A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization.
What was the concentration of the unknown HClO4 solution? The neutralization reaction is:
HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq)
If anyone can help me to set this up, thank you
moles NaOH = M x L = ?
Look at the equation; it is 1:1, therefore, moles HClO4 = moles NaOH
The M HClO4 = moles HClO4/L HClO4.
To find the concentration of the unknown HClO4 solution, you can use the concept of stoichiometry. Here's how you can set up the problem:
1. Start by writing the balanced equation for the neutralization reaction:
HClO4(aq) + NaOH(aq) → H2O(l) + NaClO4(aq)
2. Use the stoichiometry of the balanced equation to set up a mole-to-mole ratio between HClO4 and NaOH. From the equation, you can see that the ratio of HClO4 to NaOH is 1:1.
3. Calculate the number of moles of NaOH used in the reaction. You can do this by using the given information: 50.3 mL of 0.101 M NaOH solution.
Moles of NaOH = Volume (L) × Concentration (mol/L)
Moles of NaOH = 0.0503 L × 0.101 mol/L
4. Using the mole-to-mole ratio, determine the number of moles of HClO4 required for complete neutralization. Since the ratio is 1:1, the number of moles of HClO4 will be the same as the number of moles of NaOH.
Moles of HClO4 = Moles of NaOH
5. Calculate the concentration of HClO4 in the unknown solution. You know that 15.0 mL of the unknown HClO4 solution is required to neutralize the same number of moles as in 50.3 mL of 0.101 M NaOH.
Concentration (mol/L) = Moles ÷ Volume (L)
Concentration of HClO4 = (Moles of HClO4) / (0.015 L)
By plugging in the known values, you can calculate the concentration of the unknown HClO4 solution.