Answer:
0.4167 = CH₃NH₂ / CH₃NH₃Cl
Explanation:
The CH₃NH₂ / CH₃NH₃Cl buffer has a pka of 10.62. Using Henderson-Hasselbalch formula:
pH = pka + log₁₀ [A⁻] / [HA]
Where A⁻ is weak base, CH₃NH₂, and HA is conjugate acid, CH₃NH₃Cl. It is possible to obtain the ratio of CH₃NH₂ / CH₃NH₃Cl to create a buffer with pH = 10.24, thus:
pH = pka + log₁₀ [A⁻] / [HA]
10.24 = 10.62 + log₁₀ [A⁻] / [HA]
-0.38 = log₁₀ [A⁻] / [HA]
0.4167 = [A⁻] / [HA]
0.4167 = CH₃NH₂ / CH₃NH₃Cl
I hope it helps!
The ratio of CH₃NH₂ to CH₃NH₃Cl required to create a buffer with ph of 10.24 is 1.25 × 10⁻⁷.
pH of buffer solution will be calculated by using the Henderson Hasselbalch equation as:
pH = pKb + log [conjugate acid] / [weak base]
In the question given that, CH₃NH₂ is a weak base and CH₃NH₃Cl is its conjugate acid.
Value of Kb for CH₃NH₂ = 3.34
Given value of pH = 10.24
On putting all these values on the above equation, we get
10.24 = 3.34 + log[CH₃NH₃Cl]/[CH₃NH₂]
log[CH₃NH₃Cl] / [CH₃NH₂] = 6.9
[CH₃NH₃Cl] / [CH₃NH₂] = [tex]10^{6.9}[/tex]
[CH₃NH₂] / [CH₃NH₃Cl] = 1 / [tex]10^{6.9}[/tex]
[CH₃NH₂] / [CH₃NH₃Cl] = 1.25 × 10⁻⁷
Hence, required value of ratio is 1.25 × 10⁻⁷.
To know more about Henderson Hasselbalch equation, visit the below link:
https://brainly.com/question/13651361
