Question 1 a. How many mol of solid LiA would have to be added to 1.0...
Question 1
a. How many mol of solid LiA would have to be added to 1.0 L of a 4.974 M HA solution in order to obtain a buffer of 2.68? (The Ka for HA is 3.51⋅10^-7).
b. Calculate the pH at the equivalence point for the titration of 2.480 M B: (a weak base with pKb = 6.28) with 2.480 M HCl.
c. What volume of water must be added to a 10.14 mL solution of a pH = 1.43 solution of HClO4 to raise the pH to 3.15?
Homework Answers
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Question 1
a. How many mol of solid LiA would have to be added to 1.0...
How many mol of solid LiA would have to be added to 1.0 Lof a 4.064 M HA solution in order to obtain a buffer of 3....
How many mol of solid LiA would have to be added to 1.0 Lof a 4.064 M HA solution in order to obtain a buffer of 3.08? (The Ka for HA is 4.44 . 10-6). F Preview mol LiA INE
A) How many milliliters of 0.15 M HCl would have to be added to 1.0 L...
A) How many milliliters of 0.15 M HCl would have to be added to 1.0 L of a buffer containing 0.25 M NH3 and 0.45 M NH4 to make the pH decrease by 0.05 pH unit? The Ka value = 5.6 x 10^-10. B) How many milliliters of the same HCl solution would, if added to 0.204 L of pure water, make the pH decrease by 0.05 pH unit?
Consider the titration of a 23.3 −mL sample of 0.125 M RbOH with 0.110 M HCl....
Consider the titration of a 23.3 −mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each quantity: A) the volume of added acid required to reach the equivalence point B) the pH at the equivalence point C) the pH after adding 6.0 mL of acid beyond the equivalence point D) Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of the original buffer,...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing...
How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing 12.212g of benzoic acid (F.W. 122.12g ; Ka = 6.28 x 10-5) to get a pH of 4.8?
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of...
The half‑equivalence point of a titration occurs half way to the
equivalence point, where half of the analyze has reacted to form
its conjugate, and the other half still remains unreacted.
If 0.4400.440 moles of a monoprotic weak acid
(?a=7.2×10−5)(Ka=7.2×10−5) is titrated with NaOH,NaOH, what is the
pH of the solution at the half‑equivalence point?
pH=pH=
2)
A volume of 500.0 mL500.0 mL of 0.120 M0.120 M NaOHNaOH is added
to 565 mL565 mL of 0.250 M0.250 M weak acid...
1. For each of the following, predict whether an aqueous solution of the salt would be...
1. For each of the following, predict whether an aqueous solution of the salt would be acidic, basic or neutral. Explain. a. Nacis b. NaF c. NHIS d. KHCO3 e. (CH3)2NH2NO31 2. What is the pH of a solution that is 0.060 M in potassium propionate (CH3CH2COOK) and 0.085M in propionic acid (CH3CH2COOH)? The Ka for propionic acid is 1.3x10-5.5 3. Suppose you need to prepare a buffer for a pH of 10.6. An acid-base pair (HA/A') to use has...
1. A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of...
1. A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of sodium butanoate in water sufficient to yield 1.00 L of solution. The addition of 0.0O5 mol of HCI to this buffer solution causes the plH to drop slightly. The pH does not decrease drastically because the HCl reacts with the present in the buffer solution. The Ka of butanoic acid is 1.36x 10-3 A) H20 в) Нзо+ butanoate ion D butanoic acid AlE) This...
CHomework Chapter 17 Plotting a Titration Curve for a Carbonate-Bicarbonate System 9 of 24> Carbo...
CHomework Chapter 17 Plotting a Titration Curve for a Carbonate-Bicarbonate System 9 of 24> Carbonic acid (H2COa) is a weak diprotic acid with K4.43 x 10-7 and K 4.73 x 10-11 change, and equilibrium values for each species and plugging these into the equlibrium constant expression. The expression HCO as shown in the equation using the equation Salts of the bicarbonate ion, such as sodium During the titration before the equivalence point, provided that the concentration of acid is significantly...
How many grams of sodium acetate, NaC2H3O2, would have to be added to 1.0 L of...
How many grams of sodium acetate, NaC2H3O2, would have to be added to 1.0 L of 0.90 M acetic acid (pKa = 4.74) to make the solution a buffer for pH 4.00?
How many mol of solid LiA would have to be added to 1.0 Lof a 4.064 M HA solution in order to obtain a buffer of 3.08? (The Ka for HA is 4.44 . 10-6). F Preview mol LiA INE
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
The half‑equivalence point of a titration occurs half way to the
equivalence point, where half of the analyze has reacted to form
its conjugate, and the other half still remains unreacted.
If 0.4400.440 moles of a monoprotic weak acid
(?a=7.2×10−5)(Ka=7.2×10−5) is titrated with NaOH,NaOH, what is the
pH of the solution at the half‑equivalence point?
pH=pH=
2)
A volume of 500.0 mL500.0 mL of 0.120 M0.120 M NaOHNaOH is added
to 565 mL565 mL of 0.250 M0.250 M weak acid...
1. For each of the following, predict whether an aqueous solution of the salt would be acidic, basic or neutral. Explain. a. Nacis b. NaF c. NHIS d. KHCO3 e. (CH3)2NH2NO31 2. What is the pH of a solution that is 0.060 M in potassium propionate (CH3CH2COOK) and 0.085M in propionic acid (CH3CH2COOH)? The Ka for propionic acid is 1.3x10-5.5 3. Suppose you need to prepare a buffer for a pH of 10.6. An acid-base pair (HA/A') to use has...
1. A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of sodium butanoate in water sufficient to yield 1.00 L of solution. The addition of 0.0O5 mol of HCI to this buffer solution causes the plH to drop slightly. The pH does not decrease drastically because the HCl reacts with the present in the buffer solution. The Ka of butanoic acid is 1.36x 10-3 A) H20 в) Нзо+ butanoate ion D butanoic acid AlE) This...
CHomework Chapter 17 Plotting a Titration Curve for a Carbonate-Bicarbonate System 9 of 24> Carbonic acid (H2COa) is a weak diprotic acid with K4.43 x 10-7 and K 4.73 x 10-11 change, and equilibrium values for each species and plugging these into the equlibrium constant expression. The expression HCO as shown in the equation using the equation Salts of the bicarbonate ion, such as sodium During the titration before the equivalence point, provided that the concentration of acid is significantly...
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