Using the stoichiometry of the reaction between sulfuric acid and sodium hydroxide calculate the number of moles of sodium hydroxide required to neutralize the acid.
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7. In a titration of sulfuric acid against sodium hydroxide, 32.20 mL of 0.250M NaOH is required to neutralize 26.60 mL H2SO4. a. What is the balanced equation for the reaction of sulfuric acid with sodium hydroxide H2SO4(aq) + 2NaOH(aq) -> 2H2O(l) + Na2SO4(aq) b. What is the mole to mole ratio in which NaOH reacts with sulfuric acid? c. What is the molarity of the sulfuric acid based on this titration data? (hint: moles of NaOH -> to moles of H2SO4 -> molarity of H2SO4)
Madhur L.
Determine the whole number mole ratio of moles of NaOH to moles of sulfuric acid
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For the acid-base reaction (called titration) of sulfuric acid (H2SO4) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with 1.03 L of 0.500 M sulfuric acid to reach complete neutralization (endpoint)? Sodium hydroxide is a strong base and sulfuric acid is a strong acid. So they completely dissociate in an aqueous solution: 2NaOH + H2SO4 -> Na2SO4 + 2H2O.
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