Homework Answers
18.
Correct option: a
HNO2 is an is a weak acid. Therefore, it partially dissociates in water. On addition of a strong base, HNO2 will convert to KNO2. KNO2 is a salt and it completely dissociates in water. Hence, the nitrite ion concentration will increase if a strong base is added.
Option b is incorrect as pH = pKa when [KNO2] = [HNO2]. But here, [HNO2] = 2 x [KNO2].
Option c is incorrect as pKa of an acid is a constant.
Already the solution has more concentration of acid. Hence, addition of a strong acid will diminish the buffer capacity by converting KNO2 to HNO2. Hence, option d is incorrect.
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18. Consider a buffer solution containing HNO, and KNO, where the concentration of HNO2 is double...
19. If 25 mL of .875 M HNO; is combined with 100.0 mL of 0.167 M...
19. If 25 mL of .875 M HNO; is combined with 100.0 mL of 0.167 M NaOH what is the final pH? (Assume that the volumes are additive.) (d) 1.38 b) 2.28 c) 11.72 d) 12.62 strong
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH...
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO, (s) is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK. = 4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer?...
This is all info given A buffer solution that is 0.448 M in HNO2 and 0.448...
This is all info given
A buffer solution that is 0.448 M in HNO2 and 0.448 M in KNO, has a pH of 3.35. The addition of 0.01 mol of OH to 1.0 L of this buffer would cause the pH t increase slightly The capacity of this buffer for added OH could be increased by the addition increase by 2 units decrease slightly decrease by 2 units not change A buffer solution that is 0.448 M in HNO2 and...
(YES/NO) (ADDED ACID/ADDED BASE) A buffer solution that is 0.322 M in HNO2 and 0.322 M...
(YES/NO) (ADDED ACID/ADDED BASE)
A buffer solution that is 0.322 M in HNO2 and 0.322 M in NaNO, has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added OH"? (Select all that apply.) OHNO2 pure water O both HNO, and NaNO2 NaNO2 Onone of the above Use the References to access important values if needed for this question. The PK, value for HNO2 is 3.35. Would a buffer prepared from...
of Jestion Consider a buffer of HNO/NO, 1. To create the buffer, solid NaNO (MM =...
of Jestion Consider a buffer of HNO/NO, 1. To create the buffer, solid NaNO (MM = 68.995 g/mol) was added to a 500.0-ml 1.25 M HNO2 solution. The pka of HNO2 is 3.37. i. What mass needs to be added in order to have a buffer with pH 3.20. ii. If 10.0-mL of 2.50 M NaOH is added to the buffer prepared in i., what is the pH of the solution.
Question two A buffer solution is able to maintain a constant pH when small amounts of...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
please help me with these questions! At a concentration of 1 M, the weak acid HNO,...
please help me with these questions!
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
3. You are asked to make a buffer solution with a pH of 3.40 by using...
3. You are asked to make a buffer solution with a pH of 3.40 by using 0.100 M HNO, and 0.100 M NaOH (aq). a. Explain why the addition of 0.100 M HNO2 to 0.100 M NaOH(aq) can result in the formation of a buffer solution. Include the net ionic equations for the reaction that occurs when you combine HNO2 (aq) and NaOH(aq). Determine the volume, in ml, of 0.100 NaOH(aq) the student should add to 100 mL of 0.100...
help with these chemistry questions 1. Explain what happens to the concentration of H,O' ions in...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the so...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
19. If 25 mL of .875 M HNO; is combined with 100.0 mL of 0.167 M NaOH what is the final pH? (Assume that the volumes are additive.) (d) 1.38 b) 2.28 c) 11.72 d) 12.62 strong
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO, (s) is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK. = 4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer?...
This is all info given
A buffer solution that is 0.448 M in HNO2 and 0.448 M in KNO, has a pH of 3.35. The addition of 0.01 mol of OH to 1.0 L of this buffer would cause the pH t increase slightly The capacity of this buffer for added OH could be increased by the addition increase by 2 units decrease slightly decrease by 2 units not change A buffer solution that is 0.448 M in HNO2 and...
(YES/NO) (ADDED ACID/ADDED BASE)
A buffer solution that is 0.322 M in HNO2 and 0.322 M in NaNO, has a pH of 3.35. Addition of which of the following would increase the capacity of the buffer for added OH"? (Select all that apply.) OHNO2 pure water O both HNO, and NaNO2 NaNO2 Onone of the above Use the References to access important values if needed for this question. The PK, value for HNO2 is 3.35. Would a buffer prepared from...
of Jestion Consider a buffer of HNO/NO, 1. To create the buffer, solid NaNO (MM = 68.995 g/mol) was added to a 500.0-ml 1.25 M HNO2 solution. The pka of HNO2 is 3.37. i. What mass needs to be added in order to have a buffer with pH 3.20. ii. If 10.0-mL of 2.50 M NaOH is added to the buffer prepared in i., what is the pH of the solution.
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
please help me with these questions!
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
3. You are asked to make a buffer solution with a pH of 3.40 by using 0.100 M HNO, and 0.100 M NaOH (aq). a. Explain why the addition of 0.100 M HNO2 to 0.100 M NaOH(aq) can result in the formation of a buffer solution. Include the net ionic equations for the reaction that occurs when you combine HNO2 (aq) and NaOH(aq). Determine the volume, in ml, of 0.100 NaOH(aq) the student should add to 100 mL of 0.100...
help with these chemistry questions
1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
i want answer to all questions please
Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
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