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13. (25 pts total) Dimethylamine, or (CH3)2 NH, is a weak base with a Ko of...
dimethylamine (CH3)2NH, is a weak base with a Kb of 5.95*10-4. It is titrated with hydrochloric...
dimethylamine (CH3)2NH, is a weak base with a Kb of 5.95*10-4. It is titrated with hydrochloric acid (HCl). A. Write the reaction with proper substances, arrows, and states of matter. B. If 25.00mL of a 0.130 M (CH3)2NH are mixed with 8.00mL of 0.200 M HCl, what is the pH? C. At what volume of 0.200 M HCl is required to reach the equivalence point?
2. (32 points) Strychnine is a weak base with a pk of 5.74. A 150. mL...
2. (32 points) Strychnine is a weak base with a pk of 5.74. A 150. mL sample of 0.076 M strychnine solution is titrated using 0.060 M hydrochloric acid. What is the pH of the solution at the following points: a) No acid has been added. b) 25.00 mL of acid have been added. c) 100.00 mL of acid have been added. d) The midpoint of the titration. e) The equivalence point of the titration. 1) Sketch this titration curve,...
Strychnine is a weak base with a pKb of 5.74. A 150. mL sample of 0.076...
Strychnine is a weak base with a pKb of 5.74. A 150. mL sample of 0.076 M strychnine solution is titrated using 0.060 M hydrochloric acid. What is the pH of the solution at the following points: a) No acid has been added. b) 25.00 mL of acid have been added. c) 100.00 mL of acid have been added. d) The midpoint of the titration. e) The equivalence point of the titration. f) Sketch this titration curve, labeling the axes,...
Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HCI
Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL (b) 6.0 mL (c) 12.0 mL (d) 18.0 mL
1. (7 pts) 35.0 mL of a 0.275 M weak base is titrated with 0.325 M...
1. (7 pts) 35.0 mL of a 0.275 M weak base is titrated with 0.325 M HCl. Determine each of the following and sketch the titration curve. If you do the problem on other paper, you will need to do a reasonable approximation of the graph. Ky of the weak base = 2.7 x 10-4 a. The volume of added acid required to reach the equivalence point. b. The initial pH. c. The pH when 5.0 mL of acid has...
BH Ž B+H* Formal cone Sony Xm 2. A 50.0-ml aliquot of 0.200 M weak base...
BH Ž B+H* Formal cone Sony Xm 2. A 50.0-ml aliquot of 0.200 M weak base B (pKa of BH is 9.00) was titrated with 0.30 M HNO3. (a) (4 pts) calculate the pH at Va=0 mL, it H e B+ H₂O - BHt tot 0.200M-x ko ka a 1.0X10-14 lrox 16093 = 1.0X10-5 0.2001 => 2= 1.41 810 poh = 2.85 pH = /11.15 (b) (4 pts) calculate the pH at Va = 5.00 mL, [B] = 0. 200...
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...
A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is...
A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is: N2H4 + HCI= N2H5+ + C1- * O rö oo O ö in O ü o O ö O e. 7.00 Consider the following Bronsted-Lowery acid-base reaction: HCIO2 + N(CH3)3 = [HN(CH3)3]* + C1025 Which two substances represent Bronsted-Lowery bases in...
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation...
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation for the reaction of NH, (aq) with HCL(aq) (1 pt.) What is the volume of base added at the equivalence point? Show work or reasoning. b. (1 pt.) Will the pH of the equivalence point be higher than, lower than or...
please answer all parts of the question Question 13 (18 points) A 25.00mL aliquot of 0.376...
please answer all parts of the question
Question 13 (18 points) A 25.00mL aliquot of 0.376 M butanoic acid is titrated with 0.436 M sodium hydroxide. a Write an equation for the neutralization reaction that is occurring. (1 point) Calculate the initial pH of the acid solution before the titration begins (3 points) Calculate the volume of base solution that is required to reach the equivalence point (3 points) Calculate the pH at the equivalence point (3 points) Calculate the...
2. (32 points) Strychnine is a weak base with a pk of 5.74. A 150. mL sample of 0.076 M strychnine solution is titrated using 0.060 M hydrochloric acid. What is the pH of the solution at the following points: a) No acid has been added. b) 25.00 mL of acid have been added. c) 100.00 mL of acid have been added. d) The midpoint of the titration. e) The equivalence point of the titration. 1) Sketch this titration curve,...
1. (7 pts) 35.0 mL of a 0.275 M weak base is titrated with 0.325 M HCl. Determine each of the following and sketch the titration curve. If you do the problem on other paper, you will need to do a reasonable approximation of the graph. Ky of the weak base = 2.7 x 10-4 a. The volume of added acid required to reach the equivalence point. b. The initial pH. c. The pH when 5.0 mL of acid has...
BH Ž B+H* Formal cone Sony Xm 2. A 50.0-ml aliquot of 0.200 M weak base B (pKa of BH is 9.00) was titrated with 0.30 M HNO3. (a) (4 pts) calculate the pH at Va=0 mL, it H e B+ H₂O - BHt tot 0.200M-x ko ka a 1.0X10-14 lrox 16093 = 1.0X10-5 0.2001 => 2= 1.41 810 poh = 2.85 pH = /11.15 (b) (4 pts) calculate the pH at Va = 5.00 mL, [B] = 0. 200...
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...
A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is: N2H4 + HCI= N2H5+ + C1- * O rö oo O ö in O ü o O ö O e. 7.00 Consider the following Bronsted-Lowery acid-base reaction: HCIO2 + N(CH3)3 = [HN(CH3)3]* + C1025 Which two substances represent Bronsted-Lowery bases in...
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation for the reaction of NH, (aq) with HCL(aq) (1 pt.) What is the volume of base added at the equivalence point? Show work or reasoning. b. (1 pt.) Will the pH of the equivalence point be higher than, lower than or...
please answer all parts of the question
Question 13 (18 points) A 25.00mL aliquot of 0.376 M butanoic acid is titrated with 0.436 M sodium hydroxide. a Write an equation for the neutralization reaction that is occurring. (1 point) Calculate the initial pH of the acid solution before the titration begins (3 points) Calculate the volume of base solution that is required to reach the equivalence point (3 points) Calculate the pH at the equivalence point (3 points) Calculate the...
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