Need Chemistry Help ASAP -- Quinine Question:? - quinine more drug_side_effects
Quinine, a drug used to treat malaria, is a weak Bronsted base, which can be represented as Qu. In his 25oC PKB is 5.48. To make it soluble in water, in a solution as its conjugate acid, which can be represented as H-QuCl. What is the pH of a solution 0.15 M + H calculated Qu?
Tuesday, February 23, 2010
Quinine More Drug_side_effects Need Chemistry Help ASAP -- Quinine Question:?
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2 comments:
First, you want the PCA, which is found by subtracting the PRF of 14 years, since PK Calculate + pK = 14
pKa = 8.52. Find the Ka is now with the antilog function, 10 ^-pKa, Ka found. This must be equal to 3.01x10 ^ -9.
Since the conjugate acid is a weak acid (as is always the case in a buffer soln), see [H30 +] by the square root of Ka times the concentration of weak acid. We can already given molarity. I [H30 +] = 2.12x10 ^ -5.
The pH value is calculated by taking the negative logarithm of [H30 calculates] +.
pH = 4.67
Quh + + H2O -> H3O + + Qu
Ka = [Qu] [H3O +] / [Quh +]
pK = - log (Kb) = 5.48
KB = 3.31x10 ^ -6
Ka = Kw / Kb = 1x10 ^ -14 / 3.31x10 ^ -6
Ka = 3.02x10 ^ -9
Let X = moles of H3O + and hydrolysis Qu
3.02x10 ^ -9 = x ^ 2/0.15 (assuming that X \\ \\ \\ \\ \\ \\ \\ \\ u0026lt \\ \\ \\ \\ \\ \\ \\ \\ u0026lt, 0.15)
X = [H3O +] = 6.73x10 ^ -4
pH = 3.17
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