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11 June, 17:51

How many milliliters of 0.20 molar koh solution are needed to exactly neutralize 20. milliliters of 0.50 molar hcl?

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  1. 11 June, 19:55
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    The balanced equation for the neutralisation reaction between KOH and HCl is as follows

    KOH + HCl - - > KCl + H₂O

    stoichiometry of KOH to HCl is 1:1

    the number of HCl moles reacted = HCl concentration x volume

    number of HCl moles = 0.50 mol/L x 0.020 L = 0.01 mol

    according to molar ratio of 1:1

    number of KOH moles required to neutralise 0.01 mol of HCl = 0.01 mol of KOH

    molarity of KOH = 0.20 M

    there are 0.20 mol in 1 L Then 0.01 mol are - 0.01 mol / 0.20 mol/L = 50 mL

    50 mL of 0.20 M KOH required
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