i have no idea how to do this!
Calculate the volume of the specified titrant required to neutralize 35 ml of .4 M NaOH. Titrant: 0.75 M H2SO4 [2NaOH + H2SO4 „» 2H2O + Na2SO4]
No worries! I'm here to help you break it down step by step.
To find the volume of the titrant required to neutralize the given amount of NaOH, we'll use the concept of stoichiometry and the provided balanced equation.
Step 1: Write down the balanced equation:
2NaOH + H2SO4 → 2H2O + Na2SO4
This equation tells us that for every 2 moles of NaOH, we need 1 mole of H2SO4 to neutralize it.
Step 2: Calculate the amount of moles of NaOH:
moles = concentration × volume
moles = 0.4 M × 35 ml = 0.014 moles
Step 3: Determine the mole ratio between NaOH and H2SO4:
From the balanced equation, we know that for every 2 moles of NaOH, we need 1 mole of H2SO4.
Step 4: Calculate the volume of H2SO4:
volume = moles ÷ concentration
volume = 0.014 moles ÷ 0.75 M = 0.0187 L = 18.7 ml
So, to neutralize 35 ml of 0.4 M NaOH with 0.75 M H2SO4, you would need approximately 18.7 ml of H2SO4.
Remember, the calculations rely on the given concentrations and volumes of the substances involved. Make sure you always check your units and use the correct balanced equation for the reaction.