How many milliliters of 0.755 m h2so4 solution is needed to react with 55.0 ml of 2.50 m koh solution? given: 2 koh (aq) + h2so4 (aq) → 2 h2o (l) + k2so4 (aq) ?

Question

Mallory Santana

Chemistry

27 September, 02:02

How many milliliters of 0.755 m h2so4 solution is needed to react with 55.0 ml of 2.50 m koh solution? given: 2 koh (aq) + h2so4 (aq) → 2 h2o (l) + k2so4 (aq) ?

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Jonathan Wood · Answer 1

moles KOH - - - > (2.50 mol/L) (0.0550 L) = 0.1375 mol

The KOH to H2SO4 molar ratio of 2 to 1 is the key. Only half as much H2SO4 get neutralized compared to the KOH:

0.1375 mol / 2 = 0.06875 mol < - - - that's the H2SO4 amount

volume required of H2SO4 - - - > 0.06875 mol / 0.755 mol/L = 0.0910596 L = 91.0 mL (to three sig figs)