A student determines the mass percent of chloride in an unknown solid mixture containing a soluble chloride salt and an inert, non-chloride water-soluble compound. The student dissolves a \(1.000\text{ g}\) sample of the mixture in distilled water and adds an excess of \(0.20\text{ M AgNO}_3\text{(aq)}\) to precipitate all chloride ions as \(\text{AgCl(s)}\). The precipitate is collected on filter paper in a crucible and heated repeatedly in an oven to dry it. The recorded data are shown in the table below.

Measurement	Mass (g)
Mass of unknown solid mixture sample	\(1.000\)
Mass of empty crucible and filter paper	\(21.500\)
Mass of crucible, filter paper, and precipitate after 1st heating	\(23.220\)
Mass of crucible, filter paper, and precipitate after 2nd heating	\(22.950\)
Mass of crucible, filter paper, and precipitate after 3rd heating	\(22.933\)
Mass of crucible, filter paper, and precipitate after 4th heating	\(22.933\)

Given that the molar mass of \(\text{AgCl}\) is \(143.3\text{ g/mol}\) and the atomic mass of \(\text{Cl}\) is \(35.45\text{ g/mol}\), which of the following is the mass percent of chloride in the original mixture, along with the correct justification for heating to constant mass?