how many milliliters of .242 m of NaOH are required to exactly titrate 18.0 grams of H2C2O4
Since you are using text style typing, I wonder if that is 0.242 m or 0.242 M. It makes a difference. I think you probably meant for it to be M.
If so then use mL x M = mL x M.
If actually m, then convert m to M and use the above formula.
To find out how many milliliters of NaOH solution are required to titrate 18.0 grams of H2C2O4, we need to use the stoichiometry of the balanced chemical equation between NaOH and H2C2O4.
The balanced chemical equation for the reaction between NaOH and H2C2O4 is:
2NaOH + H2C2O4 → Na2C2O4 + 2H2O
From the balanced equation, we can see that the mole ratio between NaOH and H2C2O4 is 2:1. This means that 2 moles of NaOH react with 1 mole of H2C2O4.
Now let's calculate the number of moles of H2C2O4 in 18.0 grams using its molar mass.
Molar mass of H2C2O4:
H = 1.01 g/mol x 2 = 2.02 g/mol
C = 12.01 g/mol x 2 = 24.02 g/mol
O = 16.00 g/mol x 4 = 64.00 g/mol
Total molar mass of H2C2O4 = 2.02 g/mol + 24.02 g/mol + 64.00 g/mol = 90.04 g/mol
Number of moles of H2C2O4 = Mass of H2C2O4 / Molar mass
= 18.0 g / 90.04 g/mol
≈ 0.1998 moles
Since the mole ratio between NaOH and H2C2O4 is 2:1, the number of moles of NaOH required is twice that of H2C2O4.
Number of moles of NaOH = 2 x 0.1998 moles = 0.3996 moles
To find the volume of the NaOH solution required, we need to use the molarity (M) of NaOH, which is given as 0.242 M.
Molarity (M) = Moles of solute / Volume of solution in liters
Therefore, Volume of NaOH solution = Moles of NaOH / Molarity
= 0.3996 moles / 0.242 M
≈ 1.65 liters
Finally, we convert liters to milliliters:
Volume of NaOH solution = 1.65 liters x 1000 ml/liter
= 1650 ml
Therefore, approximately 1650 milliliters of 0.242 M NaOH solution are required to exactly titrate 18.0 grams of H2C2O4.