Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 decade ago

How many milliliters of 0.140 M HCl is need titrate this at equivalence point?

How many milliliters of 0.140 M HCl are needed to titrate each of the following solutions to the equivalence point?

(a) 40.0 mL of 0.0950 M NaOH

(b) 23.5 mL of 0.126 M KOH

(c) 125.0 mL of a solution that contains 1.20 g of NaOH per liter

Update:

beanie is right. except for B, which was simply a copy error. he/she was a decimal pt off.

1 Answer

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  • 1 decade ago
    Favorite Answer

    convert all to moles

    a) .0400L* 0.0950M = .0038 moles

    b) .0235L * .0126M = .0002961

    c) 1.20g/ 40gNaOH/ mole = 0.030 M *.1250L =0.00375 moles

    how many moles/ L is there of the HCl (easy one) 0.140moles/ L

    divide now

    a) .0038 moles NaOH/ 0.140 moles HCl / L =0.0271 L or 27.1mL

    b).0002961moles KOH/ 0.140 moles HCl / L = 0.00212L or 2.1mL

    c) 0.00375 moles NaOH/ 0.140moles HCl/ L = 0.0268L or 26.8mL

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