what volume of 0.85M oxalic acid (C2H2O4)

solution would be required to the following equation ( atomic mass C=12 ,O=16 and Na=23)
A. 10.8mL C.10.8L

B.108 L D.108 mL

To calculate the volume of the 0.85M oxalic acid solution required, we need to use the equation:

Molarity = moles of solute / volume of solution

First, we need to determine the number of moles of oxalic acid (C2H2O4) required using the equation:

moles = Molarity × volume (in liters)

The molar mass of oxalic acid (C2H2O4) can be calculated as:

(2 × molar mass of Carbon) + (2 × molar mass of Hydrogen) + (4 × molar mass of Oxygen)

= (2 × 12.01 g/mol) + (2 × 1.01 g/mol) + (4 × 16.00 g/mol)

= 24.02 g/mol + 2.02 g/mol + 64.00 g/mol

= 90.04 g/mol

Now, let's calculate the moles of oxalic acid required:

moles = 0.85M × volume (in liters)

Since the options are given in milliliters and liters, we need to convert the volume given in each option to liters.

A. 10.8 mL = 10.8 / 1000 L = 0.0108 L
B. 108 L
C. 10.8 L
D. 108 mL = 108 / 1000 L = 0.108 L

Now, we can substitute the values into the equation to find the moles:

moles = 0.85M × volume (in liters)

For option A:
moles = 0.85 × 0.0108
moles = 0.00918

For option B:
moles = 0.85 × 108
moles = 91.8

For option C:
moles = 0.85 × 10.8
moles = 9.18

For option D:
moles = 0.85 × 0.108
moles = 0.0924

Therefore, the correct answer is option D. 108 mL, which is equivalent to 0.108 liters, results in 0.0924 moles of oxalic acid.