What volume must the final solution reach if you want to make a #"0.01 N"# oxalic acid solution in water using #"126 g"# of oxalic acid solid?

Answer 1
I got #"280. L"#, if the oxalic acid was anhydrous.
However, it typically is purchased as a dihydrate, #"H"_2"C"_2"O"_4cdot2"H"_2"O"#, so if that is what you are looking for, then it would be #ul"200. L"#.
Normality for acids is defined with respect to the #"H"^(+)# the acid gives into solution. #"0.01 N"# oxalic acid therefore would indicate a #"0.01 M"# concentration for #"H"^(+)# given to solution, and so, it would actually be #"0.005 M"#, as it is a diprotic acid.
Oxalic acid has a molar mass of #"90.03 g/mol"#, but the dihydrate equivalent would have a molar mass of #"126.06 g/mol"#, so the mols we have are:
#126 cancel"g OA" xx "1 mol OA"/(126.06 cancel"g") = "0.9995 mols"#
These mols are dissolved in the appropriate volume #V# such that
#"0.9995 mols"/V = "0.005 mols"/"L" " oxalic acid"#
Therefore, the volume the solution must reach by the time the #"126 g"# of oxalic acid is dissolved is...
#V = (0.9995 cancel"mols OA")/(0.005 cancel"mols""/L") = "199.9 L"#

Three sig figs' worth of data would be...

#color(blue)(V = "200. L")#
Sign up to view the whole answer

By signing up, you agree to our Terms of Service and Privacy Policy

Sign up with email
Answer 2

To determine the volume of the final solution needed to make a 0.01 N oxalic acid solution using 126 g of oxalic acid solid, we need to calculate the number of moles of oxalic acid first.

Given: Mass of oxalic acid (H2C2O4) = 126 g Molar mass of oxalic acid = 126.07 g/mol (C2H2O4)

Number of moles of oxalic acid: ( \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} ) ( \text{Number of moles} = \frac{126 , \text{g}}{126.07 , \text{g/mol}} ) ( \text{Number of moles} \approx 0.9997 , \text{moles} )

To prepare a 0.01 N solution, we need 0.01 moles of oxalic acid per liter of solution.

Volume of the final solution: ( \text{Volume} = \frac{\text{Number of moles}}{\text{Normality}} ) ( \text{Volume} = \frac{0.9997 , \text{moles}}{0.01 , \text{N}} ) ( \text{Volume} \approx 99.97 , \text{L} )

Therefore, the final solution must reach approximately 99.97 liters to make a 0.01 N oxalic acid solution using 126 g of oxalic acid solid.

Sign up to view the whole answer

By signing up, you agree to our Terms of Service and Privacy Policy

Sign up with email
Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

Not the question you need?

Drag image here or click to upload

Or press Ctrl + V to paste
Answer Background
HIX Tutor
Solve ANY homework problem with a smart AI
  • 98% accuracy study help
  • Covers math, physics, chemistry, biology, and more
  • Step-by-step, in-depth guides
  • Readily available 24/7