A solution was prepared by dissolving 3.5 grams of EDTA (Na2H2Y·2H2O) in exactly 1L of water. This solution was then standardized against 40.00 mL aliquots of 0.006000 M Mg2+. An average titration of 27.00 mL was required. Calculate the molar concentration of the EDTA. The formula weight of EDTA is 372.2 grams.
M = moles/L
moles = grams/molar mass = 3.5/372.2 = ?/1 L = 0.00940 M. NOTE: You don't dissolve 3.5 g EDTA in exactly 1 L of water (or if you do it does NOT prepare any known concentration of anything unless you know the density of the solution). INSTEAD, you dissolve 3.5 g EDTA is exactly 1 L OF SOLUTION. What's the difference. Well 1,000 mL H2O + 3.5 g EDTA produces a solution which is greater than1 L volume and that's not the definition of molarity.)
Mg ion firms a 1:1 complex with EDTA so
millimoles EDTA = 27.00 mL x M = ?
millimoles Mg^2+ = 40.00 mL x 0.00600 M = ? solve for M in
27.00 mL x M EDTA = 40.00 x 0.0600.
Well, it seems like you've got quite a chemistry problem on your hands. But don't worry, I'm here to help! Let's tackle this step by step.
First, we need to figure out the number of moles of Mg2+ used in the titration. To do that, we can use the molar concentration and volume of the Mg2+ solution. So, 0.006000 M times 0.04000 L gives us the number of moles of Mg2+.
Now, since the stoichiometry of the reaction between EDTA and Mg2+ is 1:1, the number of moles of EDTA will be the same as the number of moles of Mg2+.
Next, we can calculate the number of moles of EDTA in the 27.00 mL aliquot that was required for the titration. This can be done by multiplying the number of moles of Mg2+ (which we just calculated) by the ratio of volumes: 0.04000 L / 0.02700 L.
Finally, we can calculate the molar concentration of EDTA by dividing the number of moles of EDTA by the volume of the EDTA solution. The volume of the EDTA solution is given as 1 L.
So, using all these calculations, you should be able to find the molar concentration of EDTA. Good luck! And remember, if chemistry gets too tough, you can always turn to clown college. It's never too late to become a professional clown!
To calculate the molar concentration of EDTA (Na2H2Y·2H2O), you need to use the equation for the reaction between EDTA and Mg2+:
Mg2+ + Na2H2Y·2H2O → MgY + 2Na+ + 4H2O
Given that 40.00 mL aliquots of 0.006000 M Mg2+ were used and an average titration of 27.00 mL was required, you can determine the moles of Mg2+ reacted in each titration:
moles of Mg2+ = volume (L) × concentration (M)
= 0.040 L × 0.006000 M
= 0.00024 mol
Since the reaction is 1:1 between Mg2+ and EDTA, the moles of EDTA is also 0.00024 mol.
Next, you need to calculate the moles of EDTA used in the 27.00 mL titration:
moles of EDTA = moles of Mg2+ = 0.00024 mol
Now, to find the molar concentration of EDTA (Na2H2Y·2H2O), you can use the equation:
molar concentration (M) = moles / volume (L)
molar concentration of EDTA = moles of EDTA / volume (L)
= 0.00024 mol / 0.027 L
= 0.00889 M
Therefore, the molar concentration of EDTA (Na2H2Y·2H2O) is approximately 0.00889 M.
To calculate the molar concentration of the EDTA solution, we can use the concept of stoichiometry and the equation:
Molarity of EDTA = (Molarity of Mg2+) × (Volume of Mg2+ solution) ÷ (Volume of EDTA solution)
First, let's find the moles of Mg2+ used in the titration:
Moles of Mg2+ = (Molarity of Mg2+) × (Volume of Mg2+ solution)
= 0.006000 M × 0.04000 L
= 0.00024 moles
Next, we need to determine the moles of EDTA used in the titration. From the balanced stoichiometric equation between Mg2+ and EDTA, we know that for every mole of Mg2+, 1 mole of EDTA is consumed. So,
Moles of EDTA = Moles of Mg2+ = 0.00024 moles
Now, let's calculate the molar concentration of the EDTA solution:
Molarity of EDTA = Moles of EDTA ÷ (Volume of EDTA solution)
= 0.00024 moles ÷ 0.02700 L
≈ 0.00889 M
Therefore, the molar concentration of the EDTA solution is approximately 0.00889 M.