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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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W0lf93

Answer:  
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)
GuilhermeSouzaS

Answer:

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 H2SO4 neutralized KOH

0.1375 mol / 2 = 0.06875 mol  H2SO4 amount  

volume required of H2SO4 ---> 0.06875 mol / 0.755 mol/L = 0.0910596 L = 91.0 mL

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