![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 calculated the ratios of [CH3COONa]/[CH3COOH]. You also know that the total concentration for both buffers is 0.1M ([CH3COONa][CH3COOH] 0.1M). Now calculate the concentration of [CH3COONa] and [CH3COOH] for each buffer and write your answer in the table below. Show calculations:](http://img.homeworklib.com/questions/f1f90540-7f74-11eb-83d1-9da92551022f.png?x-oss-process=image/resize,w_560)
Homework Answers
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You will prepare two of the buffer solutions used in this lab. They are the 0.1...
I need help with this experiment please.... CHE 105 LAB MANUAL Lab 10 Report Name: 2....
I need help with this experiment please....
CHE 105 LAB MANUAL Lab 10 Report Name: 2. The chemical equation for our specific buffer system was deliberately not given in the discussion. What is the chemical equation for our buffer system? 3. The Henderson-Hasselbach equation given in the discussion had cuacau In this prelab and report, we want ICH,COOH) Want [CH,COO-Write the equation from the discussion below and then convert it to have 'CHCOOH). ICH,COD-1 in it. 4. Now, time to...
Be sure to answer all parts. Calculate the pH of the following two buffer solutions: (a)...
Be sure to answer all parts. Calculate the pH of the following two buffer solutions: (a) 1.7 M CH3COONa/2.9 M CH3COOH. (b) 0.2 M CH3COONa/0.3 M CH3COOH. Which is the more effective buffer? A. 1.7 M CH,COONa/2.9 M CH,COOH B. 0.2 M CH3COONa/0.3 M CH3COOH
1 Review Constants Periodic Table You have to prepare a pH 5.07 buffer, and you have...
1 Review Constants Periodic Table You have to prepare a pH 5.07 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH, COOH, CH3COONa, HCN, and NaCN. Correct Part B How many milliliters of each solution would you use to make approximately a liter of the buffer? Express your answers using two significant figures. Enter your answers numerically separated by a comma. IVO AXO A O 2 ? Vch. cooh , Vch,cooNa = 333,667 Submit Previous Answers...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...
Properties of Buffers Lab. I need help with problems 7 & 8. They’re pretty similar, but...
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
In lab if you must make a buffer of pH=8.5, which of the following buffer systems...
In lab if you must make a buffer of pH=8.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3C00 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
In lab if you must make a buffer of pH=3.5, which of the following buffer systems...
In lab if you must make a buffer of pH=3.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3COO 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
Please help with Buffer 3 ! Part 1 (15 pts) A. Buffer 1 Mix 10.0 ml...
Please help with Buffer 3 !
Part 1 (15 pts) A. Buffer 1 Mix 10.0 ml of 10 M CHCOOH and 25.0 ml of 10 M sodium acetate (NaCH.COO). Calculate the expected pH. PH-pk + log CH, COOH NACH.COD Cacid] V=10mL V = 25mL I PM - 4.74 + log [25x!! 30x17 M.1.0M (M-1.0M ? pH 4.+ 10 3 (2) IPH: 5.1 B. Buffer 2 Mix 30.0 ml of 1.0 M CH.COOH and 5.0 mL of 1.0 M sodium acetate...
B. pH of Buffer Solutions Follow the instruction in the lab book for making the buffer...
B. pH of Buffer Solutions Follow the instruction in the lab book for making the buffer solution. Mass of NaCHC003H20 (FN= 136 g/mhol)--2209___ Moles of CH3COO Concentration of CH3COOH Volume of CH3COOH (mL) Moles of CH3COOH .OML o22 nol Analysis of Buffer Solution Measured pH of Buffer Solution Calculated pH of Buffer Solution (show work) 1. [conjugate base] weak acid to calculate the pH.
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
I need help with this experiment please....
CHE 105 LAB MANUAL Lab 10 Report Name: 2. The chemical equation for our specific buffer system was deliberately not given in the discussion. What is the chemical equation for our buffer system? 3. The Henderson-Hasselbach equation given in the discussion had cuacau In this prelab and report, we want ICH,COOH) Want [CH,COO-Write the equation from the discussion below and then convert it to have 'CHCOOH). ICH,COD-1 in it. 4. Now, time to...
Be sure to answer all parts. Calculate the pH of the following two buffer solutions: (a) 1.7 M CH3COONa/2.9 M CH3COOH. (b) 0.2 M CH3COONa/0.3 M CH3COOH. Which is the more effective buffer? A. 1.7 M CH,COONa/2.9 M CH,COOH B. 0.2 M CH3COONa/0.3 M CH3COOH
1 Review Constants Periodic Table You have to prepare a pH 5.07 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH, COOH, CH3COONa, HCN, and NaCN. Correct Part B How many milliliters of each solution would you use to make approximately a liter of the buffer? Express your answers using two significant figures. Enter your answers numerically separated by a comma. IVO AXO A O 2 ? Vch. cooh , Vch,cooNa = 333,667 Submit Previous Answers...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
In lab if you must make a buffer of pH=8.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3C00 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
In lab if you must make a buffer of pH=3.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3COO 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
Please help with Buffer 3 !
Part 1 (15 pts) A. Buffer 1 Mix 10.0 ml of 10 M CHCOOH and 25.0 ml of 10 M sodium acetate (NaCH.COO). Calculate the expected pH. PH-pk + log CH, COOH NACH.COD Cacid] V=10mL V = 25mL I PM - 4.74 + log [25x!! 30x17 M.1.0M (M-1.0M ? pH 4.+ 10 3 (2) IPH: 5.1 B. Buffer 2 Mix 30.0 ml of 1.0 M CH.COOH and 5.0 mL of 1.0 M sodium acetate...
B. pH of Buffer Solutions Follow the instruction in the lab book for making the buffer solution. Mass of NaCHC003H20 (FN= 136 g/mhol)--2209___ Moles of CH3COO Concentration of CH3COOH Volume of CH3COOH (mL) Moles of CH3COOH .OML o22 nol Analysis of Buffer Solution Measured pH of Buffer Solution Calculated pH of Buffer Solution (show work) 1. [conjugate base] weak acid to calculate the pH.
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
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