Reacting 35.4 mL of 0.220 M AgNO₃ with 52.0 mL of 0.420 M K₂CrO₄ results in what mass of solid formed? A) 2.21 g B) 4.89 g C) 1.29 g D) 1.74 g E) 7.25g

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The reaction is AgNO3 + K2CrO4 → Ag2CrO4 + 2KNO3. Calculate moles of AgNO3 (0.0354 L * 0.220 M = 0.007788 mol) and K2CrO4 (0.0520 L * 0.420 M = 0.02184 mol). AgNO3 is the limiting reagent. Moles of Ag2CrO4 formed = 0.007788 mol / 2 = 0.003894 mol. Mass = 0.003894 mol * 331.73 g/mol (molar mass of Ag2CrO4) = 1.29 g.