D. Preparation of a Buffer from a Solution of a Weak Acid So far in this experiment the buffers that we used were made up from a weak acid and its conjugate Chemists faced with making a buffer would take a simpler approach. They would start with a solutic weak acid with a pK, roughly equal to the pH of the buffer that was needed. To the acid they would add an NaOH solution from a buret, stirring well, while at the same time measuring the pH of the so When they got to the desired pH, they would stop adding the NaOH. The buffer would be ready to use In this part of the experiment you are to work alone. We will furnish you with an 0.50 M solutic weak acid with a known pK, and the pH of the buffer you will be asked to prepare. First, dilute the acie tion to 0.10 M by adding 10 mL of the acid to 40 mL water in a 100 mL beaker and stirring well. Using Equation 4b, calculate the ratio of [B] to [HB] in the buffer to be prepared. Calculate how- 0.10 M NaOH you will have to add to 20 mL of your 0.10 M acid solution to produce the required ratic is easily done. If we add y mL of the NaOH, the value of [B-]/[HB} will become equal to y/(20 – y). C= see why? Think about it, and you will soon see that is the case. Then complete the calculation and recc volume of NaOH that should be needed. Now do the experiment to check your prediction. Use the buret containing 0.10 M NaOH solutic has been set up by the pH meter. Record the volume before starting to add the base, noting the pH of th- Slowly add the NaOH to 20 mL of the acid, stirring well, and watching the pH as it slowly goes up. Whe obtain a solution of the pH to be prepared, stop adding NaOH. Record the volume reading on the buret. the volume required to produce your buffer. 0oid Study the
D. Preparation of a Buffer from a Solution of a Weak Acid So far in this experiment the buffers that we used were made up from a weak acid and its conjugate Chemists faced with making a buffer would take a simpler approach. They would start with a solutic weak acid with a pK, roughly equal to the pH of the buffer that was needed. To the acid they would add an NaOH solution from a buret, stirring well, while at the same time measuring the pH of the so When they got to the desired pH, they would stop adding the NaOH. The buffer would be ready to use In this part of the experiment you are to work alone. We will furnish you with an 0.50 M solutic weak acid with a known pK, and the pH of the buffer you will be asked to prepare. First, dilute the acie tion to 0.10 M by adding 10 mL of the acid to 40 mL water in a 100 mL beaker and stirring well. Using Equation 4b, calculate the ratio of [B] to [HB] in the buffer to be prepared. Calculate how- 0.10 M NaOH you will have to add to 20 mL of your 0.10 M acid solution to produce the required ratic is easily done. If we add y mL of the NaOH, the value of [B-]/[HB} will become equal to y/(20 – y). C= see why? Think about it, and you will soon see that is the case. Then complete the calculation and recc volume of NaOH that should be needed. Now do the experiment to check your prediction. Use the buret containing 0.10 M NaOH solutic has been set up by the pH meter. Record the volume before starting to add the base, noting the pH of th- Slowly add the NaOH to 20 mL of the acid, stirring well, and watching the pH as it slowly goes up. Whe obtain a solution of the pH to be prepared, stop adding NaOH. Record the volume reading on the buret. the volume required to produce your buffer. 0oid Study the
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...
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ka = 1.8 x 10^-5
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