Ans 1: It is given that the pKa value for Tris is 8.1 so using the relation pKa+pKb=14 we can calculate that pKb= 7.9. At the beginning of the reaction the pH is 7.8 and we know that
pH= pKa- log[HA]/[A-]; putting the respective values we get 7.8= 8.1- log[HA]/[A-].
0.3= log [HA]/ [A-]; 10(-0.3) = [A-]/ [HA]; [A-]/ [HA] = 1:2.
So the ratio of free base to the protonated form is 1:2. Option D is correct
Ans 2: As per the reaction 0.033 moles/liter of H+ is consumed this means that there is a decrease in the protonated form and increase in the basic form. SInce we know the ratio of basic to protonated form is 1:2 and we have the initial concentration 0.2 M, so the concentration of protonated form is 0.134 and the basic form is 0.066. When 0.033 moles/liter of H+ consumes the same amount is increased in basic form and decrease in the protonated form as the protonated form is breaking into free base and H+. The new concentration becomes 0.101 for protonated form and 0.099 for free base. Now taking the ratio we get 0.099/0.101 which is approximately equal to 1. So after the reaction completion the ratio of free base to the protonated form is 1:1. Option C is correct.
An enzyme-catalyzed reaction is carried out in a solution containing 0.2 M tris((hydroxymethyl)aminomethane (known as Tris,...
12,13,14 12 Assume that an enzyme-catalysed biochemical reaction is carried out in a solution ontaining 0.2 M tris(Chydroxymethylaminomethane (known as Tris, pk, 8.1). Shown below is the chemical structure in its protonated form. OH HN GOH OH The pH of the reaction mixture at the start is 8.4. As a result of the reaction, 0.033 molester of H was generated. What was the ratio of Tris (free base) to Tris (protonated form) at the beginning of the reaction? 9.45 1...
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What is the pH of a solution containing 0.3 M Tris(hydroxymethyl)amino-methane (free base) and 0.2 M Tris hydrochloride? pka = 8.1
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