Problem: The mass percent of Cl− in a seawater sample is determined by titrating 25.00 mL of seawater with AgNO3 solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free Ag+ ion is present in solution after all the Cl− has reacted. If 53.63 mL of 0.2970 M AgNO3 is required to reach the end point, what is the mass percent of Cl− in the seawater (d of seawater = 1.024 g/mL)?

FREE Expert Solution

For this problem, we have to calculate the mass percent of Cl- in the given sample of seawater

Step 1. Write the balanced equation:

AgNO3 (aq) + Cl- (aq)  AgCl (aq) + NO3(aq)


Step 2. Calculating the mass of Cl- (35.45 g/mol).

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Problem Details

The mass percent of Cl in a seawater sample is determined by titrating 25.00 mL of seawater with AgNO3 solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free Ag+ ion is present in solution after all the Cl has reacted. If 53.63 mL of 0.2970 M AgNO3 is required to reach the end point, what is the mass percent of Cl in the seawater (d of seawater = 1.024 g/mL)?

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What scientific concept do you need to know in order to solve this problem?

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 Randles' class at UCF.

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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.