Calculate the ratio of ch3nh2 to ch3nh3cl required to create a buffer with ph = 10.12.

From tables, we know that the pKa for Methylamine CH₃NH₂ is 10,61. Now, we can apply the Henderson-Hasselbach’s equation and clear for the ratio of CH₃NH₂ to CH₃NH₃Cl So, the ratio of CH₃NH₂ to CH₃NH₃Cl should be 0,32 Have a nice day!

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!

idk really know Explanation:

The chemical reaction for the ionization of CH₃NH₂ is the following: CH₃NH₂ + H₂O ⇄ CH₃NH₃⁺ + OH⁻ pKb=3,30 Now we apply the Henderson-Hasselbach equation and clear for the ratio of CH₃NH₂ to CH₃NH₃Cl: So, the ratio of CH₃NH₂ to CH₃NH₃Cl is 0,38 Have a nice day!

ka = kw/kb = 1E-14/4.4E-4 = 2.27E-11 pka = 10.64 pH = pKa + log[CH3NH2]/[CH3NH3Cl] 10.24 = 10.64 + log[CH3NH2]/[CH3NH3Cl] [CH3NH2]/[CH3NH3Cl] = 0.40 Hope this helps

Answer 6

and when we have the Ka value so, we can get Pka from this formula: Pka = -㏒Ka ∴Pka = -㏒ (2.27 x10^-11) = 10.6 now, to get the base/acid ratio by using Henderson-Hasselblach equation: PH = Pka + ㏒[base/acid] so by substitution: 10.22 = 10.6 + ㏒[base/acid] ∴[base/acid] = 0.417 ∴[CH3NH2/CH3NH3Cl] = 0.417

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