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Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1....
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH,...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1....
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. Phosphorus pentachloride decomposes according to first order kinetics at 298 K, as shown below. PC15(9) = PC13(g) + Cl2(g) a. Draw a reaction coordinate diagram for the reaction. Label reactants, products, activation energy, and AH. (5 pts) b. Draw a free energy diagram for the reaction (free energy as a function of reaction coordinate). Label reactants, products, AG®, and the equilibrium position. (5 pts)
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1....
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. Phosphorus pentachloride decomposes according to first order kinetics at 298 K, as shown below. PCls(g) =PC1(9) + Cl2(g) a. Draw a reaction coordinate diagram for the reaction. Label reactants, products, activation energy, and AH°. (5 pts) b. Draw a free energy diagram for the reaction (free energy as a function of reaction coordinate). Label reactants, products, AGC, and the equilibrium position. (5 pts)
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH....
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
Please help with solving Question 1 (A-C) Thank you! Unless otherwise specified in the problem, you...
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
Please answer #2 php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your...
Please answer #2
php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your work. Don't forget the significant figures and units!! Would the following mixtures result in buffer solutions? (Justify your answers) 1. a 100.0 ml, of 0.10 M NH, 100.0 mL of0.15 M NHaCl b. 50.0 mL of 0.10 M HCIO4, 35.0 mL if 0.15 M NaCIO c. 125.0 ml, of 0.15 CH?NH2. 120.0 mL of 0.25 M CHNE ICI d. 165.0 mL of 0.10 M...
Answer all assigned questions and problems, and show all work. Determine the pH of (a) a...
Answer all assigned questions and problems, and show all work. Determine the pH of (a) a 0.40 MCH3CO2H solution, (b) a solution that is 0.40 MCH3CO2H and 0.20 MNaCH3CO2. (8 points) (Reference: Chang 16.5) Which of the following solutions can act as a buffer? (a) KCl/HCl, (b) KHSO4/H2SO4, (c) KNO2/HNO2.(5 points) (Reference: Chang 16.9) Calculate the pH of the buffer system made up of 0.15 MNH3/0.35 MNH4Cl. (5 points) (Reference: Chang 16.11) The pH of a bicarbonate-carbonic acid buffer is...
L4) K.a-5.5 x 10s for acrylic acid (CHsCOOH) (a) (1 pt.) Determine the Kb of acrylate...
L4) K.a-5.5 x 10s for acrylic acid (CHsCOOH) (a) (1 pt.) Determine the Kb of acrylate ion (C2H COO) (b) (6 pts.) 50.0 mL of 0.40 M acrylic acid (C2H COOH) solution is titrated with 0.40 M NaOH. Determine the pH of the solution at the equivalence point when 50.0 mL of 0.40 M NaOH is added. Note that the reaction between acrylic acid and NaOH produces sodium acrylate (C2HCOONa): C:HCOOH (aq) + NaOH (aq) C2H3COONa (aq) H2O (1) (c)...
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg = 1.8 x 10-5. b. 35.0 mL of 0.175 M NH3 is mixed with 15.0 mL of 0.10 M HCl. c. 50.0 mL of 0.275 M acetic acid is mixed with 100. mL of 0.100 M HCl. d. The equivalence point of a 50.0 mL solution of 0.120 M acetic acid titrated by 0.100 M NaOH.
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. Phosphorus pentachloride decomposes according to first order kinetics at 298 K, as shown below. PC15(9) = PC13(g) + Cl2(g) a. Draw a reaction coordinate diagram for the reaction. Label reactants, products, activation energy, and AH. (5 pts) b. Draw a free energy diagram for the reaction (free energy as a function of reaction coordinate). Label reactants, products, AG®, and the equilibrium position. (5 pts)
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. Phosphorus pentachloride decomposes according to first order kinetics at 298 K, as shown below. PCls(g) =PC1(9) + Cl2(g) a. Draw a reaction coordinate diagram for the reaction. Label reactants, products, activation energy, and AH°. (5 pts) b. Draw a free energy diagram for the reaction (free energy as a function of reaction coordinate). Label reactants, products, AGC, and the equilibrium position. (5 pts)
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
Please answer #2
php/ 20 %20Extra%20Credit%20-%20Spring%2020 18.pdf CHEM 108- Extra Credit-Spring 2018 IMPORTANT: Show ALL your work. Don't forget the significant figures and units!! Would the following mixtures result in buffer solutions? (Justify your answers) 1. a 100.0 ml, of 0.10 M NH, 100.0 mL of0.15 M NHaCl b. 50.0 mL of 0.10 M HCIO4, 35.0 mL if 0.15 M NaCIO c. 125.0 ml, of 0.15 CH?NH2. 120.0 mL of 0.25 M CHNE ICI d. 165.0 mL of 0.10 M...
L4) K.a-5.5 x 10s for acrylic acid (CHsCOOH) (a) (1 pt.) Determine the Kb of acrylate ion (C2H COO) (b) (6 pts.) 50.0 mL of 0.40 M acrylic acid (C2H COOH) solution is titrated with 0.40 M NaOH. Determine the pH of the solution at the equivalence point when 50.0 mL of 0.40 M NaOH is added. Note that the reaction between acrylic acid and NaOH produces sodium acrylate (C2HCOONa): C:HCOOH (aq) + NaOH (aq) C2H3COONa (aq) H2O (1) (c)...
4. Calculate the percent ionization and pH of the following solutions: a. 0.175 M NH3 Kg = 1.8 x 10-5. b. 35.0 mL of 0.175 M NH3 is mixed with 15.0 mL of 0.10 M HCl. c. 50.0 mL of 0.275 M acetic acid is mixed with 100. mL of 0.100 M HCl. d. The equivalence point of a 50.0 mL solution of 0.120 M acetic acid titrated by 0.100 M NaOH.
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