Homework Answers
Answer:-
This question is solved by using the simple concept of dissociation of a weak acid then determination of its using the expression of Ka and its value.
The answer is given in the image,
![Answer: CcH₃cOg H] = 0.0185m usume - Soom CNovИ] - 0.JpooM & : 4.46 Kee lo-pко - 1-4-46 a> 1.74 Xlo-5 S- x x е) си,и +50 г си](http://img.homeworklib.com/questions/1022a9e0-e015-11eb-9a23-333bf32dc58d.png?x-oss-process=image/resize,w_560)
![Hoot] = 5.58810-4m PH = -log[hzot] Puz-log (5.58X10-41 PH=3-25 ) Molecos Mach z Moles of cazc02H 0.1000XV=0.0185x5.00 V=0.925](http://img.homeworklib.com/questions/10ba3560-e015-11eb-ae2c-434728916a29.png?x-oss-process=image/resize,w_560)
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9. Acetic acid (CH3CO,H) has a pk of 4.76 at 25°C. A 5.00 mL aliquot of...
9. Acetic acid (CH3CO2H) has a pk of 4.76 at 25°C. A 5.00 mL aliquot of...
9. Acetic acid (CH3CO2H) has a pk of 4.76 at 25°C. A 5.00 mL aliquot of a 0.0185 M solution of acetic acid is titrated with a 0.1000 M standardized solution of NaOH. (a) What is the pH of the acetic acid solution before any of the standardized solution is added? (b) What volume of the standardized solution is necessary to reach the equiv- alence point? (c) What is the pH of the solution after 1.48 mL of the standardized...
9. Acetic acid (CH,CO,H) asap. of 4 M solution of acetic acid is titrated with NAOH...
9. Acetic acid (CH,CO,H) asap. of 4 M solution of acetic acid is titrated with NAOH C A5.00 mL aliquot of a 0.0185 0.1000 M standardized solution of (a) What is the pH of the Netheld solution before any of the standardized solution is added? (b) What volume of the standardized solution is necessary to reach the equiv- alence point? (c) What is the pH of the solution after 1.48 mL of the standardized solution is added?
in an experiment, 5.00 mL 0.100 M acetic acid (Ka = 1.75 x 10^-5 at 25...
in an experiment, 5.00 mL 0.100 M acetic acid (Ka = 1.75 x 10^-5 at 25 C) was titrated with 0.100 M NaOH solution. The system will attain this pH after 10.0 mL of the titrant has been added
Weak-Acid Strong-Base Titrations. These next questions relate to a 25 mL aliquot of 0.35 M acetic acid (Ka = 1.77 x...
Weak-Acid Strong-Base Titrations. These next questions relate to a 25 mL aliquot of 0.35 M acetic acid (Ka = 1.77 x 10) that is titrated with 0.20 M potassium hydroxide (KOH). (f) What is the pH of the acetic acid solution before the titration begins? (g) What is the pH after 14 mL of 0.20 M KOH has been added to the solution? Use the Henderson-Hasselbalch equation. (h) What is the pH at the equivalence point?
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, PK: - 3.74) is...
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, PK: - 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution 6. After the addition of 20.00 mL of NaOH solution C. After the addition of 25.00 mL of NaOH solution d. At what volume of added NaOH will pH -pK
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, pK, = 3.74) is...
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, pK, = 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution. b. After the addition of 20.00 mL of NaOH solution c. After the addition of 25.00 mL of NaOH solution. d. At what volume of added NaOH will pH =pK,
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pK...
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pK = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume:
Question 2 15 P Weak Acid Titration Calculations. A 25.0 mL aliquot of 0.50 M propanoic...
Question 2 15 P Weak Acid Titration Calculations. A 25.0 mL aliquot of 0.50 M propanoic acid (CH3CH2O2H) is placed in a 250 mL Erlenmeyer flask and titrated with a standardized solution of 0.25 M NaOH. The pKof propanoic acid is 4.88. Calculate the pH of the solution after the addition of the following volumes of acid. Neglect activity. (15 points) a) 0.00 mL of NaOH added: 2.59 b) 50.00 mL of NaOH added: 8.49 c) 75.00 mL of NaOH...
4. You are titrating 100 ml of a 0.25 M solution of acetic acid (pk. =...
4. You are titrating 100 ml of a 0.25 M solution of acetic acid (pk. = 4.75) with a 1.25 M solution of NaOH. What is the pH of the solution after you have added 10.0 ml of the NaOH?
A 100.0m aliquot of 0.100 M diprotic acid H₂A (pk, = 4.00; ph2 = 8.00) was titrated with 1.00M NaOH
A 100.0m aliquot of 0.100 M diprotic acid H₂A (pk, = 4.00; ph2 = 8.00) was titrated with 1.00M NaOH. Find the pH at the following volumes of base added, Vb: 0mL, 2mL, 8mL, 10mL, 12 mL, 18mL, 20mL, 22mL,
9. Acetic acid (CH3CO2H) has a pk of 4.76 at 25°C. A 5.00 mL aliquot of a 0.0185 M solution of acetic acid is titrated with a 0.1000 M standardized solution of NaOH. (a) What is the pH of the acetic acid solution before any of the standardized solution is added? (b) What volume of the standardized solution is necessary to reach the equiv- alence point? (c) What is the pH of the solution after 1.48 mL of the standardized...
9. Acetic acid (CH,CO,H) asap. of 4 M solution of acetic acid is titrated with NAOH C A5.00 mL aliquot of a 0.0185 0.1000 M standardized solution of (a) What is the pH of the Netheld solution before any of the standardized solution is added? (b) What volume of the standardized solution is necessary to reach the equiv- alence point? (c) What is the pH of the solution after 1.48 mL of the standardized solution is added?
Weak-Acid Strong-Base Titrations. These next questions relate to a 25 mL aliquot of 0.35 M acetic acid (Ka = 1.77 x 10) that is titrated with 0.20 M potassium hydroxide (KOH). (f) What is the pH of the acetic acid solution before the titration begins? (g) What is the pH after 14 mL of 0.20 M KOH has been added to the solution? Use the Henderson-Hasselbalch equation. (h) What is the pH at the equivalence point?
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, PK: - 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution 6. After the addition of 20.00 mL of NaOH solution C. After the addition of 25.00 mL of NaOH solution d. At what volume of added NaOH will pH -pK
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, pK, = 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution. b. After the addition of 20.00 mL of NaOH solution c. After the addition of 25.00 mL of NaOH solution. d. At what volume of added NaOH will pH =pK,
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pK = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume:
Question 2 15 P Weak Acid Titration Calculations. A 25.0 mL aliquot of 0.50 M propanoic acid (CH3CH2O2H) is placed in a 250 mL Erlenmeyer flask and titrated with a standardized solution of 0.25 M NaOH. The pKof propanoic acid is 4.88. Calculate the pH of the solution after the addition of the following volumes of acid. Neglect activity. (15 points) a) 0.00 mL of NaOH added: 2.59 b) 50.00 mL of NaOH added: 8.49 c) 75.00 mL of NaOH...
4. You are titrating 100 ml of a 0.25 M solution of acetic acid (pk. = 4.75) with a 1.25 M solution of NaOH. What is the pH of the solution after you have added 10.0 ml of the NaOH?
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