Problem: If 25.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.842 g of precipitate, what is the molarity of silver ion in the original solution?

🤓 Based on our data, we think this question is relevant for Professor Costanza's class at USF.

FREE Expert Solution

Silver Nitrate (AgNO3) and potassium chloride (KCl) will break up into their ions in the solution and will react as shown:

Balanced Reaction:

AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)

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Problem Details

If 25.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.842 g of precipitate, what is the molarity of silver ion in the original solution?

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Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

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Based on our data, we think this problem is relevant for Professor Costanza's class at USF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.