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anonymous

  • one year ago

Acid Base stoichiometry question

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  1. anonymous
    • one year ago
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    23. In a chemical analysis, 25.0 ml of sulfuric acid was titrated to the second end point with 0.358 mol/L KOH. In the titration, an average volume of 18.2 ml was required. Calculate the molar concentration of the sulfuric acid.

  2. anonymous
    • one year ago
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    i have no idea where to start...

  3. aaronq
    • one year ago
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    first write an equation for the process

  4. anonymous
    • one year ago
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    so i put |dw:1433913881712:dw|

  5. aaronq
    • one year ago
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    That's not quite right. It says sulfuric acid and KOH, and if we include the side reactions with water, then, \(\sf H_2SO_4+2H_2O\rightarrow 2 H_3O^++SO_4^{2-}\) \(\sf 2 H_3O^++SO_4^{2-}+2KOH\rightarrow K_2SO_4+4H_2O\) If you cancel all the intermediates, the equation is: \(H_2SO_4+2KOH\rightarrow K_2SO_4+2H_2O\) Now we need to find the moles of base. Use: \(\sf Molarity=\dfrac{moles_{solute}}{L_{solution}}\)

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