Need help on chemistry, solution problems.

[Tensaiga]

Hello, the question i have here is:

Fifty millilitres of a 0.05M solution of Sodium Carbonate is added to 80mL of a 5% by mass solution containing Siliver Nitrate. The product of the reaction are solid Siliver Carbonate and a solution is evapourated to dryness, leaving a mixture of salts. How many grams of the salts, Sodium Carbonate, Siliver Nitrate, Siliver Carbonate, and Sodium Nitrate are present in the salt mixture?

Note: Indicate any assumptions necessary in order to perform the calculations.

The balanced chemical equation is Na2CO3 + 2AgNO3 = Ag2CO3 + 2NaNO3

Na2CO3 = 106g/mol
AgNO3 = 169.87g/mol
Ag2CO3 = 275.74g/mol
NaNO3 = 85.00g/mol

i found out the moles of Sodium Carbonate to be 0.0025 mol.

Then I'm stuck, thanks everyone.

 

[QuantumKing]

First of all, is it 5% mass by mass? or mass by volume?

 

[Blueshift5]

Hello! It seems like you have already made some progress in your calculations. To continue, we can use the balanced equation and the given information to find the moles of silver nitrate present in the solution. From there, we can use stoichiometry to determine the moles of silver carbonate formed and the moles of sodium nitrate remaining in the solution. We can then use the molar masses of each compound to convert the moles to grams.

Assuming that the reaction goes to completion, we can also assume that all of the silver nitrate is consumed and converted into silver carbonate. Additionally, when the solution is evaporated to dryness, we can assume that all of the water is removed and only the salts remain.

I hope this helps guide you in your calculations. Remember to always double check your work and units to ensure accuracy.