IF 10ml of H2SO4 is need to neutralize 20ml of 1N NaOH, how many milliliters of H2SO4 is needed to make 1 liter of 11M solution?
The equation is H2SO4 + 2NaOH ==>Na2SO4 + 2H2O
moles NaOH = M x L = 1 x 0.020 = 0.02.
moles H2SO4 = 0.02 x (1 mole H2SO4/2 moles NaOH) = 0.01 mole H2SO4
M H2SO4 = mols/L = 0.01 moles/0.01 L (that's 10 mL) = 1 M H2SO4. I don't know how to make it 11 M.
To find the volume of H2SO4 needed to make a 1 liter, 11M solution, we can use the concept of the normality (N) of a solution.
Normality (N) is defined as the number of equivalents of solute per liter of solution. In the case of H2SO4, it has two acidic protons, so it is a diprotic acid. Therefore, the normality is equal to twice the molarity of the H2SO4 solution.
In this question, we know that 10ml of H2SO4 is required to neutralize 20ml of 1N NaOH.
To calculate the normality of the H2SO4 solution used in the neutralization reaction:
Normality (N) of NaOH = 1N
Volume (V) of NaOH used = 20ml
Since the normality (N) of NaOH is 1N, we can determine the number of moles of NaOH:
Number of moles (n) of NaOH = Normality (N) × Volume (V) = 1N × 20ml = 20 millimoles (mmol)
Considering H2SO4 is a diprotic acid, indeed two moles of NaOH will react with one mole of H2SO4. Therefore, the number of moles of H2SO4 required is:
Number of moles (n) of H2SO4 = 20 millimoles (mmol) / 2 = 10 millimoles (mmol)
Now, to determine the volume of H2SO4 needed to make a 1 liter, 11M solution:
Molarity (M) of H2SO4 = 11M
Volume (V) of H2SO4 needed = ???
We can use the formula for molarity to find the volume of H2SO4 needed:
Molarity (M) = Number of moles (n) / Volume (V)
11M = 10 millimoles (mmol) / Volume (V)
Rearranging the equation to solve for volume:
Volume (V) = Number of moles (n) / Molarity (M) = 10 millimoles (mmol) / 11M
Since the given solution volume is 1 liter, we need to convert millimoles (mmol) to moles (mol):
Number of moles (mol) = Number of millimoles (mmol) / 1000 = 10 / 1000 = 0.01 mol
Substituting the values:
Volume (V) = 0.01 mol / 11M
Now, calculating the volume:
Volume (V) = 0.01 mol / 11M = 0.000909 L
Since 1 L is the same as 1000 ml, converting the volume to milliliters:
Volume (V) = 0.000909 L × 1000 ml/L = 0.909 ml
Therefore, approximately 0.909 milliliters of H2SO4 is needed to make a 1 liter, 11M solution.