Asked by Chuck
A 15.0 g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved
in water. This aqueous mixture then reacts with aqueous potassium chloride to form
3.97 g of solid. Calculate the percent by mass of silver nitrate in the first mixture.
in water. This aqueous mixture then reacts with aqueous potassium chloride to form
3.97 g of solid. Calculate the percent by mass of silver nitrate in the first mixture.
Answers
Answered by
DrBob222
AgNO3 + KCl ==> AgCl + KNO3.
NaNO3 + KCl ==> no reaction.
So you obtained 3.97 g AgCl. Convert that to g AgNO3 this way.
3.97 x (molar mass AgNO3/molar mass AgCl) = ? g AgNO3.
%AgNO3 = (g AgNO3/mass sample)*100 = ?
NaNO3 + KCl ==> no reaction.
So you obtained 3.97 g AgCl. Convert that to g AgNO3 this way.
3.97 x (molar mass AgNO3/molar mass AgCl) = ? g AgNO3.
%AgNO3 = (g AgNO3/mass sample)*100 = ?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.