I have two questions that I am completely clueless on.
Problem: What is the mass of sodium silicate in a 25.0 mL sample of the solution used in a chemical process?
Prediction: If the process is operating as expected, the mass of sodium silicate in a 25.0 mL sample should always be between 6.40 g and g.
Design: An excess quantity of iron (III) nitrate is added to the sample of sodium silicate. The resulting precipitate is separated by filtration. After the precipitate has dries, the mass is determined.
mass of filter paper: .98 g
mass of dried filter paper plus precipitate: 9.45 g
The color of the filtrate was yellow-orange.
For that question, I wrote out the balanced chemical equation and wrote that Iron (III) Nitrate has a mass of 8.46g and that it was a product. Sodium silicate is a reactant and 25.0 mL was used. After that, I have no clue how to proceed.
The second question:
Problem: What is the amount concentration of silver nitrate in the solution to be recycled?
Evidence: A white precipitate was formed in the reaction with acqueous sodium sulfate.
voluume of silver nitrate solution: 100 mL
mass of filter paper: 1.27 g
mass of dried filter paper plus precipitate: 6.74g
For this question, I have no idea what the products or reactants are...
Thanks for your help.