Question
Density and Specific Gravity of Solutions: Write the complete solutions:
A 6.42% (w/w) Fe(NO3)3 (241.86g/mol) solution has a density of 1.059g/ml. Calculate the molar analytical concentration of Fe(NO3)3 in the solution.
A 6.42% (w/w) Fe(NO3)3 (241.86g/mol) solution has a density of 1.059g/ml. Calculate the molar analytical concentration of Fe(NO3)3 in the solution.
Answers
Answered by
GPT 3.5
To calculate the molar analytical concentration of Fe(NO3)3 in the solution, we first need to calculate the mass of Fe(NO3)3 present in 1 L of the solution.
Since the solution is 6.42% (w/w) Fe(NO3)3, we can assume there are 6.42g of Fe(NO3)3 in 100g of solution. Therefore, in 1 L of solution (which has a density of 1.059g/ml), there would be:
(6.42g Fe(NO3)3 / 100g solution) * 1.059g/ml * 1000ml/L = 67.99738g Fe(NO3)3/L solution
Now, we can calculate the molarity of Fe(NO3)3 in the solution:
Molarity = mass / (molar mass * volume)
Molarity = 67.99738g / (241.86g/mol * 1L) = 0.2807mol/L
Therefore, the molar analytical concentration of Fe(NO3)3 in the solution is 0.2807 mol/L.
Since the solution is 6.42% (w/w) Fe(NO3)3, we can assume there are 6.42g of Fe(NO3)3 in 100g of solution. Therefore, in 1 L of solution (which has a density of 1.059g/ml), there would be:
(6.42g Fe(NO3)3 / 100g solution) * 1.059g/ml * 1000ml/L = 67.99738g Fe(NO3)3/L solution
Now, we can calculate the molarity of Fe(NO3)3 in the solution:
Molarity = mass / (molar mass * volume)
Molarity = 67.99738g / (241.86g/mol * 1L) = 0.2807mol/L
Therefore, the molar analytical concentration of Fe(NO3)3 in the solution is 0.2807 mol/L.