A 15.0 ml sample of unknown HCL04 solution requires titration with 25.3 ml of 1.200 M NaOH to reach equivalence point. what is the unknown concentration?
It is 1:1 equivalence so use
M1V1=M2V2
To find the unknown concentration of the HClO4 solution, you can use the concept of stoichiometry and the equation for the acid-base reaction that occurs during titration.
The equation for the reaction between HClO4 and NaOH is:
HClO4 + NaOH -> NaClO4 + H2O
From the balanced equation, you can see that the molar ratio between HClO4 and NaOH is 1:1. This means that one mole of HClO4 reacts with one mole of NaOH.
First, calculate the number of moles of NaOH used in the titration:
moles NaOH = Molarity * Volume
moles NaOH = 1.200 M * 0.0253 L
moles NaOH = 0.03036 mol
Since the molar ratio between HClO4 and NaOH is 1:1, the number of moles of HClO4 is also 0.03036 mol.
Now, determine the concentration of the HClO4 solution in terms of moles per liter (Molarity):
Molarity = moles HClO4 / Volume HClO4
The volume of the HClO4 solution is given as 15.0 mL, which is equivalent to 0.0150 L:
Molarity = 0.03036 mol / 0.0150 L
Molarity = 2.024 M
Therefore, the unknown concentration of the HClO4 solution is 2.024 M.