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![Calculating pka: Ka = 3.5x104 pka = - log [ Ka ] pk = - log (3.5x104 ] pka = 3.46 Calculating pH: pka = 3.46 number of moles](http://img.homeworklib.com/questions/426ac8f0-d1fc-11eb-afc4-e5dc88417ea3.png?x-oss-process=image/resize,w_560)
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Question 1 2 pts Time Ru Attempt d 55 Minu Calculate the pH formed by mixing...
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and...
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.040 M HCI. Ka of HF = 7.24 x 10-4. A 3.32 B.3.54 C.3.14 D.2.74 E 2.96
5. Calculate the pH of buffer formed by mixing 85 mL of 0.12 M lactic acid...
5. Calculate the pH of buffer formed by mixing 85 mL of 0.12 M lactic acid with 95 mL of 0.16 M sodium lactate (K, for lactic acid is 1.4 x 10-) a. 3.77 b) 4.03 ) 3.56 d) 4.23 e) 3.66 6. 18 2.5mL of 0.30M AgNO3 is mixed with 7.5mL of 0.015M Na2SO4, should a precipitate of Ag2SO4 form? (Ksp - 1.2x10-5 a) Q - Ksp the system is at equilibrium and the solution is saturated b) Q<Ksp,...
. (5 pts) The pKa of HF is 3.17. a) Calculate the pH of a 1.00...
. (5 pts) The pKa of HF is 3.17. a) Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF. b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCI?
Question 8 (10 points) Calculate the pH of a solution made by mixing 100.0 mL of...
Question 8 (10 points) Calculate the pH of a solution made by mixing 100.0 mL of 0.644 MNH; with 100.0 ml. of 0.100 MHCI. (K for NH; = 1.8 x 10-) 9.99 4.01 8.52 9.26 none of these Question 9 (10 points) Calculate the pH of a solution that is 0.50 Min HF (K-72 x 10-) and 0.66 Min NaF 3.14 3.26 b BE
Question 12 1 pts Calculate the pH of a solution obtained by mixing 60.79 mL of...
Question 12 1 pts Calculate the pH of a solution obtained by mixing 60.79 mL of 0.11 M CH3COOH with 12.47 mL of 0.12 M NaOH. (K,(CH3COOH) = 1.8 x 10-5) Enter your answer to 2 decimal places. For example, if your answer is pH = 12, enter 12.00
1) Calculate the pH of a solution formed by mixing 65 mL of a solution that...
1) Calculate the pH of a solution formed by mixing 65 mL of a solution that is 0.15 M in NaHCO3 with 75 mL of a solution that is 0.10 M in Na2CO3. Express your answer to two decimal places.
please explain how you got all your answers 10. Calculate the pH of a 0.30 M...
please explain how you got all your answers
10. Calculate the pH of a 0.30 M formic acid solution. (K-1.8 x 10") Weak monoprotic acid. 11. Calculate the K, for a 0.050 M solution of HA (weak acid) if the pH = 4.65. 12. What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25C? (K. of F = 1.4 x 10) 13. Which of...
Complex-Formation Titrations +2 10. Calculate the Ca concentration and pCa logCa D of a solution that results from the mixing of each of the following solutions (buffered at a pH of 10.0): +2 +2...
Complex-Formation Titrations +2 10. Calculate the Ca concentration and pCa logCa D of a solution that results from the mixing of each of the following solutions (buffered at a pH of 10.0): +2 +2 +2 EDTA +10 The complexation reaction: Ca CaEDTA atapH of 10.0, has an Kefr r 5.0 s 10 +2 +10 Kerr-lCaEDTAI/(1 Ca.-11 EDTA I) = 5.0 x 10 a) Calculate the pCa of a solution of 50.0 ml of 0.0102 MCa with 50.0 ml of 0.0100...
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric...
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the concentration of [F 1. Kb.[OH formed from the weak base ionization, and pH at the equivalence point? The K, of hydrofluoric acid is 3.5 x 10 In the space below enter your numerical answers in order of 1 to 4 include units. 1- Molarity of the Fluoride ion formed 2. The numerical...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.040 M HCI. Ka of HF = 7.24 x 10-4. A 3.32 B.3.54 C.3.14 D.2.74 E 2.96
5. Calculate the pH of buffer formed by mixing 85 mL of 0.12 M lactic acid with 95 mL of 0.16 M sodium lactate (K, for lactic acid is 1.4 x 10-) a. 3.77 b) 4.03 ) 3.56 d) 4.23 e) 3.66 6. 18 2.5mL of 0.30M AgNO3 is mixed with 7.5mL of 0.015M Na2SO4, should a precipitate of Ag2SO4 form? (Ksp - 1.2x10-5 a) Q - Ksp the system is at equilibrium and the solution is saturated b) Q<Ksp,...
. (5 pts) The pKa of HF is 3.17. a) Calculate the pH of a 1.00 L solution that is 1.00 M HF and 1.50 M NaF. b) What is the pH of this solution after addition of 50.0 mL of 10.0 M HCI?
Question 8 (10 points) Calculate the pH of a solution made by mixing 100.0 mL of 0.644 MNH; with 100.0 ml. of 0.100 MHCI. (K for NH; = 1.8 x 10-) 9.99 4.01 8.52 9.26 none of these Question 9 (10 points) Calculate the pH of a solution that is 0.50 Min HF (K-72 x 10-) and 0.66 Min NaF 3.14 3.26 b BE
Question 12 1 pts Calculate the pH of a solution obtained by mixing 60.79 mL of 0.11 M CH3COOH with 12.47 mL of 0.12 M NaOH. (K,(CH3COOH) = 1.8 x 10-5) Enter your answer to 2 decimal places. For example, if your answer is pH = 12, enter 12.00
please explain how you got all your answers
10. Calculate the pH of a 0.30 M formic acid solution. (K-1.8 x 10") Weak monoprotic acid. 11. Calculate the K, for a 0.050 M solution of HA (weak acid) if the pH = 4.65. 12. What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25C? (K. of F = 1.4 x 10) 13. Which of...
Complex-Formation Titrations +2 10. Calculate the Ca concentration and pCa logCa D of a solution that results from the mixing of each of the following solutions (buffered at a pH of 10.0): +2 +2 +2 EDTA +10 The complexation reaction: Ca CaEDTA atapH of 10.0, has an Kefr r 5.0 s 10 +2 +10 Kerr-lCaEDTAI/(1 Ca.-11 EDTA I) = 5.0 x 10 a) Calculate the pCa of a solution of 50.0 ml of 0.0102 MCa with 50.0 ml of 0.0100...
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the concentration of [F 1. Kb.[OH formed from the weak base ionization, and pH at the equivalence point? The K, of hydrofluoric acid is 3.5 x 10 In the space below enter your numerical answers in order of 1 to 4 include units. 1- Molarity of the Fluoride ion formed 2. The numerical...
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