(a) The sample contained 0.002306 moles of chloride ions;
(b) The sample contained 0.0817 g of chloride ions.
The idea behind this reaction is that the silver nitrate,
In order to determine whether or not all the chloride ions have been consumed by the reaction, you add chromate ions,
So, the net ionic equation for the reaction between the chloride ions and silver nitrate looks like this
Notice that you have a
In your case, the end point of the reaction required 43.75 mL of a 0.05270-M silver nitrate solution. Use this information to determine how many moles of
According to the aforementioned mole ratio, you have
To determine how many grams of chloride ions you had present in the sample, use chloride's molar mass
SIDE NOTE Looking at the mass of the sample you started with, I assume that you'll have to calculate the mass percentage of chloride ions in the original sample.
To do that, simply divide the mass of the chloride ions by the total mass of the sample and multiply by 100.