In a Volhard precipitation titration, a piece of sterling silver alloy weighing 0.5039g was dissolved in 10.0ml of concentrated (15M) nitric acid. The solution was dilluted to 60.0ml with water, and 5.00ml of 0.100M Fe(NO3)3 was added as an indicator. The contents of the flask were titrated with 43.56ml of 0.1005M KSCN to reach the red endpoint.
Write the net ionic equation for the titration reaction (the product of the titration reaction was AgSCN precipitate), and use the data to calculate to percentage of silver in the alloy.

Question

In a Volhard precipitation titration, a piece of sterling silver alloy weighing 0.5039g was dissolved in 10.0ml  of concentrated (15M) nitric acid. The solution was dilluted to 60.0ml with water, and 5.00ml of 0.100M Fe(NO3)3 was added as an indicator. The contents of the flask were titrated with 43.56ml of 0.1005M KSCN to reach the red endpoint. 
Write the net ionic equation for the titration reaction (the product of the titration reaction was AgSCN precipitate), and use the data to calculate to percentage of silver in the alloy.

aaronq · Answer

work backwards: 43.56ml of 0.1005M KSCN

moles of KSCN = 0.04356 L*0.1005 M =

then use the stoichiometric coefficients (from the reaction you wrote (and balanced)) to build a ratio to find the moles of silver.

aaronq · Answer

convert the moles of silver to grams.

find the percent of silver front the total mass of the alloy.