A student determined the chloride content of a commercial salt by using the Mohr method. A 0.5324 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0408 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 23.56 mL was recorded. Calculate the percent chloride in the sample.

moles AgNO3 = M x L = ??

moles Cl^- is the same since the equation is a 1:1 ratio. Cl^- + Ag^= => AgCl.
grams Cl = moles Cl^- x atomic mass Cl.
%Cl^- = (mass Cl^-/mass sample)*100 = ??
Note: mass of the sample is 1/10 x 0.5324g since you took a 25 mL aliquot of the 250 mL sample.

To calculate the percent chloride in the sample, we need to determine the amount of chloride ions that reacted with the silver nitrate solution during the titration. We can then divide this amount by the mass of the sample and multiply by 100 to get the percentage.

Here's how we can calculate it step by step:

1. Determine the moles of silver nitrate used in the titration:
- Volume of silver nitrate used = 23.56 mL
- Concentration of silver nitrate = 0.0408 M (given)
- Moles of silver nitrate = volume (in L) × concentration
=> Moles of silver nitrate = 23.56 mL × (1 L / 1000 mL) × 0.0408 mol/L.

2. Convert moles of silver nitrate to moles of chloride ions:
- Using the balanced chemical equation for the reaction between silver nitrate (AgNO3) and chloride ions (Cl-):
AgNO3(aq) + Cl-(aq) -> AgCl(s) + NO3-(aq)
- The stoichiometric ratio between AgNO3 and Cl- is 1:1.
- So, the moles of chloride ions = Moles of silver nitrate.

3. Calculate the mass of chloride ions:
- Mass of chloride ions = Moles of chloride ions × molar mass of chloride ions.
- The molar mass of chloride (Cl-) is 35.45 g/mol.

4. Calculate the percentage of chloride in the sample:
- Percentage of chloride = (Mass of chloride / Mass of sample) × 100.
- The mass of the sample is given as 0.5324 g.

Plug in the values and calculate the percentage of chloride in the sample.