A 20.0 mL sample of 0.150 M ethylamine CH3CH2NH2 is titrated with 0.0981 M HCl. What is the pH after the addition of 0 mL HCl? pKb (CH3CH2NH2) = 3.25.
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- A 20.0 mL sample of 0.150 M ethylamine CH3CH2NH2 is titrated with 0.0981 M HCl. What is the pH after the addition of 0 mL HCl? pKb (CH3CH2NH2) = 3.25.
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- The weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of the acids were 50.0-mL samples of 0.10 M concentration). a. Which pH curve corresponds to the weakest acid? b. Which pH curve corresponds to the strongest acid? Which point on the pH curve would you examine to see if this acid is a strong acid or a weak acid (assuming you did not know the initial concentration of the acid)? c. Which pH curve corresponds to an acid with Ka 1 106?What is the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution consisting of 0.169 M NH3 and 0.183 M NH4Cl?
- Aniline hydrochloride, (C6H5NH3)Cl, is a weak acid. (Its conjugate base is the weak base aniline, C6H5NH2.) The acid can be titrated with a strong base such as NaOH. C6H5NH3+(aq)+OH(aq)C6H5NH2(aq)+H2O(l) Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M NaOH. (Ka for aniline hydrochloride is 2.4 105.) (a) What is the pH of the (C6H5NH3) solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 could be used to detect the equivalence point? (e) Calculate the pH of the solution after adding 10.0, 20.0, and 30.0 mL of base. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?A chemistry graduate student is given 100. mL of a 0.90M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 104. f (CH3)2NHCl should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 10.66? mass of You may assume that the volume of the solution doesn't change when the (CH3)2NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0x12 What X S ? EFET ol Ar
- A chemistry graduate student is given 450. mL of a 0.50M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 10¯ª. What mass of (CH3)NHBr should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 11.20? You may assume that the volume of the solution doesn't change when the (CH3) NHBr is dissolved in it. Be sure your answer has a 3 unit symbol, and round it to 2 significant digits. ? 10: 000A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.A 65.0 mL solution of 0.158 M potassium alaninate ( H,NC, H,CO, K) is titrated with 0.158 M HCI. The pK values for the amino acid alanine are 2.344 (pKa1) and 9.868 ( CH3 pKa2), which correspond to the carboxylic acid and amino H2N CH-C- groups, respectively. Calculate the pH at the first equivalence point. Potassium Alaninate pH = %3D Calculate the pH at the second equivalence point. pH =
- 3.) A chemistry graduate student is given 300.mL of a 0.50M pyridine C5H5N solution. Pyridine is a weak base with Kb = 1.7x10^−9. What mass of C5H5NHBr should the student dissolve in the C5H5N solution to turn it into a buffer with pH =5.54? You may assume that the volume of the solution doesn't change when the C5H5NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4).This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 35.00 mL of acid has been added?A chemistry graduate student is given 250.mL of a 0.30M propanoic acid HC2H5CO2 solution. Propanoic acid is a weak acid with Ka=1.3x10^−5. What mass of KC2H5CO2 should the student dissolve in the HC2H5CO2 solution to turn it into a buffer with pH=4.30? You may assume that the volume of the solution doesn't change when the KC2H5CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
