What is the molarity of aqueous silver nitrate if 50.0 mL of AgNO₃ reacts with 25.0 mL of 0.100 M k₂CrO₄? 2 AgNO₃(aq)+ k₂CrO₄(aq)→ Ag2CrO₄(s)+ 2 KNO₃(aq)

Question

Quizplus · Accepted Answer

The stoichiometry of the reaction shows that 2 moles of AgNO₃ react with 1 mole of K₂CrO₄. Given that 25.0 mL of 0.100 M K₂CrO₄ is used, this means there are 0.0025 moles of K₂CrO₄ (since Molarity = moles/volume in liters, and 25.0 mL = 0.025 L, so 0.100 M * 0.025 L = 0.0025 moles). Since the reaction requires twice as many moles of AgNO₃, this means 0.0050 moles of AgNO₃ are needed. Given that the volume of the AgNO₃ solution is 50.0 mL (or 0.050 L), the molarity of the AgNO₃ solution is 0.0050 moles / 0.050 L = 0.100 M.

What Is the Molarity of Aqueous Silver Nitrate If 50