How many milliliters of 0.0560 M EDTA are required to react with 50.0 mL of 0.0170 M Cu^2+? With 50 mL of 0.0170 M Sc^3+?
My work so far:
(50mL)(0.0170mmol/mL)= 0.85 mmol Cu^2+
I'm not sure how to do the rest. Please help.
The easy thing to remember about EDTA titrations is that metals (essentially asll of them) react on a 1:1 basis. Therefore, you 0.85 mmols Cu^2+ will require 0.85 mmols EDTA. M = mmol/mL or
mL = mmol/M = ?
Well, well, well, looks like we've got a chemistry question here! Let's see if I can add a little humor to the mix while helping you out.
To determine the amount of EDTA needed to react with each metal ion, we can use the mole ratio between the metal ion and EDTA from the balanced chemical equation. Unfortunately, I don't have a mole-to-fun ratio. Oh well, let's go!
The balanced chemical equation for the reaction between Cu^2+ ions and EDTA is:
Cu^2+ + EDTA --> [Cu(EDTA)]^2-
We can see from this equation that the mole ratio between Cu^2+ and EDTA is 1:1. So, if we have 0.85 mmol of Cu^2+, we'll need the same amount of EDTA.
Now, let's move on to Sc^3+. The balanced chemical equation for the reaction between Sc^3+ ions and EDTA is:
Sc^3+ + EDTA --> [Sc(EDTA)]^-
Again, we can see that the mole ratio between Sc^3+ and EDTA is 1:1. So, if we have 0.85 mmol of Sc^3+, we'll need the same amount of EDTA.
That wasn't too bad, was it? Just remember to consider the mole ratio between the metal ion and EDTA in the balanced equation, and you'll be on the right track!
Keep up the good work, and don't let chemistry stress you out too much. Remember, laughter is the best chemistry!
Hope this helps, and don't hesitate to ask if you have any more questions!
To determine the number of milliliters of 0.0560 M EDTA required to react with the given Cu^2+ and Sc^3+, we can set up and solve two separate stoichiometry problems.
First, let's calculate the number of millimoles of Cu^2+:
Given:
Volume of Cu^2+ solution = 50.0 mL
Concentration of Cu^2+ solution = 0.0170 M
To determine the number of millimoles, we can use the formula:
moles = concentration * volume
moles of Cu^2+ = 0.0170 M * 50.0 mL
moles of Cu^2+ = 0.0170 moles/mL * 50.0 mL
moles of Cu^2+ = 0.850 mmol
Now, let's calculate the volume of 0.0560 M EDTA required:
Given:
Concentration of EDTA solution = 0.0560 M
To calculate the required volume, we can use the formula:
volume = moles / concentration
volume of EDTA = 0.850 mmol / 0.0560 mmol/mL
volume of EDTA = 15.2 mL (rounded to two decimal places)
Therefore, 15.2 milliliters of 0.0560 M EDTA solution are required to react with 50.0 mL of 0.0170 M Cu^2+.
Now, let's calculate the number of millimoles of Sc^3+:
The calculations are quite similar:
moles of Sc^3+ = 0.0170 M * 50.0 mL
moles of Sc^3+ = 0.0170 moles/mL * 50.0 mL
moles of Sc^3+ = 0.850 mmol
Lastly, let's calculate the volume of 0.0560 M EDTA required for Sc^3+:
volume of EDTA = 0.850 mmol / 0.0560 mmol/mL
volume of EDTA = 15.2 mL (rounded to two decimal places)
Therefore, 15.2 milliliters of 0.0560 M EDTA solution are required to react with 50.0 mL of 0.0170 M Sc^3+.
To determine how many milliliters of 0.0560 M EDTA are required to react with the given solutions, we need to use the stoichiometry of the reaction.
The balanced chemical equation for the reaction between EDTA (Ethylenediaminetetraacetic acid) and Cu^2+ is as follows:
Cu^2+ + EDTA → CuEDTA^2-
From the equation, we can see that one mole of Cu^2+ reacts with one mole of EDTA to form one mole of CuEDTA^2-. Therefore, the mole ratio between Cu^2+ and EDTA is 1:1.
First, let's calculate the number of moles of Cu^2+ in 50.0 mL of the 0.0170 M Cu^2+ solution:
0.0170 mmol/mL * 50.0 mL = 0.85 mmol
Since the mole ratio between Cu^2+ and EDTA is 1:1, we know that 0.85 mmol of Cu^2+ will react with an equal number of moles of EDTA.
To find the number of milliliters of 0.0560 M EDTA needed, we'll use the concentration and the number of moles of EDTA:
[EDTA] = 0.0560 M
moles of EDTA = 0.85 mmol
We can use the formula:
moles = concentration * volume
to solve for the volume (in mL):
0.85 mmol = 0.0560 M * volume
Rearranging the equation, we get:
volume = moles / concentration
volume = 0.85 mmol / 0.0560 M
volume ≈ 15.179 mL
Therefore, approximately 15.179 mL of the 0.0560 M EDTA solution is required to react with 50.0 mL of the 0.0170 M Cu^2+ solution.
To find the volume of 0.0560 M EDTA required to react with 50 mL of 0.0170 M Sc^3+, we follow the same procedure as above.
The balanced chemical equation for the reaction between EDTA and Sc^3+ is:
Sc^3+ + EDTA → ScEDTA^-
Again, from the balanced equation, we can see that one mole of Sc^3+ reacts with one mole of EDTA to form one mole of ScEDTA^-.
Calculate the number of moles of Sc^3+ in 50.0 mL of the 0.0170 M Sc^3+ solution:
0.0170 mmol/mL * 50.0 mL = 0.85 mmol
Since the mole ratio between Sc^3+ and EDTA is 1:1, we know that 0.85 mmol of Sc^3+ will react with an equal number of moles of EDTA.
Using the same formula as before:
volume = moles / concentration
volume = 0.85 mmol / 0.0560 M
volume ≈ 15.179 mL
Therefore, approximately 15.179 mL of the 0.0560 M EDTA solution is required to react with 50.0 mL of the 0.0170 M Sc^3+ solution.