# 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).

81% (399 ratings)
###### 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)?