Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Chapter 16, Problem 16.64QE
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When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5
1) Calculate the pH at this point
2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
Calculate the pH during the titration of 20.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.2000 M HNO3(aq) after 7.24 mL of the acid have been added.
Kb of ethylamine = 6.5 x 10-4.
A sample of vinegar weighing 10.52 g is titrated with NaOH. The end point is overstepped, and the solution is titrated back with HCl. From the following data, calculate the acidity of the vinegar in terms of percentage of acetic acid, CH3COOH
Standardization Data:1.050 mL HCl ≡ 1.000 mL NaOH1.000 mL NaOH ≡ 0.06050 g benzoic acid, C6H5COOH (122.12 g/mol)
Analysis Data:Volume NaOH used = 19.03 mLVolume HCl used for back titration = 1.50 mL
Chapter 16 Solutions
Chemistry: Principles and Practice
Ch. 16 - Prob. 16.1QECh. 16 -
Sketch a titration curve for the titration of...Ch. 16 - Prob. 16.4QECh. 16 - Prob. 16.5QECh. 16 - Explain why the HendersonHasselbalch equation...Ch. 16 - Prob. 16.7QECh. 16 - Prob. 16.8QECh. 16 - Prob. 16.9QECh. 16 - Prob. 16.11QECh. 16 - Prob. 16.13QE
Ch. 16 - Prob. 16.14QECh. 16 - Prob. 16.15QECh. 16 - Prob. 16.16QECh. 16 - Prob. 16.17QECh. 16 - Prob. 16.18QECh. 16 - Calculate the pH during the titration of 100.0 mL...Ch. 16 - Prob. 16.20QECh. 16 - Prob. 16.21QECh. 16 - Calculate the pH during the titration of 50.00 mL...Ch. 16 - Prob. 16.23QECh. 16 - Calculate the pH during the titration of 50.00 mL...Ch. 16 - Prob. 16.25QECh. 16 - Prob. 16.26QECh. 16 - Prob. 16.27QECh. 16 - Prob. 16.28QECh. 16 -
Calculate the pH of solutions that are
0.25 M...Ch. 16 - Prob. 16.30QECh. 16 - Prob. 16.31QECh. 16 - Prob. 16.32QECh. 16 - Prob. 16.35QECh. 16 - Prob. 16.36QECh. 16 - Prob. 16.37QECh. 16 - Prob. 16.38QECh. 16 - Prob. 16.39QECh. 16 -
How many grams of sodium acetate must be added to...Ch. 16 - Prob. 16.41QECh. 16 - Prob. 16.42QECh. 16 - A buffer solution that is 0.100 M acetate ion and...Ch. 16 - Prob. 16.44QECh. 16 - Prob. 16.45QECh. 16 - Prob. 16.46QECh. 16 - Prob. 16.47QECh. 16 - Prob. 16.48QECh. 16 - Estimate the pH that results when the following...Ch. 16 - Estimate the pH that results when the following...Ch. 16 - Prob. 16.51QECh. 16 - Prob. 16.52QECh. 16 - Prob. 16.53QECh. 16 - Prob. 16.54QECh. 16 - Prob. 16.55QECh. 16 - Prob. 16.56QECh. 16 - Prob. 16.57QECh. 16 - Prob. 16.58QECh. 16 - Prob. 16.59QECh. 16 - Consider all acid-base indicators discussed in...Ch. 16 - Prob. 16.61QECh. 16 - Chloropropionic acid, ClCH2CH2COOH, is a weak...Ch. 16 - Prob. 16.63QECh. 16 - Prob. 16.64QECh. 16 - Prob. 16.65QECh. 16 - Write the chemical equilibrium and expression for...Ch. 16 - Calculate the pH of 0.010 M ascorbic acid.Ch. 16 - Prob. 16.68QECh. 16 - Prob. 16.69QECh. 16 - Prob. 16.70QECh. 16 - Prob. 16.71QECh. 16 - Prob. 16.72QECh. 16 - Prob. 16.73QECh. 16 - Prob. 16.74QECh. 16 - Prob. 16.75QECh. 16 - Which compound in each pair is more soluble in...Ch. 16 - Prob. 16.77QECh. 16 - Prob. 16.78QECh. 16 - Prob. 16.79QECh. 16 - Calculate the pH of each of the following...Ch. 16 - Write the chemical equation and the expression for...Ch. 16 - Prob. 16.82QECh. 16 - Prob. 16.83QECh. 16 - Phenolphthalein