# grenoble

using the hasselbach-Handerson equation calculate the fraction of asprin Pka is 5.6 and PH is 8.6?

1. 👍 0
2. 👎 0
3. 👁 108

http://search.yahoo.com/search?fr=mcafee&p=hasselbach-Handerson+equation

For the calculation itself, you might find something useful in some of the following:

http://search.yahoo.com/search?fr=mcafee&p=calculate+the+fraction+of+asprin+Pka+is+5.6+and+PH+is+8.6%3F

Sra

1. 👍 0
2. 👎 0
2. Do you want the fraction [A-]/[HA] dissociated?

[Your value for the pKa for aspirin is low from memory =about 3.5??]

From the H-H equation

pH=pKa+log([A-]/[HA])

8.6=5.6 + log([A-]/[HA])

3.0=log([A-]/[HA])

so

10^+3 = [A-]/[HA]

1. 👍 0
2. 👎 0

## Similar Questions

1. ### chemistry

Asprin, C9H8O4, is prepared by reacting salicylic acid, C7H6O3, with acetic anhydride, C4H6O3, in the reaction C7H6O3(s) + C4H6O3(l) -> C9H8O4(s) + C2H4O2(l) A student is told to prepare 45.0 g of aspirin. She is also told to use

asked by Chris on October 18, 2006
2. ### chemistry

The weak acid HQ has pKa of 4.89. 1)Calculate the [H3O+] of .035 M HQ. 2)Calculate the (OH-) of 0.500 M HQ ....Am I correct? a) pKa = 4.89 => - log(Ka) = 4.89 => Ka = antilog(- 4.89) = 10-4.89 = 1.29x10-5 1. Given concentration of

asked by patrick on October 4, 2015
3. ### Chemistry, acids and bases

(a) Find pH and pOH of 1.0 M solution of sodium benzoate, NaC6H5COO. (Ka of benzoic acid is 6.2x10^-5) (b) Calculate pH after 0.205 moles per liter of HCl was added (assume volume does not change (c) Calculate pH after 1.0 moles

asked by Marissa on May 6, 2008
4. ### Chemistry

100 mL of 1.0 M formic acid (HCOOH) is titrated with 1.0 M sodium hydroxide (NaOh). The Approximate pKa is 4 At the pKa, what fraction of the carboxyl group will have been converted to COO-?

asked by Aria on September 27, 2013
5. ### chemistry buffers

What molar ratio of HPO4 2- to H2PO4 - in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotonic acid, has pKa values: 2.14, 6.86, and 12.4. Only one of the pKa values is relevant here. how do i know which pka

asked by ron on September 9, 2012
1. ### Biochem

You prepare a 1L solution of 0.5 M imidazole. (pKa= 7.05). Calculate the pH of the solution after you add 0.1 moles of HCl. I need to create an ICE table. I also know I need to use the Henderson- Hasselbalch equation but I'm

asked by Ashley on September 23, 2016
2. ### chemistry

Which of the following 0.10 M aqueous solutions gives the LOWEST pH? 1. CH3COOH (pKa = 4.75) 2. CCl3COOH (pKa = 0.52) 3. HF (pKa = 3.45) 4. H3PO4 (pKa1 = 2.12) 5. Because all are acids, the pH is the same for all solutions

asked by Anonymous on April 26, 2015
3. ### Chemistry

A 35.0 mL sample of 0.150 M acetic acid is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: a) 0mL, b) 17.5 mL, c) 34.5 mL, d) 35 mL I've figured out a,b, and c. But at 35

asked by Anonymous on October 28, 2010
4. ### chemistry

The pH of a 0.164 M aqueous solution of dimethylamine is 11.98. Write the ionization equation, calculate the values of Kb and pKa and comment on strength of the

asked by nica on September 27, 2013
5. ### Chemistry

A buffer is made up of .300 L each of .500 M KH2PO4 and .317 M K2HPO4. Assuming tha the volumes are additive, calculate a) the pH of the buffer b) the pH of the bugger after the addition of .0500 mol of HCl to .600 L of the

asked by James on May 1, 2007
6. ### chemistry

I have already posted this and never got a response, please help. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of

asked by student on February 3, 2008