A 25.0 mL sample of perchloric acid solution required 45.3 mL of 0.101 sodium hydroxide solution for complete neutralization. what was the concentration of the perchloric acide solution?
work:
0.0453 L NaOH x ( .101 mol NaOH/ 1L NaOH) x (1 mol HClO4/ 1 mol NaOH) x (25.0 mL HClO4/ 1 mol HClO4) = .114
.114 x 100%= 11.4
I have no clue if I did that right. Thank you
Va*Ma=Vb*Mb
Ma=Vb/Va *Mb=43.3/25 *.101=.17M check that
Your calculations are almost correct. Let's go through the steps together to ensure accuracy.
Step 1: Convert the volume of the sodium hydroxide solution to liters.
Given: 45.3 mL NaOH
Conversion: 45.3 mL NaOH x (1 L / 1000 mL) = 0.0453 L NaOH
Step 2: Calculate the number of moles of sodium hydroxide (NaOH).
Given: 0.0453 L NaOH, 0.101 mol NaOH / 1 L NaOH
Calculation: 0.0453 L NaOH x (0.101 mol NaOH / 1 L NaOH) = 0.00458 mol NaOH
Step 3: Use the balanced chemical equation to find the number of moles of perchloric acid (HClO4) that reacted with sodium hydroxide (NaOH).
The balanced equation for the neutralization reaction is:
HClO4 + NaOH -> NaClO4 + H2O
According to the equation, 1 mole of HClO4 reacts with 1 mole of NaOH.
Given: 0.00458 mol NaOH, 1 mol HClO4 / 1 mol NaOH
Calculation: 0.00458 mol NaOH x (1 mol HClO4 / 1 mol NaOH) = 0.00458 mol HClO4
Step 4: Convert the volume of the perchloric acid solution to liters.
Given: 25.0 mL HClO4
Conversion: 25.0 mL HClO4 x (1 L / 1000 mL) = 0.0250 L HClO4
Step 5: Calculate the concentration of the perchloric acid (HClO4) solution.
Given: 0.00458 mol HClO4, 0.0250 L HClO4
Calculation: Concentration (M) = moles / volume = 0.00458 mol HClO4 / 0.0250 L HClO4 = 0.1832 M HClO4
Step 6: Convert the concentration to a percentage.
Given: 0.1832 M HClO4
Conversion: Percentage = 0.1832 M HClO4 x 100% = 18.3%
Therefore, the concentration of the perchloric acid solution is 18.3%.