when titrating 50 mL of .10M H2SO45 with .10 M NaOH, how many mL of NaOH will you have added to reach first equivalence point?
NaOH + H2SO4 ==> NaHSO4 + H2O
You have 0.1M x 50 mL = 5 millimols H2SO4. Therefore, to reach the first equivalence point you must titrate 5 millimols (another 5 millimols will be needed to titrate the second H).
So you will need 50 mL of 0.1M NaOH to titrate that first H and another 50 to titrate the second H.
To determine the volume of NaOH needed to reach the first equivalence point when titrating 50 mL of 0.10 M H2SO4 with 0.10 M NaOH, we need to consider the stoichiometry of the reaction.
The balanced chemical equation for the reaction between H2SO4 and NaOH is:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
From this equation, we can see that one mole of H2SO4 reacts with two moles of NaOH.
First, we can calculate the number of moles of H2SO4 in the given volume. Moles (n) can be calculated using the formula:
n = Molarity (M) x Volume (V) / 1000
n(H2SO4) = 0.10 M x 50 mL / 1000 = 0.005 moles
Since the stoichiometric ratio between H2SO4 and NaOH is 1:2, we would need twice the number of moles of NaOH to react with all the H2SO4 present. Therefore, we require 0.010 moles of NaOH.
Now we can calculate the volume of 0.10 M NaOH needed to reach the first equivalence point. Again, we will use the formula:
V = n / M
V(NaOH) = 0.010 moles / 0.10 M = 0.10 L = 100 mL
Thus, you would need to add 100 mL of 0.10 M NaOH to reach the first equivalence point.
To determine the amount of NaOH needed to reach the first equivalence point when titrating sulfuric acid (H2SO4) with sodium hydroxide (NaOH), we need to consider the stoichiometry of the reaction.
The balanced equation for the neutralization reaction between H2SO4 and NaOH is as follows:
H2SO4 + 2NaOH ⟶ Na2SO4 + 2H2O
From the equation, we can see that each mole of H2SO4 reacts with two moles of NaOH. This means that the stoichiometric ratio is 1:2.
Given that the initial concentration of both H2SO4 and NaOH is 0.10 M, we can calculate the number of moles of H2SO4 present in the 50 mL of solution.
Moles of H2SO4 = concentration (M) × volume (L)
= 0.10 mol/L × 0.050 L
= 0.005 mol
Since the stoichiometric ratio is 1:2, we would need twice the number of moles of NaOH to completely react with the H2SO4.
Moles of NaOH needed = 2 × moles of H2SO4
= 2 × 0.005 mol
= 0.010 mol
Now, we can calculate the volume of 0.10 M NaOH solution needed to provide 0.010 moles of NaOH.
Volume of NaOH = moles / concentration
= 0.010 mol / 0.10 mol/L
= 0.100 L
= 100 mL
Therefore, you will need to add 100 mL of 0.10 M NaOH solution to reach the first equivalence point.