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anonymous
 one year ago
Acid Base stoichiometry question
anonymous
 one year ago
Acid Base stoichiometry question

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.023. 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.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i have no idea where to start...

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1first write an equation for the process

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0so i put dw:1433913881712:dw

aaronq
 one year ago
Best ResponseYou've already chosen the best response.1That'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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