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If the dissociation constant of 5×10-4 m aqueous solution of diethylamine is 2.5×10-5 its ph value is?
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If the dissociation constant of 5×10-4 m aqueous solution of diethylam...
The pH value of a solution is a measure of its acidity or alkalinity. It is determined by the concentration of hydrogen ions (H+) present in the solution. In order to calculate the pH value of a solution, we need to know the concentration of H+ ions, which can be determined based on the dissociation constant of the compound in the solution.
Dissociation constant is a measure of the extent to which a compound dissociates into its ions in a solution. In this case, we have a 5×10-4 M aqueous solution of diethylamine (C4H11N), and its dissociation constant is given as 2.5×10-5.
First, let's understand the dissociation reaction of diethylamine:
C4H11N ⇌ C4H10N+ + H^-
The dissociation constant (Ka) can be expressed as:
Ka = [C4H10N+][H^-] / [C4H11N]
where [C4H10N+] and [H^-] are the concentrations of the ions, and [C4H11N] is the concentration of the diethylamine.
Since the concentration of diethylamine is given as 5×10-4 M, we can substitute the values into the equation:
2.5×10-5 = [C4H10N+][H^-] / (5×10-4)
Now, let's assume that x is the concentration of both [C4H10N+] and [H^-], as they are formed in a 1:1 ratio. Therefore, the equation becomes:
2.5×10-5 = x^2 / (5×10-4)
Rearranging the equation, we get:
x^2 = 2.5×10-5 × 5×10-4
x^2 = 1.25×10-8
Taking the square root of both sides, we find:
x = √(1.25×10-8)
x ≈ 1.12×10-4
Since the concentration of H+ ions is equal to the concentration of [H^-], we can conclude that the concentration of H+ ions in the solution is approximately 1.12×10-4 M.
Now, to calculate the pH value, we use the formula:
pH = -log[H+]
Substituting the concentration of H+ ions, we get:
pH = -log(1.12×10-4)
pH ≈ 3.95
Therefore, the pH value of the 5×10-4 M aqueous solution of diethylamine with a dissociation constant of 2.5×10-5 is approximately 3.95.
In summary:
- The dissociation constant of the diethylamine solution is given as 2.5×10-5.
- We assume the concentration of [C4H10N+] and [H^-] to be x.
- By substituting the values into the dissociation constant equation and solving for x, we find the concentration of H+ ions to be 1.12×10-4 M.
- Using the pH formula, we calculate the pH value to be approximately 3.95.
Dissociation constant is a measure of the extent to which a compound dissociates into its ions in a solution. In this case, we have a 5×10-4 M aqueous solution of diethylamine (C4H11N), and its dissociation constant is given as 2.5×10-5.
First, let's understand the dissociation reaction of diethylamine:
C4H11N ⇌ C4H10N+ + H^-
The dissociation constant (Ka) can be expressed as:
Ka = [C4H10N+][H^-] / [C4H11N]
where [C4H10N+] and [H^-] are the concentrations of the ions, and [C4H11N] is the concentration of the diethylamine.
Since the concentration of diethylamine is given as 5×10-4 M, we can substitute the values into the equation:
2.5×10-5 = [C4H10N+][H^-] / (5×10-4)
Now, let's assume that x is the concentration of both [C4H10N+] and [H^-], as they are formed in a 1:1 ratio. Therefore, the equation becomes:
2.5×10-5 = x^2 / (5×10-4)
Rearranging the equation, we get:
x^2 = 2.5×10-5 × 5×10-4
x^2 = 1.25×10-8
Taking the square root of both sides, we find:
x = √(1.25×10-8)
x ≈ 1.12×10-4
Since the concentration of H+ ions is equal to the concentration of [H^-], we can conclude that the concentration of H+ ions in the solution is approximately 1.12×10-4 M.
Now, to calculate the pH value, we use the formula:
pH = -log[H+]
Substituting the concentration of H+ ions, we get:
pH = -log(1.12×10-4)
pH ≈ 3.95
Therefore, the pH value of the 5×10-4 M aqueous solution of diethylamine with a dissociation constant of 2.5×10-5 is approximately 3.95.
In summary:
- The dissociation constant of the diethylamine solution is given as 2.5×10-5.
- We assume the concentration of [C4H10N+] and [H^-] to be x.
- By substituting the values into the dissociation constant equation and solving for x, we find the concentration of H+ ions to be 1.12×10-4 M.
- Using the pH formula, we calculate the pH value to be approximately 3.95.
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If the dissociation constant of 5×10-4 m aqueous solution of diethylam...
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If the dissociation constant of 5×10-4 m aqueous solution of diethylamine is 2.5×10-5 its ph value is?
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