Calculate the volume of EDTA stoichiometrically equivalent to 1.0 mg of CaCO3.'
To calculate the volume of EDTA stoichiometrically equivalent to 1.0 mg of CaCO3 (calcium carbonate), we need to use the stoichiometry of the reaction between EDTA (ethylenediaminetetraacetic acid) and CaCO3.
The balanced reaction equation is:
CaCO3 + EDTA → Ca-EDTA + CO2
From the balanced equation, we can see that 1 mole of CaCO3 reacts with 1 mole of EDTA to produce 1 mole of Ca-EDTA. This means that the stoichiometric ratio between CaCO3 and EDTA is 1:1.
To calculate the volume of EDTA, we need to know the concentration of EDTA solution. Let's assume we have a 0.1 M (mol/L) solution of EDTA.
Step 1: Convert the mass of CaCO3 to moles:
1.0 mg CaCO3 = 0.001 g CaCO3
molar mass of CaCO3 = 40.08 g/mol + 12.01 g/mol + (3 * 16.00 g/mol) = 100.09 g/mol
moles of CaCO3 = (0.001 g CaCO3) / (100.09 g/mol)
Step 2: Use the stoichiometric ratio to find the moles of EDTA:
moles of EDTA = moles of CaCO3
Step 3: Calculate the volume of EDTA solution:
volume (L) = moles of EDTA / Molarity (M)
volume of EDTA solution = moles of EDTA / 0.1 M (assuming concentration of EDTA solution is 0.1 M)
Now you can substitute the values into the equation to find the volume of EDTA solution stoichiometrically equivalent to 1.0 mg of CaCO3.