Help! Please solve Q5 all parts (b)The table shows information about some acid-base indicators.(i)(ii)Indicatorpentamethoxy rednaphthyl red4-nitrophenolcresol purplepentamethoxy rednaphthyl red4-nitrophenolpH rangecresol purple1.2-3.2Page 9 of 143.7-5.05.6-7.07.6-9.2Lower pHcolourvioletredcolourlessyellowWhich indicator in the table could be used for the titration that produces curveE but not for the titration that produces curve F?Tick (✓) one box.Higher pH colourcolourlessyellowyellowpurpleGive the colour change at the end point of the titration that produces curve Hwhen naphthyl red is used as the indicator.(iii) A beaker contains 25 cm³ of a buffer solution at pH = 6.0Two drops of each of the four indicators in the table are added to this solution.State the colour of the mixture of indicators in this buffer solution.You should assume that the indicators do not react with each other. Q5.Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions ofacids and bases are shown below.All solutions have concentrations of 0.1 mol dm-³.PHPH(ii)1412-10-(iii)8-14.1210-usPH6-4-2-6-6-4-E2-Page 8 of 1400 10 20 30 40 50Volume/cm³G14-12-10-8-Ľ6-19074-2-0-010 20 30 40 50Volume/cm³PH00 10 20 30 40 50Volume/cm³141210-(i) sodium hydroxide to 25 cm³ of ethanoic acidammonia to 25 cm³ hydrobromic acid8-6-4-2F0(a)In this part of the question, write the appropriate letter in each box.From the curves E, F, G and H, choose the curve produced by the addition ofH10 20 30 40 50Volume/cm³hydrochloric acid to 25 cm³ of potassium hydroxide

5) Here we have to predict the correct titration curve for the following acid - base titration. At…

Q5. Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. All solutions have concentrations of 0.1 mol dm-³. (a) PH 14- 12- PH 10- 8- 6- 6- 4- 2- 0 0 14- 12- 10- 8- 6- 4- 2- 14 12 10- en 8- PH 6- 4- 2 10 20 30 40 50 Volume/cm³ 0- E 0 Page 8 of 14 10 20 30 40 50 Volume/cm³ G PH 14. 12 10- F 6- 4- 2- 0 0 10 20 30 40 50 Volume/cm³ H 0 10 20 30 40 50 Volume/cm³ In this part of the question, write the appropriate letter in each box. From the curves E, F, G and H, choose the curve produced by the addition of

Q5. Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. All solutions have concentrations of 0.1 mol dm-³. (a) PH 14- 12- PH 10- 8- 6- 6- 4- 2- 0 0 14- 12- 10- 8- 6- 4- 2- 14 12 10- en 8- PH 6- 4- 2 10 20 30 40 50 Volume/cm³ 0- E 0 Page 8 of 14 10 20 30 40 50 Volume/cm³ G PH 14. 12 10- F 6- 4- 2- 0 0 10 20 30 40 50 Volume/cm³ H 0 10 20 30 40 50 Volume/cm³ In this part of the question, write the appropriate letter in each box. From the curves E, F, G and H, choose the curve produced by the addition of

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.46QE

See similar textbooks

Similar questions

Consider the bases in Table 13-3. Which base would be the best choice for preparing a pH = 5.00 buffer? Explain how to make 1.0 L of this buffer.
Consider the acids in Table 13-2. Which acid would be the best choice for preparing a pH = 7.00 buffer? Explain how to make 1.0 L of this buffer.
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
8-58 What is the connection between buffer action and Le Chatelier's principle?
8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.
8-51 What is the end point of a titration?
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 57 and 59?
Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the major species in solution at equilibrium (besides water), and what are their concentrations?