00:01
For part a, we need to write the ionization equilibrium of the acetyl salicylic acid.
00:08
That is hc9 h704.
00:13
So we have hc9 h704.
00:18
That would be aquius.
00:22
So we have hydrogen ions and also c9 h704 in aquius solution.
00:32
Assume that the equilibrium concentration of your hydrogen ions and that of your c9h704 is equal to x capital m.
00:45
So the equilibrium concentration of aspirin would be 0 .20 minus xm.
00:54
The ka expression is as follows.
00:57
So we have ka is equals to hydrogen ions.
01:02
C9 h704 over hc9 h704 we need to substitute the equilibrium values and the ka values so we have 3 .0 times 10 raised to the power 4 we have x times x over 0 .20 minus x since 3 .0 times 10 raised to the power of negative 4 is less than 0 .20.
01:39
Assume that 0 .20 minus x is equals to 0 .20.
01:46
So 3 .0 times 10 raised the power of negative 4, it will be x squared over 0 .20.
01:54
So our x will become 0 .0077.
02:01
Now we need to calculate the percent ionization as follows.
02:07
The percent ionization so to get the percent ionization we have hydrogen ions over h c9 h704 this would be the initial times 100 percent hydrogen ion will be our x we have hc9 h704 times 100 percent hydrogen ion will be our x'd we have hc9 h704 times 100 percent and our x is 0 .007m over 0 .20 times 100%.
02:53
So the percent ionization will be 3 .9%.
02:58
For ionization of aspirin, there would be 3 .9%.
03:05
For part b, we need to calculate the ph of the stomach, which is in 1 .0...