Answer:
To determine the volume of potassium hydroxide (KOH) solution needed to neutralize citric acid, we need to consider the balanced chemical equation between the two compounds.
The balanced equation for the neutralization reaction between citric acid (C6H8O7) and potassium hydroxide (KOH) is:
3 KOH + C6H8O7 -> 3 H2O + K3C6H5O7
From the equation, we can see that 3 moles of potassium hydroxide react with 1 mole of citric acid. Therefore, the molar ratio is 3:1.
Given:
Mass of citric acid = 3.35 g
Molar mass of citric acid = 192.1 g/mol
Molarity of potassium hydroxide solution = 0.100 M
First, we need to calculate the number of moles of citric acid:
Number of moles of citric acid = (Mass of citric acid) / (Molar mass of citric acid)
Number of moles of citric acid = 3.35 g / 192.1 g/mol
Next, we can use the molar ratio to determine the number of moles of potassium hydroxide needed:
Number of moles of KOH needed = (Number of moles of citric acid) × (3 moles of KOH / 1 mole of citric acid)
Now, we can calculate the volume of potassium hydroxide solution needed using the molarity:
Volume of KOH solution needed = (Number of moles of KOH needed) / (Molarity of KOH solution)
Let's perform the calculations:
Number of moles of citric acid = 3.35 g / 192.1 g/mol ≈ 0.01742 mol
Number of moles of KOH needed = 0.01742 mol × (3 mol KOH / 1 mol citric acid) ≈ 0.05226 mol
Volume of KOH solution needed = 0.05226 mol / 0.100 M ≈ 0.5226 L
Finally, we convert the volume from liters to milliliters:
Volume of KOH solution needed = 0.5226 L × 1000 mL/L ≈ 522.6 mL
Therefore, approximately 522.6 mL of the 0.100 M potassium hydroxide solution will be needed to neutralize 3.35 g of citric acid.