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4. (3) The first disinfectant used by Joseph Lister was called carbolic acid. This substance now...
Phenol (C6H3OH), commonly called carbolic acid, is a weak organic acid. C6H5OH(aq) + H2O(l) # C6H50- (aq) + H30+ (aq) K...
Phenol (C6H3OH), commonly called carbolic acid, is a weak organic acid. C6H5OH(aq) + H2O(l) # C6H50- (aq) + H30+ (aq) Ka = 1.3 x 10-10 If you dissolve 0.300 g of the acid in enough water to make 856 mL of solution, what is the equilibrium hydronium ion concentration? [H30+1=C M What is the pH of the solution? pH = 0
ch 14 reg hw: 5) When 0.0034 moles of a weak acid are dissolved in enough...
ch 14 reg hw: 5) When 0.0034 moles of a weak acid are dissolved in enough water to make 0.500 L, the pH of the resulting solution is 5.86. Calculate Ka. 23) Phenol (C6H5OH, also called carbolic acid) has a pKa of 9.89. It is used to preserve body tissues and is quite toxic. Calculate the percent ionized in 0.0789 M phenol--a dilute solution.
Can anyone please help with how to calculate degree of ionization for the first 3 solutions...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
U Crone (NH4CI). What is the pH of the solution? 3. (4 pts) Calculate the pH...
U Crone (NH4CI). What is the pH of the solution? 3. (4 pts) Calculate the pH of a 0.250 M solution of potassium phenolate, KC6H50. Ka foi phenol (C6H5OH) is 1.0 x 10-10. 4. (8 pts) How do the concentration/volumes of the buffer affect the buffer capacity! E.g. 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid...
How do you find the degree of ionization of the solutions when accounting for the dillution...
How do you find the degree of ionization of the solutions when
accounting for the dillution effect of adding 10 mL of water? Also
for the second page, how do you calculate pH with a buffer using
the Henderson-Hasselbalch equation?
Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for the dilution effect of adding 10.0 mL of water, and use MV1 = M2V2 Degree of lonization of solution 2...
please help. 1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 %...
please help.
1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 % ionized. What is the pH of the solution? a. b. Calculate the K, of the acid. 2. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? 3. (2 points) Determine the percent ionization of a 0.0028 M HA solution. (K, of HA 1.4 x 10") 4. (4 points) Lysine is...
Calculate and fill in the following information and indicate whether the solution is acidic, basie, of...
Calculate and fill in the following information and indicate whether the solution is acidic, basie, of neutral (2 pts, each) You must show work in order to receive full credit. TH:0" рон scidi, boste or neutral TOH 0.34 6.77 x 10 [You must show work in order to receive full credit for mathematical problems) (8 pts.) Phenol (HOCH) is a weak acid used as a general disinfectant and in the manufacture of plastics Calculate the concentration of all species present...
-/0.1 points 33 0/4 Submissions Used (a) Calculate the percent ionization of 0.00720 M carbonic acid...
-/0.1 points 33 0/4 Submissions Used (a) Calculate the percent ionization of 0.00720 M carbonic acid (Ka = 4.3e-07). % ionization = % (b) Calculate the percent ionization of 0.00720 M carbonic acid in a solution containing 0.0470 M sodium hydrogen carbonate. % % ionization = Submit Answer + -/0.1 points 34. 0/4 Submissions Used A buffer solution contains 0.76 mol of propionic acid (HC3H502) and 0.30 mol of sodium propionate (NaC3H502) in 7.30 L The Ka of propionic acid...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the pH of the solution? Calculate the Ka of the acid. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? (2 points) Determine the percent ionization of a 0.0028 M HA solution. (Ka of HA = 1.4 x 10-9) (4 points) Lysine is triprotic amino acid (separately loses three H’s in...
instructions 1 pts Question 4 Concentrated sulfuric acid is 18.1 M. The first hydrogen is a...
instructions 1 pts Question 4 Concentrated sulfuric acid is 18.1 M. The first hydrogen is a strong acid and is completely ionized, the second hydrogen is a weak acid with a K 2 = 0.012 If only the first hydrogen ionized the pH would be pH = -log(18.1) = -1.258. When we include the partial ionization of the second hydrogen, what is the pH of this solution? • Previous MacBook |
Phenol (C6H3OH), commonly called carbolic acid, is a weak organic acid. C6H5OH(aq) + H2O(l) # C6H50- (aq) + H30+ (aq) Ka = 1.3 x 10-10 If you dissolve 0.300 g of the acid in enough water to make 856 mL of solution, what is the equilibrium hydronium ion concentration? [H30+1=C M What is the pH of the solution? pH = 0
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
U Crone (NH4CI). What is the pH of the solution? 3. (4 pts) Calculate the pH of a 0.250 M solution of potassium phenolate, KC6H50. Ka foi phenol (C6H5OH) is 1.0 x 10-10. 4. (8 pts) How do the concentration/volumes of the buffer affect the buffer capacity! E.g. 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid...
How do you find the degree of ionization of the solutions when
accounting for the dillution effect of adding 10 mL of water? Also
for the second page, how do you calculate pH with a buffer using
the Henderson-Hasselbalch equation?
Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for the dilution effect of adding 10.0 mL of water, and use MV1 = M2V2 Degree of lonization of solution 2...
please help.
1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 % ionized. What is the pH of the solution? a. b. Calculate the K, of the acid. 2. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? 3. (2 points) Determine the percent ionization of a 0.0028 M HA solution. (K, of HA 1.4 x 10") 4. (4 points) Lysine is...
Calculate and fill in the following information and indicate whether the solution is acidic, basie, of neutral (2 pts, each) You must show work in order to receive full credit. TH:0" рон scidi, boste or neutral TOH 0.34 6.77 x 10 [You must show work in order to receive full credit for mathematical problems) (8 pts.) Phenol (HOCH) is a weak acid used as a general disinfectant and in the manufacture of plastics Calculate the concentration of all species present...
-/0.1 points 33 0/4 Submissions Used (a) Calculate the percent ionization of 0.00720 M carbonic acid (Ka = 4.3e-07). % ionization = % (b) Calculate the percent ionization of 0.00720 M carbonic acid in a solution containing 0.0470 M sodium hydrogen carbonate. % % ionization = Submit Answer + -/0.1 points 34. 0/4 Submissions Used A buffer solution contains 0.76 mol of propionic acid (HC3H502) and 0.30 mol of sodium propionate (NaC3H502) in 7.30 L The Ka of propionic acid...
instructions 1 pts Question 4 Concentrated sulfuric acid is 18.1 M. The first hydrogen is a strong acid and is completely ionized, the second hydrogen is a weak acid with a K 2 = 0.012 If only the first hydrogen ionized the pH would be pH = -log(18.1) = -1.258. When we include the partial ionization of the second hydrogen, what is the pH of this solution? • Previous MacBook |
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