Answer:
Concentration of sodium carbonate solution = Moles of sodium carbonate / (135 mL / 1000) (convert mL to L)
Step-by-step explanation:
To find the concentration of the sodium carbonate solution, we need to use the concept of stoichiometry and the amount of precipitate recovered.
First, we need to calculate the moles of the precipitate (barium carbonate) using its mass:
Mass of precipitate = 7.13 g
Next, we determine the moles of barium carbonate using its molar mass. The molar mass of barium carbonate (BaCO3) is 197.34 g/mol:
Moles of barium carbonate = Mass of precipitate / Molar mass of barium carbonate
Moles of barium carbonate = 7.13 g / 197.34 g/mol
Now, since the reaction between barium chloride and sodium carbonate is 1:1, the moles of barium carbonate also represent the moles of sodium carbonate present in the solution.
Therefore, the moles of sodium carbonate = Moles of barium carbonate
Now, we need to calculate the volume of the sodium carbonate solution using its concentration. Let's assume the concentration of the sodium carbonate solution is "C" mol/L.
Moles of sodium carbonate = Concentration of sodium carbonate solution * Volume of sodium carbonate solution
Since we have the moles of sodium carbonate and the volume is given as 135 mL, we can rearrange the equation to solve for the concentration:
Concentration of sodium carbonate solution = Moles of sodium carbonate / Volume of sodium carbonate solution
Concentration of sodium carbonate solution = Moles of sodium carbonate / (135 mL / 1000) (convert mL to L)
Substituting the value of moles of sodium carbonate, we can calculate the concentration.
Note: Make sure to perform the necessary unit conversions to ensure consistency in units.