Homework Answers
Question 4.29
[H+]NaOH = Kw/[OH-] = 10-14/10-3 = 10-11 M
Therefore, pH = -Log[H+] = -Log(10-11) = 11
Here, the presence of Na2CO3 further increases the basicity slightly by 0.1 units, then the pH the concentration of the resulting solution is 11.1
Question 4.30
pH = 7 - 1/2 (pKa - pKb) = 7 - 1/2 (4.74 - 4.74) = 7
Add Answer to:
I
need help with constructing the Log C vs pH diagram. Also I need
the solution...
6. (a) Construct a log Il-pH diagram to determine the pH of a solution containing 10-3...
6. (a) Construct a log Il-pH diagram to determine the pH of a solution containing 10-3 M Na2CO3 (PKAI = 6.37. KA2 = 10.33) and 10 Macetic acid (p =4.74) (b) What's the equilibrium pH if 10" M NaOH is added to the system? 7. Assume that a wastewater contains phenol (CH3OH) as a major constituent. Write the redox half reactions for the conversion of phenol to carbon dioxide (CO2) and the reaction of Cr 0-to Cr(OH). Combine the two...
Refer back to the standard curve that you built previously (absorbance vs. concentration) The pH of...
Refer back to the standard curve that you built previously (absorbance vs. concentration) The pH of a solution describes the concentration of H+ in a solution, where pH = -log[H+]. Note that this is a log10, not the natural log, so the inverse is [H+] = 10-pH. Acetic acid dissociates in water according to the following reaction: -+CH3COOH (aq) ⇄ CH3COO (aq) + H (aq) The pH of a 1.0 M solution of acetic acid is 2.37. What is the...
Need help with number three please salt Find the pH of a buffer solution containing of...
Need help with number three please
salt Find the pH of a buffer solution containing of 1.5M sodium acetate and 0.9M acetic acid. The K. of acetic acid is 1.8 x 105. acid pH=pka + log I salt) pH =-103(18410 9) +10g -(-4.74)+(. 2a) =14.96 2. Find the pH of 100.0 mL of the buffer from exercise 1 after the addition of 0.030 mol of gascous hydrochloric acid. Assume no volume change. Find the pH of 200.0 mL buffer from...
With this information how would I calculate the pH of .01 M Ammonia solution and the...
With this information how would I calculate the pH of
.01 M Ammonia solution and the pH of .01 M Ammonia buffer
solution
I need
Ph of acetic acid! sorry for the wrong wording!
A. Preparation of Acetic Acid-Acetate Buffer Solution An acetate buffer contains the acid-base pair, acetic acid and the acetate fon (typically added as sodium acetate). For acetic acid, pk, = -log (1.8 10 = 4.74. Consider the con ditions that will yield 100 ml of an...
The pH of a solution describes the concentration of H+ in a solution, where pH =...
The pH of a solution describes the concentration of H+ in a solution, where pH = -log[H+]. Note that this is a log10, not the natural log, so the inverse is [H+] = 10-pH. Acetic acid dissociates in water according to the following reaction: -+CH3COOH (aq) ⇄ CH3COO (aq) + H (aq) The pH of a 1.0 M solution of acetic acid is 2.37. What is the value of the equilibrium constant for the dissociation of acetic acid?
Graph (draw the diagram) pH Vs Log Q, where Q is the relation of concentrations of the...
Graph (draw the diagram) pH Vs Log Q, where Q is the relation of concentrations of the base / conjugate acid species, where the following results were obtained in the evaluation of o-fluorophenol in 30% alcohol at 25 ° C. Said titration is carried out with X ml of 0.01N NaOH to 50 ml of a 0.01N solution of o-fluorophenol and the following pH values were obtained: ml of NaOH 0,01N 10 15 20 30 40 pH 8,73 9,01 9,20 9,56...
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic...
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic acid, HCOOH, K=1.78x10-4 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the Ka for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
Properties of Buffers Lab. I need help with problems 7 & 8. They’re pretty similar, but...
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic acid, HCOOH. K=1.78x104 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the K, for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
What would the concentration of acetic acid need to be in a solution containing 0.25 M...
What would the concentration of acetic acid need to be in a solution containing 0.25 M sodium acetate to have a pH of 4.0? Given that Ka for acetic acid is 1.8 × 10-5.
6. (a) Construct a log Il-pH diagram to determine the pH of a solution containing 10-3 M Na2CO3 (PKAI = 6.37. KA2 = 10.33) and 10 Macetic acid (p =4.74) (b) What's the equilibrium pH if 10" M NaOH is added to the system? 7. Assume that a wastewater contains phenol (CH3OH) as a major constituent. Write the redox half reactions for the conversion of phenol to carbon dioxide (CO2) and the reaction of Cr 0-to Cr(OH). Combine the two...
Need help with number three please
salt Find the pH of a buffer solution containing of 1.5M sodium acetate and 0.9M acetic acid. The K. of acetic acid is 1.8 x 105. acid pH=pka + log I salt) pH =-103(18410 9) +10g -(-4.74)+(. 2a) =14.96 2. Find the pH of 100.0 mL of the buffer from exercise 1 after the addition of 0.030 mol of gascous hydrochloric acid. Assume no volume change. Find the pH of 200.0 mL buffer from...
With this information how would I calculate the pH of
.01 M Ammonia solution and the pH of .01 M Ammonia buffer
solution
I need
Ph of acetic acid! sorry for the wrong wording!
A. Preparation of Acetic Acid-Acetate Buffer Solution An acetate buffer contains the acid-base pair, acetic acid and the acetate fon (typically added as sodium acetate). For acetic acid, pk, = -log (1.8 10 = 4.74. Consider the con ditions that will yield 100 ml of an...
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic acid, HCOOH, K=1.78x10-4 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the Ka for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic acid, HCOOH. K=1.78x104 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the K, for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
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