is a commonly used indicator that...Ch. 16 - Prob. 16.85QECh. 16 - Prob. 16.86QECh. 16 - Prob. 16.87QECh. 16 - Determine the dominant acid-base equilibrium that...Ch. 16 - Prob. 16.89QECh. 16 - Prob. 16.90QECh. 16 - Prob. 16.91QECh. 16 - Prob. 16.92QECh. 16 - Prob. 16.93QECh. 16 - Prob. 16.94QECh. 16 - Prob. 16.95QECh. 16 - Prob. 16.96QECh. 16 - Prob. 16.97QECh. 16 - A monoprotic organic acid that has a molar mass of...Ch. 16 - A scientist has synthesized a diprotic organic...Ch. 16 - Prob. 16.100QECh. 16 - What is a good indicator to use in the titration...Ch. 16 - Prob. 16.102QECh. 16 - A bottle of concentrated hydroiodic acid is 57% HI...
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- Which of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.arrow_forwardGiven three acid-base indicators—methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)—which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acidarrow_forwardPhenolphthalein, a colorless weak acid (Ka = 6.31 x 10^-10) which dissociates in water forming pink anions is widely considered a suitable indicator for this titration. Along with a suitable calculation, find the working/useful range of this indicator to explain its use.arrow_forward
- Suppose that a student is determining the total base content of an antacid tablet by performing a back titration. He/she weighs out a 0.3012 g portion of a tablet whose total weight is 1.5312 g, dissolves this in exactly 40.00 mL of deionized water, and then adds exactly 30.00 mL of 0.1000M HCl in order to bring the pH down to 1.9. This solution is then carefully back-titrated with 0.2000M NaOH, with 12.50 mL required to reach the equivalence point. Calculate the total base content (i.e., the number of mmoles of base contained) of the antacid tablet. (Formula weight of HCL = 36.46 g/m; formula weight of NaOH= 40.00 g/m) A) 0.500 mmolesD) 8.90 mmoles B) 1.75 mmolesE) none of the above C) 2.54 mmolesarrow_forwardanalytical chemistry. Given the following titration curve, what is the suitable indicator for this titration? a) thymolphthaline; pH range (9.3-10.5) b) bromothymol blue; pH range (6.2-7.6) c) Thymol blue; pH range (1.2-2.8) d) bromcresol green; pH range (4.1-5.4) e) phenolphthalein; pH range (8.6-10.2)arrow_forwardA sample of 50.00 mL of 0.1000 M aqueous solution of chloroacetic acid, CH2ClCOOH (K1= 1.4 × 10-3), is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following stages in the titration, and plot thetitration curve: 0, 5.00, 25.00, 49.00, 49.90, 50.00, 50.10, and 55.00 mL NaOH.arrow_forward
- explain each of the following cases. a) when we treat 1 mol / liter of hydrochloric acid, the pH increases. There comes a cast that the pH reaches a certain value and does not change anymore. Why does this happen? b) Methyl orange can be used to determine the final titration point of nitric acid with ammonia solution, while phenophthalein is not used in this case. Why? c) pH of 10-8 mol / l HCl is not 8. Why?arrow_forwardCalculate the pH after addition of 0.00, 5.00, 25.00, 45.00 mL, 50.00 mL, 55.00 mL of 0.1200 M HCl in the titration of 50.00 mL of 0.1500 M hydrazinearrow_forwardCalculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. Group of answer choices 3.22 3.32 4.70 4.80 9.60 9.39arrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY