Question

If two aspirin tablets, each having a mass of 325 mg, are dissolved in a full stomach whose volume is 1 L and whose pH is 2, what percent of the aspirin is in the form of neutral molecules?

Answer 1

Answer:

99.7 %

Explanation:

pH = pKa + log(B/A)

In this case, the basic form is the charged form. The neutral form is the acid, because aspirin is o-acetyl benzoic acid

pKa = -log (ka) = 4.53

2 - 4.53 = log(b/a) = -2.53

10^(-2.53) = 0.00288

so, that means that Base/Acid = 0.0028 / 1

so, total is .00288 + 1 = 1.00288

and the percent of acid is 1/1.00288 x100%= 99.7 %

Answer 2

The percentage of aspirin in the form of neutral molecules will be equal to 99.7%

How can we arrive at this result?

• We will use the equation: $pH = pKa + log(B/A)$

As aspirin is an acid, let's assume that the base form of the substance is electrically charged, but the acid form is neutral, that is, it has no charge.

• We can solve the equation as follows:

$pK_a = -log (ka) = 4.53\\2 - 4.53 = log(b/a) = -2.53\\10^(^-^2^.^5^3^) = 0.00288\\Base/Acid = 0.0028 / 1 --------------- .00288 + 1 = 1.00288$

• To obtain this value in percentage, we must multiply it by 100, as shown below:

$1/1.00288 *100= 99.7$%

More information about acid and base at the link:

https://brainly.com/question/15192126