Question 3: Gravimetric Analysis (12 points)
a) A 50.00 mL AgNO3 solution with unknown concentration reacts with excess Na2CO3. A precipitate of Ag2CO3 is formed.

Write the equation for the reaction (3 points):
b)After filtering and drying, the mass of the precipitate is measured as 2.76 g. Calculate the number of moles of precipitate that are formed by the reaction. (3 points)
c) Calculate the number of moles of solution that react. (3 points)
d) Determine the concentration of the AgNO3 solution in mol/L. (3 points)

Question

Question 3: Gravimetric Analysis (12 points)
a) A 50.00 mL AgNO3 solution with unknown concentration reacts with excess Na2CO3. A precipitate of Ag2CO3 is formed.

Write the equation for the reaction (3 points):
b)After filtering and drying, the mass of the precipitate is measured as 2.76 g. Calculate the number of moles of precipitate that are formed by the reaction. (3 points)
c) Calculate the number of moles of solution that react. (3 points)
d) Determine the concentration of the AgNO3 solution in mol/L. (3 points)

vera_ewing · Answer

@Technodynamic Can you please help me with this one?

vera_ewing · Answer

@Abmon98 Please help me

abmon98 · Answer

2AgNO3+Na2CO3-->Ag2CO3+2NaNO3
use the equation Number of moles=Mass(g)/Molar mass(g/mol) to find out the number of moles of the precipitate(Ag2CO3)
c) after you have figure out the number of moles of the ppt use mole ration according to the balanced chemical equation above to work out the moles of AgNO3
d) use Number of moles=Concentration(mol/dm^3)*Volume(dm^3, Volume is already given, do not forget to change the units of volume when using the equation.

vera_ewing · Answer

@Abmon98 So would that be all? That's everything I have to do?

abmon98 · Answer

yes

vera_ewing · Answer

ok thanks so much! :)