EBK GENERAL CHEMISTRY
11th Edition
ISBN: 8220103631259
Author: Bissonnette
Publisher: YUZU
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Chapter 17, Problem 52E
For the titration of 25.00 mL 0.100M
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EBK GENERAL CHEMISTRY
Ch. 17 - For a solution that e 0.275M CH2CH2 COOH...Ch. 17 - For a solution that is 0164 U NH2 and 0.102MNH4Cl...Ch. 17 - Prob. 3ECh. 17 - In Example 16-4, we calculated the percent...Ch. 17 - Calculate [H2OOH-] in a solution that is (a)...Ch. 17 - Calculate [OH-] in a solution that is (a) 0.0062 U...Ch. 17 - What concentration of formate ion, [HCOO-], should...Ch. 17 - What concentration of ammonia. [NH2] , should be...Ch. 17 - Calculate the pH of a buffer that is a. 0.012 M...Ch. 17 - Lactic acid, CH2CH(OH)COOH , is found in sour...
Ch. 17 - Indicate which of the following aqueous solutions...Ch. 17 - The H2PO4-HPO4- combination plays a role in...Ch. 17 - What is the pH of a solution Obtained by adding...Ch. 17 - What the pH of solution prepared by dissolving...Ch. 17 - You wish to prepare a buffer solution w pH = 945...Ch. 17 - You prepare a buffer solution by dissolving 2.00 g...Ch. 17 - If 0.55 ml. of 12 M HCI is added to 0100 L of the...Ch. 17 - If 0.35 mL of 15 P.4 NH is added to 0750 L of the...Ch. 17 - You are asked to prepare e buffer solution why a...Ch. 17 - You are asked to reduce the pH of the 03001 of...Ch. 17 - Given 1.00 L of a solution that is 0.100 hl...Ch. 17 - Given 125mL of a solution that is 0.0500 M CH2NH2...Ch. 17 - A solution of volume 750 mL contars 15.5 mmol...Ch. 17 - A solution of volume 0.500 L contains 1.68 g NH...Ch. 17 - A handbook lets various procedures for preparing...Ch. 17 - An acetic acid-sodium acetate buffer can be...Ch. 17 - A handbook lists the following data: Which of...Ch. 17 - With reference to the indicators listed in...Ch. 17 - In use of acid—base indicators, a. Why is it...Ch. 17 - The indicator methyl red has a pKHIN=4.95 . It...Ch. 17 - Phenol red indicator changes from yellow to red in...Ch. 17 - Thymol blue indicator has two pH ranges. It...Ch. 17 - In the titration of 10.00 mL of 0.04050 M HCI with...Ch. 17 - Solution (a) is 1000 mL of 0.100 N HCI and...Ch. 17 - A 25.00 mL sample of H2PO4(aq) requires 31.15 mL...Ch. 17 - A 2000 ml sample of H2PO4(aq) requires 18.67 mL...Ch. 17 - Two aqueous solutions are mixed 50.0 mL of 0.0150M...Ch. 17 - Two solutions are mixed 100.0 mL of HCI(aq) with...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points m the titration...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points lithe titration of...Ch. 17 - Explain why the volume of 0.100 M NeOH required to...Ch. 17 - Explain whether the equivalence point of each of...Ch. 17 - Sketch the titration curves of the following...Ch. 17 - Determine the blowing characteristeristics of the...Ch. 17 - In the titration of 2000 mL of 0175 M NaOH,...Ch. 17 - In the titration of 25.00mL of 0.100M CH2COOH ,...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - For me titration of 25.00 mL of 0.100M NaOH with...Ch. 17 - For the titration of 25.00 mL 0.100M NH2 with...Ch. 17 - Is a solution that is 0.10 M Na2S(aq) likely to be...Ch. 17 - Is a solution of sodium dihydrogen citrate,...Ch. 17 - Sodium phosphate Na2PO4 , is made commecie1y by...Ch. 17 - Both sodium hydrogen carbonate (sodium...Ch. 17 - The pH of a solution of 19.5 g of malonic acid in...Ch. 17 - The ionization constants of ortho-phthalic acid...Ch. 17 - What stoichimetric concentration of the indicated...Ch. 17 - What stocichiometric concentration of the...Ch. 17 - Using appropriate equilibrium constants