A solid sample (mass ) that is claimed to be pure potassium sulfate is analyzed…
CHEMISTRY · Multi-part · AP · Chemistry · Chemical Reactions · Chemical Reactions
Problem
A solid sample (mass =1.500g) that is claimed to be pure potassium sulfate is analyzed gravimetrically. The sample is dissolved in water, and an excess of aqueous barium nitrate is added. After the reaction is complete, the barium sulfate precipitate is filtered, washed, and dried to constant mass. The mass of dry barium sulfate obtained is 1.137g.
Use this information to complete the following tasks.
(a) Write the balanced net ionic equation for the precipitation reaction that occurs.
(b) Calculate the number of moles of barium sulfate collected.
(c) Determine the mass percent of potassium sulfate in the original solid sample.
(d) Discuss one possible experimental source of error that could lead to the calculated mass percent being lower than the true value, and explain its effect qualitatively.