If you mix 40.0 mL of a 0.389 M solution of K₂CrO₄ with 40.0 mL of a 0.389 M solution of AgNO₃, what mass of solid forms? A) 5.16 g B) 2.58 g C) 3.02 g D) 15.6 g E) 7.78 g

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Quizplus · Accepted Answer

First, identify the reaction: $ \text{KCrO}_4 + \text{AgNO}_3 \rightarrow \text{Ag}_2\text{CrO}_4 $ (solid) + KNO3. The limiting reactant is neither, as they are in stoichiometric amounts. Moles of $ \text{AgNO}_3 $ = 0.389 mol/L * 0.040 L = 0.01556 mol. The reaction ratio is 2:1 for $ \text{AgNO}_3 $ to $ \text{Ag}_2\text{CrO}_4 $, so moles of $ \text{Ag}_2\text{CrO}_4 $ = 0.01556 mol / 2 = 0.00778 mol. The molar mass of $ \text{Ag}_2\text{CrO}_4 $ is approximately 331.73 g/mol, so mass = 0.00778 mol * 331.73 g/mol = 2.58 g.

If You Mix 40