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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

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ISBN:9781305957404
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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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 base. Chemists faced with making a buffer would take a simpler approach. They would start with a solution of a weak acid with a pK, roughly equal to the pH of the buffer that was needed. To the acid they would slowly add an NaOH solution from a buret, stirring well, while at the same time measuring the pH of the solution. 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 solution of a weak acid with a known pK, and the pH of the buffer you will be asked to prepare. First, dilute the acid solu- 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 much 0.10 M NaOH you will have to add to 20 mL of your 0.10 M acid solution to produce the required ratio. This is easily done. If we add y mL of the NaOH, the value of [B-]/[HB} will become equal to y/(20 – y). Can you see why? Think about it, and you will soon see that is the case. Then complete the calculation and record the volume of NaOH that should be needed. Now do the experiment to check your prediction. Use the buret containing 0.10 M NaOH solution that has been set up by the pH meter. Record the volume before starting to add the base, noting the pH of the acid. Slowly add the NaOH to 20 mL of the acid, stirring well, and watching the pH as it slowly goes up. When you obtain a solution of the pH to be prepared, stop adding NaOH. Record the volume reading on the buret. Report the volume required to produce your buffer. Lnoid Study the buffer-
Transcribed Image Text: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 base. Chemists faced with making a buffer would take a simpler approach. They would start with a solution of a weak acid with a pK, roughly equal to the pH of the buffer that was needed. To the acid they would slowly add an NaOH solution from a buret, stirring well, while at the same time measuring the pH of the solution. 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 solution of a weak acid with a known pK, and the pH of the buffer you will be asked to prepare. First, dilute the acid solu- 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 much 0.10 M NaOH you will have to add to 20 mL of your 0.10 M acid solution to produce the required ratio. This is easily done. If we add y mL of the NaOH, the value of [B-]/[HB} will become equal to y/(20 – y). Can you see why? Think about it, and you will soon see that is the case. Then complete the calculation and record the volume of NaOH that should be needed. Now do the experiment to check your prediction. Use the buret containing 0.10 M NaOH solution that has been set up by the pH meter. Record the volume before starting to add the base, noting the pH of the acid. Slowly add the NaOH to 20 mL of the acid, stirring well, and watching the pH as it slowly goes up. When you obtain a solution of the pH to be prepared, stop adding NaOH. Record the volume reading on the buret. Report the volume required to produce your buffer. Lnoid Study the buffer-
stilsup nislqxs of noiteupo oinol 11U D. Preparing a Buffer from a Solution of a Weak Acid oisupa pH of buffer to be prepared PK, of acid oanpeH onautoe Hq Ratio of [B-V[HB] required in buffer ot nogg loasonod diw bovrsedo olea ordi ydw nelx enslhua to eelhego19 omo2 mL Volume of 0.10 M NaOH calculated (bion orh emsn) pH of acid solution before titration OF N ollud to Hq Initial volume reading of NaOH mL Final volume reading ffL HO agonb 2 to noilibbs rofts Ha mL OR 2gotb ho noitibbe ofle Hq mL Volume of NaOH actually required svedo uo no inomo How does that volume compare to your calculated value? 40
Transcribed Image Text:stilsup nislqxs of noiteupo oinol 11U D. Preparing a Buffer from a Solution of a Weak Acid oisupa pH of buffer to be prepared PK, of acid oanpeH onautoe Hq Ratio of [B-V[HB] required in buffer ot nogg loasonod diw bovrsedo olea ordi ydw nelx enslhua to eelhego19 omo2 mL Volume of 0.10 M NaOH calculated (bion orh emsn) pH of acid solution before titration OF N ollud to Hq Initial volume reading of NaOH mL Final volume reading ffL HO agonb 2 to noilibbs rofts Ha mL OR 2gotb ho noitibbe ofle Hq mL Volume of NaOH actually required svedo uo no inomo How does that volume compare to your calculated value? 40
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