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Determination of the Dissociation Constant ka, of a Weak Acid Part A Phosphoric acid is a...
24.5 24.9 5.49 6.20 34 36 2.1 12.2 12.26 Determine K, for the unknown acid 2....
24.5 24.9 5.49 6.20 34 36 2.1 12.2 12.26 Determine K, for the unknown acid 2. What is the pH of the solution that results when 25.0 mL. of 0.125 M NaOH is added to 25.0 mL of0.250 M HCl? What is the pH of a solution that is 0.40 M in sodium acetate and 0.60 M on acetic acid? (K, for acetic acid is 1.85 x 10-5.) 3. 17 CHEM 1412 Experiment 6 | Determination of the Dissociation Constant...
Phosphoric acid is triprotic with the step-wise dissociation shown below. A 1.34 M phosphoric acid solution is prep...
Phosphoric acid is triprotic with the step-wise dissociation shown below. A 1.34 M phosphoric acid solution is prepared. Calculate the equilibrium concentrations of the species indicated. Report all answers in scientific notation using 2 sig figs. Rather than use the quadratic equation, you can make assumptions like we do in class (ie if K<<1, then 0.1-x -0.1) H3PO HO H.PO H3O Kai = 7.5c10-3 Preview Preview Preview H.PO H20 HPo? + H50+ K - 6.2:10 -* Preview Preview HPO H2O...
(1) The Ka values for citric acid (2) and phosphoric acid (3) The exact concentration of the citr...
(1) The Ka values for citric acid (2) and phosphoric acid
(3) The exact concentration of the citric acid and (4)
phosphoric acid
Citric Acid Titration 12 10 2 40 60 20 80 volume NaOH (mL) Phosphoric acid Titration 12 r 10 ds 4 25 50 75 vol NaOH (mL)
Citric Acid Titration 12 10 2 40 60 20 80 volume NaOH (mL)
Phosphoric acid Titration 12 r 10 ds 4 25 50 75 vol NaOH (mL)
1. Phosphoric acid, H3PO4 is a triprotic acid with pKsı = 2.14 and pKa = 7.20 and pkas 12.38. Dra...
1. Phosphoric acid, H3PO4 is a triprotic acid with pKsı = 2.14 and pKa = 7.20 and pkas 12.38. Draw the titration curve predicted for 0.1 M phosphoric acid titrated by 0.1 M NaOH. (Assume the volume of acid is 20. mL) 2. The pKb of the acetate ion is 9.25. a. Using this information, calculate the pKa of acetic acid. b. Using the Henderson-Hasselbalch equation, calculate the ratio of the concentration of acetate to acetic acid required to produce...
14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00...
14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00 ml sample with a concentration of 0.250 M is titrated with 0.150 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.250 M sample of HA? c. What is the percent ionization of the 0.250 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 12.00 ml 0.150M...
A 25.0 mL sample of 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ✕ 10-5) is...
A 25.0 mL sample of 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ✕ 10-5) is titrated with 0.100 M KOH solution. Calculate the pH after the addition of the following amounts of KOH. 0.0 mL 4.0 mL 8.0 mL 12.5 mL 20.0 mL 24.0 mL 24.5 mL 24.9 mL 25.0 mL 25.1 mL 26.0 mL 28.0 mL 30.0 mL
A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with...
A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with a concentration of 0.1200 M is titrated with 0.1500 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.1200 M sample of HA? c. What is the percent ionization of the 0.1200 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 8.00 ml NaOH have been added?
Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M...
Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39, what is the K_a of the acid? K_a = Hydrofluoric Acid, A weak Acid with K_a = 7.1 times 10^-4 A. For a 0.50 M solution of HF, calculate the equilibrium concentrations of HF, H^+ and F^-. [HF] = [H^+] = [F^-] = % Dissociation =, pH = B. Now consider a 0.050 M solution of HF....
284 Report Sheet . Determination of the Dissociation Constant of a Weak Acid 2.96 2.99 4.37...
284 Report Sheet . Determination of the Dissociation Constant of a Weak Acid 2.96 2.99 4.37 4.55 C. Determination of pKof Unknown Acid First determination Second determination ml NaOH pH ml NaOH pH 0.00 mL 0.00 mL 1.00 mL 2.00 mL 2.00 mL 4.00 mL 3.64 3.00 mL 6.00 ml 3.97 4.00 mL 7.00 ml 4.17 5.00 ml 8.00 mL 6.00 mL 9.00 ml. 7.00 mL 9.50 mL 4.61 8.00 ml 10.00 ml 4.71 9.00 mL 10.50 ml 4.85 10.00...
