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Suppose a standard strong-base solution was prepared byweighing out 1.934g of NaOH in 500mL of water. This solution wastitrated against KHP dissolved in 200 mL of water required 48.23mLof the base solution.

How many moles of NaOH were required to neutralize the KHPthat was weighed out and what is the Molariy of the "standard base"using the information obtained from the KHP titration. 1.934g NaOH(1mol NaOH/39.998NaOH) = 0.048 moles NaOH so wouldthe same amount of KHP be weighed out as well?

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Category:- Chemistry
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