Problem: The mass percentage of chloride ion in a 26.00 mL sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took 42.52 mL of 0.2996 M silver nitrate solution to reach the equivalence point in the titration.What is the mass percentage of chloride ion in the seawater if its density is 1.025 g/mL? Express your answer using four significant figures.

FREE Expert Solution

Balanced equation is:

Cl-+ AgNO3 AgCl + NO3-

  • Mole ratio:
    • 1 mole Cl- reacts with 1 mole AgNO3
  • At equivalence point:
    • moles Cl- = moles AgNO3


Molarity (M) =moles of soluteLiters of solution


moles Cl-=(0.2996 molAgNO3 L)(42.52  mL×10-3L1 mL)×1 molCl-1 molAgNO3

= 0.01274 mol Cl-


93% (229 ratings)
View Complete Written Solution
Problem Details

The mass percentage of chloride ion in a 26.00 mL sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took 42.52 mL of 0.2996 M silver nitrate solution to reach the equivalence point in the titration.

What is the mass percentage of chloride ion in the seawater if its density is 1.025 g/mL? Express your answer using four significant figures.

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.