For a particular formic acid buffer (pKa of HCOOH is 3.74), the ratio of CHOO- to...
For a particular formic acid buffer (pKa of HCOOH is 3.74), the ratio of CHOO- to CHOOHr at pH 4.25 was 3.236. If you have 100 mL of the buffer and the total ion concentration (CHOOH and CHOO-) is 0.20 M, how many moles of NaCHOO do you need to add to raise the pH to 4.71?
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For a particular formic acid buffer (pKa of HCOOH is 3.74), the
ratio of CHOO- to...
A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The...
A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The volume of the buffer is 100 mL ; with [HCOOH] = 0.110 mol L-1 and [HCOO- ] = 0.101 mol L-1 . The pKa of HCOOH = 3.74. What is the pH of this buffer? Write down the balanced chemical equation that describes the reaction of this buffer when an HCl solution is added. c) What is the resultant pH of this solution after...
23. A 1.0 L buffer solution is prepared with 0.25 M formic acid (HCOOH) and 0.50...
23. A 1.0 L buffer solution is prepared with 0.25 M formic acid (HCOOH) and 0.50 M sodium formate (HCOONa). HCOOH(aq) + H2O(aq) – HCOO (aq) + H30+(aq) pKa = 3.74 What is the pH of this buffer solution? (A) 3.74 (B) 4.04 (C) 4.50 (D) 4.20
A formic acid buffer solution contains 0.22 M HCOOH and 0.24 M HCOO. The pKa of formic acid is 3.75. What is the pH...
A formic acid buffer solution contains 0.22 M HCOOH and 0.24 M HCOO. The pKa of formic acid is 3.75. What is the pH of the buffer? Answer:
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of...
Part A You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the end point? You are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . If you add 20.00 of to the beaker before...
For the solution of 0.020 moles of formic acid (HCOOH) and 0.010 moles of sodium formate (pka = 3.7545 at 25 C) obtain:...
For the solution of 0.020 moles of formic acid (HCOOH) and 0.010 moles of sodium formate (pka = 3.7545 at 25 C) obtain: a) the reactions involved in the process b) the derivation of the Henderson-Hasselbalch expression from equilibrium for the dissolution of the formic acid. c) the pH of the system and the pOH d) the concentration of H3O+ e) the concentration of OH- of the system
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for...
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4) with a...
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4)
with a pH = 4.00, what ratio of formic acid to sodium formate is
required? (Notice that I am asking for the ratio of acid to base,
not base to acid!)
a) 1.25
b) 0.56
c) 0.82
d) 1.87
QUESTION 4 If you find that you need an acid to base ratio of
4.23 and you are using 50.00mL of a 1.00M acid solution, what
volume...
3. Formic acid, HCOOH, is a weak acid with a pK, of 3.74. Draw up a...
3. Formic acid, HCOOH, is a weak acid with a pK, of 3.74. Draw up a reaction table for the reaction of 0.300 M formic acid with water, and calculate the pH of this solution. 4. Consider the following gas-phase equilibrium reaction: N(g) O,(g)2NOg K, 4.10x 10 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000 C, what is the concentration of NO when equilibrium is reached? 5. Consider the equilibrium Predict and...
(3) 36. What is the ratio (HCOOHCOOH) at pH 2.75? The pK, of formic acid is...
(3) 36. What is the ratio (HCOOHCOOH) at pH 2.75? The pK, of formic acid is 3.75. 37. 1.42 L buffer solution consists of 0.181M butanoic acid and 0.310 M sodium butanoate. Calculate the pH of the solution following the addition of 0.069 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52x10-5 (6) 38. You need to prepare 100.0 mL of a pH 4.00...
Use the Henderson-Hasselbalch equation to determine the ratio of acid to base in a formic acid-formate...
Use the Henderson-Hasselbalch equation to determine the ratio of acid to base in a formic acid-formate buffer with a pH of 3.00 Assume that the human blood buffer includes 0.00080 M carbonic acid and 0.0080 M hydrogen carbonate. What is the pH of 7.00 liter of blood under these conditions? How many moles of strong acid must be added to the blood in question 2 to bring the hydrogen carbonate/ carbonic acid ratio to the hazardous level of 5:1 AND...
23. A 1.0 L buffer solution is prepared with 0.25 M formic acid (HCOOH) and 0.50 M sodium formate (HCOONa). HCOOH(aq) + H2O(aq) – HCOO (aq) + H30+(aq) pKa = 3.74 What is the pH of this buffer solution? (A) 3.74 (B) 4.04 (C) 4.50 (D) 4.20
A formic acid buffer solution contains 0.22 M HCOOH and 0.24 M HCOO. The pKa of formic acid is 3.75. What is the pH of the buffer? Answer:
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4)
with a pH = 4.00, what ratio of formic acid to sodium formate is
required? (Notice that I am asking for the ratio of acid to base,
not base to acid!)
a) 1.25
b) 0.56
c) 0.82
d) 1.87
QUESTION 4 If you find that you need an acid to base ratio of
4.23 and you are using 50.00mL of a 1.00M acid solution, what
volume...
3. Formic acid, HCOOH, is a weak acid with a pK, of 3.74. Draw up a reaction table for the reaction of 0.300 M formic acid with water, and calculate the pH of this solution. 4. Consider the following gas-phase equilibrium reaction: N(g) O,(g)2NOg K, 4.10x 10 at 2000°C If 1.0 mol of NO is introduced into a 1.0 L container at 2000 C, what is the concentration of NO when equilibrium is reached? 5. Consider the equilibrium Predict and...
(3) 36. What is the ratio (HCOOHCOOH) at pH 2.75? The pK, of formic acid is 3.75. 37. 1.42 L buffer solution consists of 0.181M butanoic acid and 0.310 M sodium butanoate. Calculate the pH of the solution following the addition of 0.069 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52x10-5 (6) 38. You need to prepare 100.0 mL of a pH 4.00...
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