Question
How many moles of sulfuric acid (H2SO4) are needed to neutralize 0.15 moles of sodium hydroxide (NaOH) in an acid-base reaction?
How many moles of sulfuric acid (H2SO4) are needed to neutralize 0.15 moles of sodium hydroxide (NaOH) in an acid-base reaction?
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Koala Tutor
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The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH) is:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
From the balanced equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydroxide.
Therefore, the number of moles of sulfuric acid needed to neutralize 0.15 moles of sodium hydroxide is:
0.15 moles NaOH * (1 mole H2SO4 / 2 moles NaOH) = 0.075 moles H2SO4
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