• Determination of the Dissociation Constant of a Weak Acid Report Sheet The pH at one-half the equivalence point...
• Determination of the Dissociation Constant of a Weak Acid Report Sheet The pH at one-half the equivalence point in an acid-base titration was found to be 5.67. What is the value of K, for this unknown acid? 8. If 30.15 mL of 0.0995 M NaOH is required to neutralize 0.279 g of an unknown acid, HA, what is the molar mass of the unknown acid? the Assuming that K is 1.85x10 for acetic acid, calculate the pH at one-half...
24.5 24.9 5.49 6.20 34 36 2.1 12.2 12.26 Determine K, for the unknown acid 2. What is the pH of the solution that results when 25.0 mL. of 0.125 M NaOH is added to 25.0 mL of0.250 M HCl? What is the pH of a solution that is 0.40 M in sodium acetate and 0.60 M on acetic acid? (K, for acetic acid is 1.85 x 10-5.) 3. 17 CHEM 1412 Experiment 6 | Determination of the Dissociation Constant...
Phosphoric acid is triprotic with the step-wise dissociation shown below. A 1.34 M phosphoric acid solution is prepared. Calculate the equilibrium concentrations of the species indicated. Report all answers in scientific notation using 2 sig figs. Rather than use the quadratic equation, you can make assumptions like we do in class (ie if K<<1, then 0.1-x -0.1) H3PO HO H.PO H3O Kai = 7.5c10-3 Preview Preview Preview H.PO H20 HPo? + H50+ K - 6.2:10 -* Preview Preview HPO H2O...
(1) The Ka values for citric acid (2) and phosphoric acid
(3) The exact concentration of the citric acid and (4)
phosphoric acid
Citric Acid Titration 12 10 2 40 60 20 80 volume NaOH (mL) Phosphoric acid Titration 12 r 10 ds 4 25 50 75 vol NaOH (mL)
Citric Acid Titration 12 10 2 40 60 20 80 volume NaOH (mL)
Phosphoric acid Titration 12 r 10 ds 4 25 50 75 vol NaOH (mL)
1. Phosphoric acid, H3PO4 is a triprotic acid with pKsı = 2.14 and pKa = 7.20 and pkas 12.38. Draw the titration curve predicted for 0.1 M phosphoric acid titrated by 0.1 M NaOH. (Assume the volume of acid is 20. mL) 2. The pKb of the acetate ion is 9.25. a. Using this information, calculate the pKa of acetic acid. b. Using the Henderson-Hasselbalch equation, calculate the ratio of the concentration of acetate to acetic acid required to produce...
14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00 ml sample with a concentration of 0.250 M is titrated with 0.150 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.250 M sample of HA? c. What is the percent ionization of the 0.250 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 12.00 ml 0.150M...
Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39, what is the K_a of the acid? K_a = Hydrofluoric Acid, A weak Acid with K_a = 7.1 times 10^-4 A. For a 0.50 M solution of HF, calculate the equilibrium concentrations of HF, H^+ and F^-. [HF] = [H^+] = [F^-] = % Dissociation =, pH = B. Now consider a 0.050 M solution of HF....
284 Report Sheet . Determination of the Dissociation Constant of a Weak Acid 2.96 2.99 4.37 4.55 C. Determination of pKof Unknown Acid First determination Second determination ml NaOH pH ml NaOH pH 0.00 mL 0.00 mL 1.00 mL 2.00 mL 2.00 mL 4.00 mL 3.64 3.00 mL 6.00 ml 3.97 4.00 mL 7.00 ml 4.17 5.00 ml 8.00 mL 6.00 mL 9.00 ml. 7.00 mL 9.50 mL 4.61 8.00 ml 10.00 ml 4.71 9.00 mL 10.50 ml 4.85 10.00...
• Determination of the Dissociation Constant of a Weak Acid Report Sheet The pH at one-half the equivalence point in an acid-base titration was found to be 5.67. What is the value of K, for this unknown acid? 8. If 30.15 mL of 0.0995 M NaOH is required to neutralize 0.279 g of an unknown acid, HA, what is the molar mass of the unknown acid? the Assuming that K is 1.85x10 for acetic acid, calculate the pH at one-half...
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