but...Ch. 17 - Prob. 62ECh. 17 - Sodium hydrogen sulfate NaHSO4 , an acidic salt...Ch. 17 - You are given 250.0mL of 0.100M CH3 CH2 COOH...Ch. 17 - Even though the carbonic acid-hydrogen carbonate...Ch. 17 - Thymol blue in its acid range is not a suitable...Ch. 17 - Rather than calculate the pH for different volumes...Ch. 17 - Use the method of Exercise 67 to determine the...Ch. 17 - A buffer solution can be prepared by starting with...Ch. 17 - You are asked to prepare a KH2PO4-Na2HPO2 solution...Ch. 17 - You are asked to bring the pH of 0.500 L of 0.500...Ch. 17 - Because an acid-base indicator a weak acid, I can...Ch. 17 - The neutralization of NaOH 2by HCl is represented...Ch. 17 - The titration of a weak acid by a weak base a not...Ch. 17 - At times a salt of a we base can be titrated by a...Ch. 17 - Sulfuric acid is a diprotic acid, strong in the...Ch. 17 - Carbonic acid is a weak diprotic acid (H2CO2) with...Ch. 17 - Prob. 78IAECh. 17 - Complete the derivation of equation (17.10)...Ch. 17 - Explain why equation (17.10) fads when applied to...Ch. 17 - Prob. 81IAECh. 17 - Prob. 82IAECh. 17 - Prob. 83IAECh. 17 - Prob. 84IAECh. 17 - Prob. 85IAECh. 17 - Calculate the pH of a solution that is 0.050 U...Ch. 17 - Prob. 87IAECh. 17 - The Henderson-Hasselbalch equation can be written...Ch. 17 - The pH of ocean water depends on the amount of...Ch. 17 - A sample of water contains 23.0 g L1 of Na+ (aq),...Ch. 17 - Prob. 91IAECh. 17 - Prob. 92FPCh. 17 - In some cases the titration curve for a mature of...Ch. 17 - Amino acids contain both an acidic carboxylic acid...Ch. 17 - In your own words, define or explain the following...Ch. 17 - Prob. 96SAECh. 17 - Explain the important distinctions between each...Ch. 17 - Write equations to show how each of the following...Ch. 17 - Sketch the titration curves that you would expect...Ch. 17 - A 2500-mL sample of 0.0100M C8C5COOH (Kg=6.3103)...Ch. 17 - Prob. 101SAECh. 17 - Prob. 102SAECh. 17 - Prob. 103SAECh. 17 - Prob. 104SAECh. 17 - Prob. 105SAECh. 17 - Calculate the pH of a 0.5 M solution of Ca(HSe)2...Ch. 17 - Prob. 107SAECh. 17 - Prob. 108SAECh. 17 - Prob. 109SAECh. 17 - Prob. 110SAECh. 17 - Prob. 111SAE
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- Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.arrow_forwardThe titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?arrow_forwardCalculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.arrow_forward
- When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.arrow_forwardCalculate the pH during the titration of 50.00 mL of 0.100 M Sr(OH)2 with 0.100 M HNO3 after 0, 50.00, 100.00, and 150.00 mL nitric acid have been added. Graph the titration curve and compare with the titration curve obtained in Exercise 16.22.arrow_forwardRepeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl.arrow_forward
- Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?arrow_forwardA 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?arrow_forwardFor the titration of 50.0 mL of 0.100-M HCl with 0.100-M NaOH, calculate the pH when these volumes of NaOH have been added: (a) 10.0 mL (b) 25.00 mL (c) 45.0 mL (d) 50.5 mLarrow_forward
- Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).arrow_forwardMalonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)arrow_forwardConsider the titration of 100.0 mL of 0.10 M H3AsO4 by 0.10 M NaOH. What are the major species present at 50.0 mL of NaOH added? How would you calculate the pH at this point? Answer the same questions for 150.0 mL of NaOH added. At what volume of NaOH added does pH = pKa1?arrow_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