A 13.0 mL sample of an unknown HClO4 solution requires titration with 25.2 mL of 0.180 M to reach the equivalence point.
What is the concentration of the unknown HClO4 solution? The neutralization reaction is as follows:
HClO4 +NaOH ===>> H2O +NaClO4
Since the reaction is 1:1 you may use the simplified formula of mL x M = mL x M
To find the concentration of the unknown HClO4 solution, we can use the concept of stoichiometry and the balanced equation for the neutralization reaction. Here's how you can calculate it:
1. First, let's write and balance the equation for the neutralization reaction:
HClO4 + NaOH -> H2O + NaClO4
2. Determine the stoichiometric ratio between HClO4 and NaOH. It can be obtained from the balanced equation, which is 1:1. This means that 1 mole of HClO4 reacts with 1 mole of NaOH.
3. Convert the volume of the NaOH solution used in the titration to moles:
Volume of NaOH solution = 25.2 mL = 0.0252 L (since 1 mL = 0.001 L)
Moles of NaOH = Volume × Concentration = 0.0252 L × 0.180 M = 0.004536 moles
4. Since the stoichiometric ratio between HClO4 and NaOH is 1:1, the number of moles of HClO4 is also 0.004536 moles.
5. Calculate the concentration of the HClO4 solution by dividing the moles of HClO4 by the volume of the HClO4 solution used in the titration:
Volume of HClO4 solution = 13.0 mL = 0.013 L (since 1 mL = 0.001 L)
Concentration of HClO4 = Moles / Volume = 0.004536 moles / 0.013 L = 0.349 M
Therefore, the concentration of the unknown HClO4 solution is 0.349 M.