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Consider the titration of 40.0 mL of 0.500 M NH, with 1.00 M HC a) What...
A 40.0 mL solution of 30.0 M of succinic acid (aq) is titrated with 0.300 M...
A 40.0 mL solution of 30.0 M of succinic acid (aq) is titrated with 0.300 M of KOH. Find the pH of the solution. (pKa=4.2). A) initially B) 1/2 way to the equivalence point C) at the equivalence point D) 1.00 mL past the equivalence post 2) sketch the titration curve that results from above titration. Label A) only a weak base present. B) Buffer. C) Only a weak acid present. D) Strong base in excess. E) pH = pKa
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka...
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka NH,OH) with 0.01 M HCI. Stir. Measure the pH values of the solutions. Plot the titration curve on the same graph with your strong acid/strong base and weak acid/strong base titration curves. Compare with the computer-simulated curve (Figure 14.7). NOTE: Data from the computer calculation give an equivalence point pH of 5.70 at 5.0 drops of added 0.01 M HCI. Observations: Lane 1-purple (pH...
Consider the titration of 40.0 mL of 0.223-M of KX with 0.174-M HCl. The pKa of...
Consider the titration of 40.0
mL of 0.223-M of KX with 0.174-M HCl. The pKa of HX =
6.72. Give all pH values to 0.01 pH units.
Consider the titration of 40.0 mL of 0.223-M of KX with 0.174-M HCI. The pk, of HX = 6.72. Give all pH values to 0.01 pH units. a) What is the pH of the original solution before addition of any acid? pH = b) How many mL of acid are required to reach...
30 Consider the titration of a 40.0 mL of 0.113 M weak acid HA (Ka=2.7 x...
30 Consider the titration of a 40.0 mL of 0.113 M weak acid HA (Ka=2.7 x 10) with 0.100 M LIOH. a What is the pH of the solution before any base has been added? 3 points b What would be the pH of the solution after the addition of 20.0 mL of LIOH? 3 points How many mL of the LiOH would be required to reach the halfway point of the titration? 3 points d What is the pH...
16.36 Consider the titration of 40.0 mL of 0.100 M NaOH with 0.100 M HCI. a)...
16.36 Consider the titration of 40.0 mL of 0.100 M NaOH with 0.100 M HCI. a) b) c) What is the pH after adding 35.0 mL of acid? What is the pH at the equivalence point? What is the pH after adding 45.0 mL of acid?
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂...
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. HC4H7O2 (aq) + OH- --> H2O (l) +C4H7O2-
Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.
Consider the curve shown here for the titration of a weak base with a strong acid and answer each question. a. What is the pH and what is the volume of added acid at the equivalence point? b. At what volume of added acid is the pH calculated by working an equilibrium problem based on the initial concentration and Ks of the weak base? c. At what volume of added acid does pH = 14 - pka ? d. At what volume of added...
1. The potentiometric titration of 25.00 mL of sodium malonate (the conjugate base of malonic acid,...
1. The potentiometric titration of 25.00 mL of sodium malonate (the conjugate base of malonic acid, HOOCCH2COOH which has Kal -1.42x103 and Ka2 2.01x10 with 0.2041 M HCl gave endpoints at 13.01 mL and 26.08 mL. A) Sketch the titration curve (roughly, don't worry about exact pH values, just the general shape of the curve) and label each of the following points with the type of acid/base solution (i.e., is it a strong acid, a weak base, a buffer, etc.):...
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500...
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: 3.96 Make ICE table and use simplified method of successive approximations (no iterations needed). How many mL of NaOH are added to reach the equivalence point? Answer: 8 What is the pH after 3.20...
7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate...
7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate the pH of the following and sketch the titration curve. Kb 1.8 x 10 f. Before the titration starts g. After addition of 2.5 ml of HCl h. After addition of 5.0 ml of HCI i. After addition of 10.0 ml of HC
Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka NH,OH) with 0.01 M HCI. Stir. Measure the pH values of the solutions. Plot the titration curve on the same graph with your strong acid/strong base and weak acid/strong base titration curves. Compare with the computer-simulated curve (Figure 14.7). NOTE: Data from the computer calculation give an equivalence point pH of 5.70 at 5.0 drops of added 0.01 M HCI. Observations: Lane 1-purple (pH...
Consider the titration of 40.0
mL of 0.223-M of KX with 0.174-M HCl. The pKa of HX =
6.72. Give all pH values to 0.01 pH units.
Consider the titration of 40.0 mL of 0.223-M of KX with 0.174-M HCI. The pk, of HX = 6.72. Give all pH values to 0.01 pH units. a) What is the pH of the original solution before addition of any acid? pH = b) How many mL of acid are required to reach...
30 Consider the titration of a 40.0 mL of 0.113 M weak acid HA (Ka=2.7 x 10) with 0.100 M LIOH. a What is the pH of the solution before any base has been added? 3 points b What would be the pH of the solution after the addition of 20.0 mL of LIOH? 3 points How many mL of the LiOH would be required to reach the halfway point of the titration? 3 points d What is the pH...
16.36 Consider the titration of 40.0 mL of 0.100 M NaOH with 0.100 M HCI. a) b) c) What is the pH after adding 35.0 mL of acid? What is the pH at the equivalence point? What is the pH after adding 45.0 mL of acid?
1. The potentiometric titration of 25.00 mL of sodium malonate (the conjugate base of malonic acid, HOOCCH2COOH which has Kal -1.42x103 and Ka2 2.01x10 with 0.2041 M HCl gave endpoints at 13.01 mL and 26.08 mL. A) Sketch the titration curve (roughly, don't worry about exact pH values, just the general shape of the curve) and label each of the following points with the type of acid/base solution (i.e., is it a strong acid, a weak base, a buffer, etc.):...
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: 3.96 Make ICE table and use simplified method of successive approximations (no iterations needed). How many mL of NaOH are added to reach the equivalence point? Answer: 8 What is the pH after 3.20...
7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate the pH of the following and sketch the titration curve. Kb 1.8 x 10 f. Before the titration starts g. After addition of 2.5 ml of HCl h. After addition of 5.0 ml of HCI i. After addition of 10.0 ml of HC
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