how much ml of oxalic acid is needed to standardize 0.1M NaoH
Both are moniprotic. However, you need to know what volume of lye is being used., and the concentration of the oxalic acid.
Oxalic acid is H2C2O4 and that is diprotic.
To determine the amount of oxalic acid needed to standardize 0.1M NaOH, we need to use the concept of stoichiometry.
The balanced chemical equation between oxalic acid (H2C2O4) and sodium hydroxide (NaOH) is:
H2C2O4 + 2NaOH -> Na2C2O4 + 2H2O
From the equation, we can see that each mole of oxalic acid reacts with 2 moles of NaOH.
To solve this, we need to know the volume of NaOH solution being standardized (the volume of 0.1M NaOH solution you plan to titrate).
Let's assume the volume of NaOH solution is V NaOH (in mL).
To calculate the amount of oxalic acid needed, we'll use the following formula:
moles of oxalic acid = moles of NaOH
moles = Molarity * Volume (in L)
Here, the molarity of NaOH solution is 0.1M, and the volume of NaOH solution used is V NaOH (converted to L).
So, the amount of oxalic acid needed can be calculated as:
moles of oxalic acid = (0.1 mol/L) * (V NaOH / 1000 L/mL)
The expression (V NaOH / 1000) converts the volume from milliliters to liters.
Now, since the stoichiometry is 1:1 between oxalic acid and NaOH, the moles of oxalic acid needed will be the same as the moles of NaOH used.
Therefore, the amount of oxalic acid needed in milliliters (ml) can be determined as:
Amount of oxalic acid (in mL) = moles of oxalic acid * molar mass of oxalic acid / Molarity of oxalic acid
The molar mass of oxalic acid (H2C2O4) is 126.07 g/mol.
Note: The molarity of oxalic acid is not provided in the question. If you have the molarity of oxalic acid, you can substitute it in the above equation to calculate the volume needed.