Determination of Chloride by the Mohr Method $($cont$\text{'}$d$)$

H$.$ Pre$-$Lab Questions

Provide the balanced net ionic chemical equation for the reaction between the titrant and analyte.

Provide the balanced net ionic chemical equation for the reaction between the titrant $(A{g}^{+})$and indicator $(Cr{O}_4^{2-}).$

Calculate the mass of primary standard sodium chloride $)=(58\mathrm{.}44$ necessary to react with $350mL$ of $0\mathrm{.}05MAgN{O}_3.$ This is the mass of NaCl to be dried.

Calculate the mass of $K_{2}Cr{O}_4$ necessary to prepare $10mL$ of a $5\%(\frac{w}{v})$ indicator solution.

Calculate the mass of primary standard sodium chloride $(FW=58\mathrm{.}44$ necessary to react with $25mL$ of $0\mathrm{.}05MAgN{O}_3.$ This is the target mass of NaCl to be titrated for each standardization.

A student used $31\mathrm{.}04mL$ of titrant to reach the endpoint of a titration of $0\mathrm{.}1049g$ sample of NaCl. Calculate the ratio of the volume $(mL)$ of titrant used to mass $(g)$ of sample.

Using the ratio calculated in question six above, calculate the mass of sample necessary to consume exactly $25\mathrm{.}00mL$ of titrant.

What color is $AgC{l}_{(s)}?$

What color is $A{g}_2$CrO$4($s$)?$

At the beginning of the titration, after the indicator is added what color will the solution be$?$

At the beginning of the titration, after the indicator is added will there be a precipitate?

At the endpoint of the titration, what color will the mixture be$?$

At the endpoint of the titration, will there be a precipitate?