A chemist prepares a solution of zinc oxalate (ZnC_2O_4) by measuring out 0.01 g of zinc oxalate into a 450. mL volumetric flask and filling the flask to the mark with water
Calculate the concentration in mol/L of the chemist's zinc oxalate solution. Round your answer to 1 significant digit.
The molar mass of zinc oxalate (ZnC2O4) is calculated as follows:
Zinc (Zn) has a molar mass of 65.38 g/mol
Carbon (C) has a molar mass of 12.01 g/mol
Oxygen (O) has a molar mass of 16.00 g/mol
Therefore, the molar mass of ZnC2O4 is:
65.38 + 2(12.01) + 4(16.00) = 179.40 g/mol
Now, we need to calculate the number of moles of zinc oxalate in 0.01 g:
Number of moles = mass / molar mass
Number of moles = 0.01 g / 179.40 g/mol
Number of moles = 5.57 x 10^-5 mol
Next, we need to calculate the concentration in mol/L of the solution:
Concentration = number of moles / volume in liters
Volume = 450. mL = 0.450 L
Concentration = 5.57 x 10^-5 mol / 0.450 L
Concentration = 1.2 x 10^-4 mol/L
Rounded to 1 significant digit, the concentration of the chemist's zinc oxalate solution is 1.2 mol/L.