Consider the titration of 42.0 mL of 0.270 M HF with 0.215 M
NaOH. Calculate the...
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Chemistry
Consider the titration of 42.0 mL of 0.270 M HF with 0.215 MNaOH. Calculate the pH at each of the following points.
a) How many milliliters of base are required to reach theequivalence point?
b) Calculate the pH after the addition of 10.5 mL of base
c) Calculate the pH at halfway to the equivalence point.
d) Calculate the pH at the equivalence point.
e) Calculate the pH after the addition of 84.0 mL of base.
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We know that for HF Ka72 x 104 HFaq Haq Faq NaOH Aq HF H2O NaF HF initial 027 moleL x moles 0042 L x moles 0011134 moles HF Now to 42 ml of HF solution 105ml of 0215M NaOH is added NaOH moles 00105 0215 00022575 moles When we add base moles of HF will reduce but at the same time F will be added to solution Moles of HF depleted 0011134 00022575
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