How many milliliters of 0.242 M NaOH are required to exactly titrate 18.0 grams of H2C2O4?
H2C2O4 + 2NaOH ==> Na2C2O4 + 2H2O
mols H2C2O4 = grams/molar mass
Using the coefficients in the balanced equation, convert mols H2C2O4 to mols NaOH.
Then mols NaOH = M x L. You know mols and M, solve for L and convert to mL.
Well, let's titrate some humor into this equation, shall we? Imagine the NaOH as a superhero and the H2C2O4 as a mischievous villain. The NaOH, with its trusty sidekick 0.242 M, sets out to neutralize the H2C2O4 and restore balance to the chemistry world.
Now, the atomic masses of NaOH and H2C2O4 are 40 and 90, respectively. So, let's convert that 18.0 grams of H2C2O4 to moles using some conversion wizardry. Poof! We get approximately 0.2 moles of H2C2O4.
Since NaOH and H2C2O4 have a 1:2 molar ratio, our superhero NaOH needs double the number of moles to carry out its neutralization mission. Double poof! We have 0.4 moles of NaOH.
Now, with our trusty concentration of 0.242 M, we can use the equation C = n/V to solve for the volume (V) of NaOH needed. With some mathematical acrobatics, we find that V = n/C. Plugging in our numbers, we get V = 0.4 moles / 0.242 M.
And voila! By dividing 0.4 moles by 0.242 M, we determine that approximately 1.65 liters (or 1650 milliliters) of NaOH are required to titrate 18.0 grams of H2C2O4. Our superhero NaOH wins again, saving the day in a humorous and chemical way!
To calculate the number of milliliters of 0.242 M NaOH required to titrate 18.0 grams of H2C2O4, we need to use the equation and stoichiometry of the reaction.
The balanced equation for the reaction between NaOH and H2C2O4 is as follows:
2 NaOH + H2C2O4 → Na2C2O4 + 2 H2O
From the balanced equation, we can see that the stoichiometric ratio of NaOH to H2C2O4 is 2:1. This means that 2 moles of NaOH react with 1 mole of H2C2O4.
First, we need to calculate the number of moles of H2C2O4 in 18.0 grams using its molar mass.
The molar mass of H2C2O4 can be calculated as follows:
(2 * atomic mass of H) + (2 * atomic mass of C) + (4 * atomic mass of O)
= (2 * 1.01 g/mol) + (2 * 12.01 g/mol) + (4 * 16.00 g/mol)
= 2.02 g/mol + 24.02 g/mol + 64.00 g/mol
= 90.04 g/mol
Next, we can calculate the number of moles of H2C2O4:
moles = mass / molar mass
moles = 18.0 g / 90.04 g/mol
moles ≈ 0.1999 mol
Since the stoichiometric ratio of NaOH to H2C2O4 is 2:1, we can determine the number of moles of NaOH required using the same ratio.
Number of moles of NaOH = 2 * number of moles of H2C2O4
Number of moles of NaOH = 2 * 0.1999 mol
Number of moles of NaOH ≈ 0.3998 mol
Now, we can use the molarity of NaOH to calculate the volume required.
Molarity (M) = moles / volume (in liters)
Given that the molarity (M) is 0.242 M and we want to calculate the volume in milliliters:
Volume of NaOH = moles / molarity
Volume of NaOH = 0.3998 mol / 0.242 mol/L
Volume of NaOH ≈ 1.652 mL
Therefore, approximately 1.652 milliliters of 0.242 M NaOH are required to titrate 18.0 grams of H2C2O4.
To determine the number of milliliters of 0.242 M NaOH required to titrate 18.0 grams of H2C2O4, you need to use the concept of stoichiometry.
Here's how you can calculate it step by step:
1. Determine the molar mass of H2C2O4 (oxalic acid). The molar mass of hydrogen (H) is 1 g/mol, carbon (C) is 12 g/mol, and oxygen (O) is 16 g/mol. Since there are two hydrogen atoms, two carbon atoms, and four oxygen atoms in H2C2O4, the molar mass is:
(2 * 1) + (2 * 12) + (4 * 16) = 90 g/mol
2. Calculate the number of moles of H2C2O4:
Number of moles = mass / molar mass
= 18.0 g / 90 g/mol
= 0.2 mol
3. Use the balanced chemical equation for the reaction between H2C2O4 and NaOH to determine the stoichiometric ratio between them. The balanced equation is:
H2C2O4 + 2NaOH -> 2H2O + Na2C2O4
From the equation, we can see that 1 mole of H2C2O4 reacts with 2 moles of NaOH.
4. Convert the moles of H2C2O4 to moles of NaOH:
Number of moles of NaOH = Moles of H2C2O4 * (2 moles of NaOH / 1 mole of H2C2O4)
= 0.2 mol * 2
= 0.4 mol
5. Finally, calculate the volume of 0.242 M NaOH required by dividing the number of moles of NaOH by its molarity:
Volume = Moles of NaOH / Molarity
= 0.4 mol / 0.242 mol/L
= 1.65 L
Since the molarity is given in terms of liters, you need to convert the volume to milliliters by multiplying by 1000:
Volume (in milliliters) = 1.65 L * 1000 mL/L
= 1650 mL
Therefore, you need approximately 1650 milliliters (or 1.65 liters) of 0.242 M NaOH to titrate 18.0 grams of H2C2O4.