Homework Answers
1)
High buffer capacity can be defined as the ability of a buffer solution to resist in changes in pH by addition of the maximum amount of acid or base. The buffer capacity is greatest when there are equal amounts of weak acid and conjugate base or weak base and conjugate acid. present in buffer solution.
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Post Lab Questions: To receive full credit, you must SHOW ALLOON 1. What is meant when...
Post Lab Questions: To receive full credit, you must SHOW ALL YOUR WORKI 1. What is...
Post Lab Questions: To receive full credit, you must SHOW ALL YOUR WORKI 1. What is meant when one says that a buffer has a high buffer capacity? 2. What differences did you notice when you added acid or base to distilled water as compared to the buffer solutions? 3. The blood buffer system is made up of H2CO3 and HCO3-. Describe with the use of equations how this system responds to added H3O* and to added OH-. POST LAB...
2. What differences did you notice when you added acid or base to distilled water as...
2. What differences did you notice when you added acid or base to distilled water as compared to the buffer solutions? The blood buffer system is made up of H2CO, and HCO3-. Describe with the use of equations how this system responds to added H3O* and to added OH". 4. Looking at the fractional speciation curve, what is important about the point of intersection between the intermediate species and both the acidic species and basic species? Compare the same point...
You must show your work to receive credit. pH = -log[H₂O 1.(4 pts) For each [H3O+]...
You must show your work to receive credit. pH = -log[H₂O 1.(4 pts) For each [H3O+] below, give the pH. a. 8.7 x 10-8 M b. 7.9 x 100M 17.06 18. 2. (4 pts) For each [OH-] below, give the [H3O+] a. 10.0 x 10-6 M b. 8.4 x 10-M 1x 10 9 3. (4 pts) For each pH below, give the [H30“). 10 a. 8.5 b. 2.9 ..th 0:1.0*11- Сен 10 P7 13.16 *10-9 11.26 x 10-3 4. (4...
A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of...
A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of water. Which statement about the solution is correct? A)The solution is basic. B) The solution is C) The solution is weakly acidic. D) The solution is strongly acidic. E The values for K_a and K_b for the species in solution must be known before a prediction can be made. The pH of blood is 7.35. It is maintained in part by the buffer system...
A thorough explanation would sure be appreciated!!!! Thank you!! Acid-Base Chemistry: Unknown Acid Analysis (in two...
A thorough explanation would sure be appreciated!!!!
Thank you!!
Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka...
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka NH,OH) with 0.01 M HCI. Stir. Measure the pH values of the solutions. Plot the titration curve on the same graph with your strong acid/strong base and weak acid/strong base titration curves. Compare with the computer-simulated curve (Figure 14.7). NOTE: Data from the computer calculation give an equivalence point pH of 5.70 at 5.0 drops of added 0.01 M HCI. Observations: Lane 1-purple (pH...
Question 3 1 pts Which statement accurately describes what happens in a buffer solution when you...
Question 3 1 pts Which statement accurately describes what happens in a buffer solution when you add strong acid or strong base? The strong species is converted to weak species by reaction The pH change is smaller than you expect based on the amount of acid or base added Two reactions occurs-first a completion reaction, then an equilibrium reaction All three statements above accurately describe this situation Question 4 Can you create a buffer by mixing HNO3 with KOH? Yes-...
please help with my pre lab additional information Pre-Lab Questions: 1. What is the definition of...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
Pre-Lab Calculating pH and Buffer Capacity (You must show work for credit) Name: 1. Calculate the...
Pre-Lab Calculating pH and Buffer Capacity (You must show work for credit) Name: 1. Calculate the volume of glacial acetic acid (17.6 M) and mass of sodium acetate (mm 82.03) required to make 102 ml of 0.20 M buffer at pH 4.85. The Ka of acetic acid is 1.4 x10. (this question is challenging, use the background section and your book for help). 2. Consult the table of Ka values in the back of your textbook and suggest acid/conjugate base...
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...
Post Lab Questions: To receive full credit, you must SHOW ALL YOUR WORKI 1. What is meant when one says that a buffer has a high buffer capacity? 2. What differences did you notice when you added acid or base to distilled water as compared to the buffer solutions? 3. The blood buffer system is made up of H2CO3 and HCO3-. Describe with the use of equations how this system responds to added H3O* and to added OH-. POST LAB...
2. What differences did you notice when you added acid or base to distilled water as compared to the buffer solutions? The blood buffer system is made up of H2CO, and HCO3-. Describe with the use of equations how this system responds to added H3O* and to added OH". 4. Looking at the fractional speciation curve, what is important about the point of intersection between the intermediate species and both the acidic species and basic species? Compare the same point...
You must show your work to receive credit. pH = -log[H₂O 1.(4 pts) For each [H3O+] below, give the pH. a. 8.7 x 10-8 M b. 7.9 x 100M 17.06 18. 2. (4 pts) For each [OH-] below, give the [H3O+] a. 10.0 x 10-6 M b. 8.4 x 10-M 1x 10 9 3. (4 pts) For each pH below, give the [H30“). 10 a. 8.5 b. 2.9 ..th 0:1.0*11- Сен 10 P7 13.16 *10-9 11.26 x 10-3 4. (4...
A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of water. Which statement about the solution is correct? A)The solution is basic. B) The solution is C) The solution is weakly acidic. D) The solution is strongly acidic. E The values for K_a and K_b for the species in solution must be known before a prediction can be made. The pH of blood is 7.35. It is maintained in part by the buffer system...
A thorough explanation would sure be appreciated!!!!
Thank you!!
Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka NH,OH) with 0.01 M HCI. Stir. Measure the pH values of the solutions. Plot the titration curve on the same graph with your strong acid/strong base and weak acid/strong base titration curves. Compare with the computer-simulated curve (Figure 14.7). NOTE: Data from the computer calculation give an equivalence point pH of 5.70 at 5.0 drops of added 0.01 M HCI. Observations: Lane 1-purple (pH...
Question 3 1 pts Which statement accurately describes what happens in a buffer solution when you add strong acid or strong base? The strong species is converted to weak species by reaction The pH change is smaller than you expect based on the amount of acid or base added Two reactions occurs-first a completion reaction, then an equilibrium reaction All three statements above accurately describe this situation Question 4 Can you create a buffer by mixing HNO3 with KOH? Yes-...
please help with my pre lab
additional information
Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
Pre-Lab Calculating pH and Buffer Capacity (You must show work for credit) Name: 1. Calculate the volume of glacial acetic acid (17.6 M) and mass of sodium acetate (mm 82.03) required to make 102 ml of 0.20 M buffer at pH 4.85. The Ka of acetic acid is 1.4 x10. (this question is challenging, use the background section and your book for help). 2. Consult the table of Ka values in the back of your textbook and suggest acid/conjugate base...
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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