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).
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)?
Frequently Asked Questions
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.
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.