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13 Dec 2019

Codeine is a very popular perscription pain killer because it is a lot less addictive than morephine. Coedine contains a basic nitrogen atom that can be protonated to give the conjugate acid of codeine. Calculate the pH of 3.30x10^-4M solution of codeine if the pKa of the conjugate acid is 8.21.

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Related questions

The equation for the protonation of acetamide shows a hypothetical product that is not actually formed. When acetamide is protonated by a strong enough acid, it does not protonate on nitrogen, but at a different basic site.

Calculate the pKa of this conjugate acid.

Express your answer as an integer.

Buffer solutions can be produced by mixing a weak acid with its conjugate base or by mixing a weak base with its conjugate acid. The Henderson-Hasselbalch equation, pH=pKa+log[base][acid] allows you to calculate the pH of a buffer. Note that molarity, moles, and millimoles are all proportional, so you can substitute the number moles, or millimoles, for the concentration terms in this formula.

Part A

You need to produce a buffer solution that has a pH of 5.43. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74.

Express your answer numerically in millimoles.
_________ mmol acetate

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