Reliever Fever
GREAT Reliever Fever DEALS BELOW THE ARTICLES
Can anyone solve these chemistry problems?
1. Calculate the percentage of dissociation of propionic acid in a solution of 0.075 M propionic acid at 298 K. CH 3CH2COOH (Aq) + H2O = CH3CH2COO-(aq) + H3O + (aq) Kc = 1.3 × 10-5 at 298 K. 2 .. Acetylsalic acid (aspirin) HC9H7O4, is widely used the pain and fever. Find the pH of 0.042 M aqueous aspirin body temperature (37 ° C Ka = 0.00060). 3 .. A solution 0.036 M of a weak acid (HA) has a pH of 4.51. What is the Ka of the acid?
[CH3CH2OO]] [H /] [CH3CH2COOH = 1.3 x 10-5 is not response? Just multiply by 100% in putting the means to solve these problems is to write the equation, then drag the right side of the equation the left so that: C9H7O4 + HI = HC9H7O4 left the + / - OUT. The difference between the first issue and that is that the Kc as you call it is a measure of dissociation. Here, they want to know the concentration of [] of a product that gives you the original concentraction. [C9H704] [H] / [HC9H7O4] = 0.00060 We know that the concentration H is equal to that of C9H7O4, and that the concentration of aspirin is 0.42 mol / liter. So the solution is x ^ 2 / (0.42-x) = 0.00060, which gives an equation quadratic. solve. Remember that if there was a 2 before a component, then its conc. shape to be square, cube 3, etc, you must make some assumptions here. Suppose yeilds acid to a single H and dissasssociates completely and no problems with pH balance varies over time, as some weak acids. If the simple HA = H + A pH =- log [H] [H] = [A] = x [H] * [A] / [HA] = Ka with [HA] = 0.036 - You get xx ^ 2 / (0.036 - X) = Ka
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