Calculate the milliliters of 0.8916 M KOH needed to neutralize 25.00 mL of 0.6552 M H2SO4 (to produce K2SO4 and H2O)?

Expert Answers

An illustration of the letter 'A' in a speech bubbles

First let's write out a balanced chemical equation:

H2SO4 + 2KOH --> K2SO4 + 2H2O

So for each mole of sulfuric acid (H2SO4), you will need two moles of KOH to neutralize it.  So now let's calculate the moles of sulfuric acid that we have:

0.025 L * (0.6552 moles/L) = 0.01638 moles acid

So we need two moles of KOH per mole of acid, so that means we need 0.01638 * 2 = 0.03276 moles KOH.  So now we can calculate the volume of KOH solution that we need:

0.03276 moles * (1 L/0.8916 moles) = 0.03674 L KOH = 36.74 mL of KOH solution.

The answer is 36.74 mL of KOH solution.

Approved by eNotes Editorial Team
Soaring plane image

We’ll help your grades soar

Start your 48-hour free trial and unlock all the summaries, Q&A, and analyses you need to get better grades now.

  • 30,000+ book summaries
  • 20% study tools discount
  • Ad-free content
  • PDF downloads
  • 300,000+ answers
  • 5-star customer support
Start your 48-Hour Free Trial