Achemistry graduate student is given 250. ml of a 1.00 m trimethylamine cch, n solution. trimethylamine is a weak base with kb=7.4x 10 . what mass of (ch3)3nhbr should the student dissolve in the (ch3)3n solution to turn it into a buffer with ph-11.467 you may assume that the volume of the solution doesn't change when the (ch3) nhbr is dissolved in it. be sure your answer has a unit symbol, and round it to 2 significant digits.

8.8 g

Explanation:

Given:-

[Trimethylamine] = 1.00 M

Volume = 250 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 0.25 L

Given that:

pH = 11.467

Also, pH + pOH = 14

So, pOH = 14 - 11.467 = 2.533

Considering the Henderson- Hasselbalch equation for the calculation of the pOH of the basic buffer solution as:

So,

[Salt] = 0.2526 M

Considering:

So,,

So, Moles of = 0.2526*0.25 moles = 0.06315 moles

Molar mass of = 140.02 g/mol

The formula for the calculation of moles is shown below:

Thus,

explanation:

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