) = 0.199 L = 199 mL

Refer to the above solution, mole ratio K₂CrO₄ : Ag₂CrO₄ = 1 : 1
No. of Ag₂CrO₄ formed = (0.01496 mol) × 1 = 0.01496 mol
Molar mass of AgNO₃ = (107.9 + 14.0 + 16.0×3) g/mol = 169.9 g/mol
Mass of Ag₂CrO₄ formed = (0.01496 mol) × (169.9 g/mol) = 2.54 g