Once the salt is formed an equilibrium is established by the reaction of NH 4

Once the salt is formed an equilibrium is established

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2)Once the salt is formed, an equilibrium is established by the reaction of NH4+with H2O and the pH of the solution can be calculated (as was done before). NH4+(aq) + H2O NH3(aq) + H3O+Ka= Exercise: a)What is the pH of 0.10 M acetic acid (Ka= 1.8 x 105), supposing that one has 20 mL of solution? b)What is the pH of the above solution when 5.0 mL of 0.10 M NaOH are added? c)What is the pH of the solution at the stoichiometric point? d)What is the pH of the solution when half of the initial amount of the acid is titrated (special case)? Kw][NH]O][H[NH433 (aq) =
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Solution: O + 0 M + x x 5 x 5 + ] 2.88 0 M mol
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= M = M O + + x x 2 5 K a = 4.27 Question: How many milliliters of base should be added? )
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2 O = OH 0 M + x x 10 ]
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