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12 Question 24 (4 points) You are asked to go into the lab and prepare an...
You will prepare two of the buffer solutions used in this lab. They are the 0.1...
You will prepare two of the buffer solutions used in this lab. They are the 0.1 M CHaCOOH/CH3COONa buffer at pH- 4.74 and at pH-6. You will need to write your own procedure for the preparation of these buffers. To write the procedure, study the manual and follow the pre-lab questions. Using Henderson-Hasselbach equation to calculate the ratio of [CH,COONa/[CH COOH] for each buffer and write your answers in the table on the right. Show calculations: 1. 2. You just...
5. You are asked to prepare an acetate buffer solution at pH 4.6. Use the Henderson-Hasselbalch...
5. You are asked to prepare an acetate buffer solution at pH 4.6. Use the Henderson-Hasselbalch equation to calculate the ratio of sodium acetate and acetic acid required to prepare a buffer at pH 4.6. 6. If you had 500mL of 0.200M sodium acetate buffer pH4.76, how many mL of 1.00M HCI would you need to add to adjust the pH to 4.60?
When you go to prepare the buffer described in the previous problem, you discover that your...
When you go to prepare the buffer described in the previous problem, you discover that your laboratory is out of sodium acetate. But you do have sodium hydroxide. How much (in mol and g) acetic acid and sodium hydroxide do you need to make the buffer? (Previous problem: You wish to prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acetate concentration of 250 mM and a pH of 5.0. What concentrations of...
If you are to prepare a 1.000 L of a 0.100 M buffer at pH 5.00...
If you are to prepare a 1.000 L of a 0.100 M buffer at pH 5.00 using the CH3COOH/ Na+CH3COO- buffer system (pKa 4.76a), answer the following questions: What is the molar ratio of the base to acid at pH 5.0? The concentration of the buffer (0.100 M in this example) refers to the sum of the weak acid and its conjugate base. Given this information, what is the concentration of the weak acid and its conjugate base at pH...
During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2)...
During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2) of the same pH (pH = 4.0), but with different concentration of the components. Use the Henderson -Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 x 10-5 M. a. Buffer A: Calculate the mass of the solid sodium acetate (NaC2H3O2) required to mix with 100 ml of 0.1 M acetic acid (HC2H3O2), to prepare a pH 4 buffer....
You must prepare a solution to use as an environment that involves a particular strain of...
You must prepare a solution to use as an environment that involves a particular strain of bacteria that has a very limited pH range in which it can survive. This bacteria needs a medium with a pH = 6.10. You are tasked with making 500 mL buffer for this bacterium given the following reagents available to you in the lab, these are in the table b. State which reagent(s) and exactly how much you used of each to create the...
can you please write the calculations with clear writing and explanations and thank you (3) (4)...
can you please write the calculations with clear
writing and explanations and thank you
(3) (4) B) Preparation a) Place about 50 ml of distilled water in a 0.1 liter volumetric flask. b) Use a 1 ml pipette to transfer 0.83 ml of conc. HCl to the flask. Add distilled water until the volume is 0.1 liter. Save for later use. Prepare 0.1 liter of 0.1 M sodium hydroxide (MW= 40.0 (skip this exercise)). A) Calculations B) Preparation Prepare 0.1...
12. You are asked to prepare 500. mL of a 0.200 M acetate buffer at pH...
12. You are asked to prepare 500. mL of a 0.200 M acetate buffer at pH 4.90 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76), 3.00 M NaOH, and water. Answer the following questions regarding the preparation of the buffer. a) How many grams of acetic acid will you need to prepare the 500 mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. g=? B) What volume of 3.00 M...
In your pre-lab, we asked you to consider a few of the properties you could measure...
In your pre-lab, we asked you to consider a few of the properties you could measure during the titration of a 100.0 mL sample of 1.0 M acetic acid, CH3COOH (Ka = 1.8 x 10-5) with 0.50 mol/L NaOH solution at 25°C. Let's think about this same titration again, this time at the molecular-scale. Question 2 (1 point) After you have added a total of 100.0 mL of NaOH (aq), what are the major species in your beaker other than...
Please help with the prelab questions! thank you!!!! Especially 2 and 3! Pre-Lab Questions 1. Calculate...
Please help with the prelab questions! thank you!!!!
Especially 2 and 3!
Pre-Lab Questions 1. Calculate the theoretical equivalence point (the volume!) in terms of ml NaOH adde each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2. Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa. What is the pH after...
You will prepare two of the buffer solutions used in this lab. They are the 0.1 M CHaCOOH/CH3COONa buffer at pH- 4.74 and at pH-6. You will need to write your own procedure for the preparation of these buffers. To write the procedure, study the manual and follow the pre-lab questions. Using Henderson-Hasselbach equation to calculate the ratio of [CH,COONa/[CH COOH] for each buffer and write your answers in the table on the right. Show calculations: 1. 2. You just...
5. You are asked to prepare an acetate buffer solution at pH 4.6. Use the Henderson-Hasselbalch equation to calculate the ratio of sodium acetate and acetic acid required to prepare a buffer at pH 4.6. 6. If you had 500mL of 0.200M sodium acetate buffer pH4.76, how many mL of 1.00M HCI would you need to add to adjust the pH to 4.60?
can you please write the calculations with clear
writing and explanations and thank you
(3) (4) B) Preparation a) Place about 50 ml of distilled water in a 0.1 liter volumetric flask. b) Use a 1 ml pipette to transfer 0.83 ml of conc. HCl to the flask. Add distilled water until the volume is 0.1 liter. Save for later use. Prepare 0.1 liter of 0.1 M sodium hydroxide (MW= 40.0 (skip this exercise)). A) Calculations B) Preparation Prepare 0.1...
In your pre-lab, we asked you to consider a few of the properties you could measure during the titration of a 100.0 mL sample of 1.0 M acetic acid, CH3COOH (Ka = 1.8 x 10-5) with 0.50 mol/L NaOH solution at 25°C. Let's think about this same titration again, this time at the molecular-scale. Question 2 (1 point) After you have added a total of 100.0 mL of NaOH (aq), what are the major species in your beaker other than...
Please help with the prelab questions! thank you!!!!
Especially 2 and 3!
Pre-Lab Questions 1. Calculate the theoretical equivalence point (the volume!) in terms of ml NaOH adde each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2. Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa. What is the pH after...
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