Question

Ibuprofen is a drug sold as a nonprescription anti-inflammatory medication. 3.21 CH, о C-OH H,O (CH3)2CHCH2 CH CH, о CH-C-O HO АН ibuprofen (pK, 4.43) (CH) CHCH- A (a) What are the concentrations of ibuprofen and its conjugate base if 10 mole of ibuprofen is dissolved in an aqueous solution containing a large excess of a buffer at pH 5.0?

Answer 1

The answer is provided in the attachment .

from the Henderson - Hasselboleh' equation of acidie buffer, we have . [conjugute base pH=pka+log 7 Lacid] pH= 5.0, pką= 9.43 Now, miñally, ibuprofen was at 10-4 mole amount. E Then after adding it in water, let 'n mole converts to conjugare base. Thus, (8-9 n mole remains as acid. So, from equation - 5.0= 4:43+ log in Or, 0.57=logoran or o ran = 3:72 Or, 4.72n =10-1*372 Or, x= 7.88x10-5 mole . 109_2= 2-12x10-5 mole. Thus, ibuprofen remains 212*405 mole ? Conjugale base formed 7.888305 wale. IAnswer?