10.0 mL of 0.15M of sulfuric acid is titrated with 0.05M of sodium hydroxide. how many mL of sodium hydroxide solution are required to reach the equivalence point?
Answered below
use M1V1=M2V2. don't need to change units
2.0
To determine the volume of sodium hydroxide (NaOH) solution required to reach the equivalence point, we need to use the concept of stoichiometry.
Step 1: Write the balanced chemical equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH):
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
This equation tells us that one mole of sulfuric acid reacts with two moles of sodium hydroxide to produce one mole of sodium sulfate and two moles of water.
Step 2: Calculate the number of moles of sulfuric acid using the formula:
moles = concentration (M) × volume (L)
Given concentration of sulfuric acid: 0.15 M
Volume of sulfuric acid: 10.0 mL (which is 0.010 L)
moles of H2SO4 = 0.15 M × 0.010 L = 0.0015 moles
Step 3: Determine the stoichiometric ratio between sulfuric acid and sodium hydroxide by comparing their coefficients in the balanced equation:
From the balanced equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH.
Step 4: Calculate the volume of sodium hydroxide required:
moles of NaOH = (moles of H2SO4) × (stoichiometric ratio)
moles of NaOH = 0.0015 moles × 2 = 0.003 moles
Finally, convert moles of NaOH back to volume using the formula:
volume (L) = moles / concentration (M)
volume of NaOH = 0.003 moles / 0.05 M = 0.060 L, which is equal to 60.0 mL.
Therefore, 60.0 mL of sodium hydroxide solution is required to reach the equivalence point in titrating 10.0 mL of 0.15M sulfuric acid.