What is the approximate pH of a 0.06 M solution of CH3COOH (given that Ka = 1.78 x 10-5
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Given conditions ⇒
Molarity of the Solutions = 0.06 M.
Ka = 1.78 × 10⁻⁵
For finding the ion of the concentration , We know
[H+]² = Kₐ × a
[H+]² = 1.78 × 10⁻⁵ × 0.06
[H+]² = 1.068 × 10⁻⁶
[H+] = 1.033 × 10⁻³
Where H+ is the ion of the concentration .
Now , Using the Formula,
pH = -log₁₀[H+]
pH = -log₁₀(1.033 × 10⁻³)
pH = 2.985
Hence the required pH of 0.06 M of solution of acetic acid is 2.985
Hope it Helps.
Molarity of the Solutions = 0.06 M.
Ka = 1.78 × 10⁻⁵
For finding the ion of the concentration , We know
[H+]² = Kₐ × a
[H+]² = 1.78 × 10⁻⁵ × 0.06
[H+]² = 1.068 × 10⁻⁶
[H+] = 1.033 × 10⁻³
Where H+ is the ion of the concentration .
Now , Using the Formula,
pH = -log₁₀[H+]
pH = -log₁₀(1.033 × 10⁻³)
pH = 2.985
Hence the required pH of 0.06 M of solution of acetic acid is 2.985
Hope it Helps.
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