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30 Ιαν 2023 · Define the fraction of dissociation of a weak electrolyte. Calculate the fraction of dissociation of a weak acid or base. Sketch the fraction of dissociation as a function of concentration. A chemical equilibrium involving dissociation can be represented by the following reaction. AB ⇌ A + B, K = [A][B] [AB]
- Exact pH Calculations
When two or more acids are present in a solution, the...
- 9.5: Degree of Dissociation
Such reactions can be easily described in terms of the...
- Exact pH Calculations
16 Ιαν 2023 · Such reactions can be easily described in terms of the fraction of reactant molecules that actually dissociate to achieve equilibrium in a sample. This fraction is called the degree of dissociation. For the reaction in the previous example. A(g) ⇌ 2B(g) the degree of dissociation can be used to fill out an ICE table.
15 Απρ 2024 · Calculate the pH of a solution of a weak monoprotic weak acid or base, employing the "five-percent rule" to determine if the approximation 2-4 is justified. Predict whether an aqueous solution of a salt will be acidic or alkaline, and explain why by writing an appropriate equation.
20 Δεκ 2018 · (ECA5, p.187) Calculate the pH and fraction of dissociation of (a) 10 −2.00 M and (b) 10 −10.00 M barbituric acid. ( Ka = 9.8 × 10 −5 ) Solution: This is a weak acid equilibrium calculation. We can write a table to help us define the equation we need to solve.
K a and K b can be used to calculate the percentage of a weak acid or weak base that is dissociated in a solution with a known pH and pOH. A symbol that denotes percent dissociation is α (alpha). Dissociation is simply the conversion of a compound into its respective ions in a suitable solvent.
[A -] and [H +] is produced when weak acid dissociates. When water dissociates, [OH -] and [H +] are produced. When more HA is dissociated in solution than water, we can assume that the concentration of [A -] is far greater than that of [OH -], so we can exclude [OH -]. Thus the charge balance equation becomes [H +]= [A -].
If the solution pH is 3.202, what percentage of the acid is dissociated? Solution: 1) Convert pK a to K a: K a = 10 ¯ pK a = 10¯ 4.289 = 5.14 x 10¯ 5. 2) The pH gives [H +] (and the [A¯]): [H +] = 10¯ pH = 10¯ 3.202 = 6.28 x 10¯ 4 M 3) Determine the concentration of the weak acid: K a = ([H +] [A¯]) / [HA] 5.14 x 10¯ 5 = [(6.28 x 10 ...
