show all work Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 2.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following. HA (aq) + H2O(l) ⇌ A (aq) + H3O (aq) The neutralization reaction between HA and NaOH can be expresses as the following. HA (aq) + NaOH (aq) NaA (aq) + H2O (l) Answer the following questions.
A) What will be the initial pH of the 0.10 M HA solution?
B) What will be the pH of the HA solution after the addition of 5.0 mL of 0.10 M NaOH to the solution?
C) What will be the pH of the HA solution after the addition of 10.0 mL of 0.10 M NaOH to the solution?
D) What will be the pH of the HA solution after the addition of 20.0 mL of 0.10 M NaOH to the solution?
E) What will be the pH of the HA solution after the addition of 25.0 mL of 0.10 M NaOH to the solution?
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show all work Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka=...
A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA has a pH of 1.890 at 25°C. HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq) What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =
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