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Please record your answers directly onto these pages. Show all work for full credit. 1. A...
please show work :) 7. You need to make a buffer to keep a solution at...
please show work :)
7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K4 = 1.40 x 103) and sodium chloroacetate 2. Formic acid (Ka = 1.77 x 10-4) and sodium formate 3. Iodic acid (Ka = 1.60 x 10-1) and sodium iodate 4. Phosphoric acid (K. = 7.52 x 10-3) and sodium phosphate 5. Propionic...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa)...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
please explain how you got all your answers 10. Calculate the pH of a 0.30 M...
please explain how you got all your answers
10. Calculate the pH of a 0.30 M formic acid solution. (K-1.8 x 10") Weak monoprotic acid. 11. Calculate the K, for a 0.050 M solution of HA (weak acid) if the pH = 4.65. 12. What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25C? (K. of F = 1.4 x 10) 13. Which of...
show work please! (they are two different problems & that is all im given/ asked for)...
show work please! (they are two different problems & that is
all im given/ asked for)
1. You are asked to prepare 10.00 mL of a buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A). The target pH of the buffer solution is 5.45. The K, of HA is 5.0 x 10-6. What volume of A is required to make the buffer? You must show your work to receive credit, (3 pts.) d. Aujus...
In the following questions write your answers with the detailed steps. Show all necessary equations or...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H12O6) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
In the following questions write your answers with the detailed steps. Show all necessary equations or...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H1206) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
Please answer #2 php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your...
Please answer #2
php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your work. Don't forget the significant figures and units!! Would the following mixtures result in buffer solutions? (Justify your answers) 1. a 100.0 ml, of 0.10 M NH, 100.0 mL of0.15 M NHaCl b. 50.0 mL of 0.10 M HCIO4, 35.0 mL if 0.15 M NaCIO c. 125.0 ml, of 0.15 CH?NH2. 120.0 mL of 0.25 M CHNE ICI d. 165.0 mL of 0.10 M...
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...
1. 2. 3. 4. 5. please show all work What is the concentration of the acetate...
1.
2.
3.
4.
5.
please show all work
What is the concentration of the acetate ion in a 1.00 M CH3COOH solution given that the K, of CH3COOH is 1.8 x 10-5? a. 4.20 x 10-3 M d. 2.84 x 10-4 M b. 0.996 M e. 5.62 x 10-5 M c. 1.00 M Methylamine (CH3NH2) is a weakly basic compound. Calculate the Ky for methylamine if a 0.253 M solution is 4.07% ionized. a. 2.29 x 103 d. 4.24...
1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M...
1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M nitric acid, HNO3 b. 0.50 M hydrocyanic acid, HCN Ka = 4.0 x 10-10 2. A student was given the following problem: Calculate the pH of a 0.50 Mama bromide (NHaBr) solution if the Kb of NH3 is 1.8 x 10. The student provided the fo work. Identify the error(s) and calculate the correct pH. NH; (aq) + H20 (1) = NH3 (aq) +...
please show work :)
7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K4 = 1.40 x 103) and sodium chloroacetate 2. Formic acid (Ka = 1.77 x 10-4) and sodium formate 3. Iodic acid (Ka = 1.60 x 10-1) and sodium iodate 4. Phosphoric acid (K. = 7.52 x 10-3) and sodium phosphate 5. Propionic...
4) Show your work to get full credit. (a) How much in g) sodium acetate (CH3COONa) must be added to 100 mL 0.1 M CH3COOH solution to prepare a buffer solution with pH 4.90? (assume no change in volume) (b) What will be the pH of the final solution if 2.50 x 10 mol HCl solution is added to the buffer solution above? (c) What will be the pH of the solution if 2.00 x 10 mol NaOH solution is...
please explain how you got all your answers
10. Calculate the pH of a 0.30 M formic acid solution. (K-1.8 x 10") Weak monoprotic acid. 11. Calculate the K, for a 0.050 M solution of HA (weak acid) if the pH = 4.65. 12. What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25C? (K. of F = 1.4 x 10) 13. Which of...
show work please! (they are two different problems & that is
all im given/ asked for)
1. You are asked to prepare 10.00 mL of a buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A). The target pH of the buffer solution is 5.45. The K, of HA is 5.0 x 10-6. What volume of A is required to make the buffer? You must show your work to receive credit, (3 pts.) d. Aujus...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H12O6) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H1206) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
Please answer #2
php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your work. Don't forget the significant figures and units!! Would the following mixtures result in buffer solutions? (Justify your answers) 1. a 100.0 ml, of 0.10 M NH, 100.0 mL of0.15 M NHaCl b. 50.0 mL of 0.10 M HCIO4, 35.0 mL if 0.15 M NaCIO c. 125.0 ml, of 0.15 CH?NH2. 120.0 mL of 0.25 M CHNE ICI d. 165.0 mL of 0.10 M...
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...
1.
2.
3.
4.
5.
please show all work
What is the concentration of the acetate ion in a 1.00 M CH3COOH solution given that the K, of CH3COOH is 1.8 x 10-5? a. 4.20 x 10-3 M d. 2.84 x 10-4 M b. 0.996 M e. 5.62 x 10-5 M c. 1.00 M Methylamine (CH3NH2) is a weakly basic compound. Calculate the Ky for methylamine if a 0.253 M solution is 4.07% ionized. a. 2.29 x 103 d. 4.24...
1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M nitric acid, HNO3 b. 0.50 M hydrocyanic acid, HCN Ka = 4.0 x 10-10 2. A student was given the following problem: Calculate the pH of a 0.50 Mama bromide (NHaBr) solution if the Kb of NH3 is 1.8 x 10. The student provided the fo work. Identify the error(s) and calculate the correct pH. NH; (aq) + H20 (1) = NH3 (aq) +...
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