Consider the following list of indicators. Indicator pK, Methyl red Chlorophenol red Ethyl orange m-nitrophenol Bromphenol blue 5.00 6.25 4.34 8.28 3.20 Which one of these indicators would be best to use in a titration of a 0.100 M solution of acetic acid (K, - 1.8 x 105) witha 0.100 M solution of strong base. Bromphenol blue Methyl red m-nitrophenol Chlorophenol red Ethyl orange

Consider the following list of indicators. Indicator pK, Methyl red Chlorophenol red Ethyl orange m-nitrophenol Bromphenol blue 5.00 6.25 4.34 8.28 3.20 Which one of these indicators would be best to use in a titration of a 0.100 M solution of acetic acid (K, - 1.8 x 105) witha 0.100 M solution of strong base. Bromphenol blue Methyl red m-nitrophenol Chlorophenol red Ethyl orange

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

12 pH 7- a ml added 1. The titration curve represents the titration of (a) strong acid titrates a strong base. (b) strong acid titrates a weak base. (c) strong base titrates a weak acid. (d) weak acid titrates a weak base. 2. Using the chart of indicators (below), select a suitable indicator for the end point of the titration. pH Range 3.1 – 4.4 Indicator (a) Methyl orange (b) Bromothymol blue (c) Thymol blue (d) Cresol red 6.0 – 7.6 1.2 – 2.8 7.2 – 8.8
Give detailed Solution with explanation (no need Handwritten answer
The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?
In the titration curve below, which species would NOT be in solution at Point B? 14 Unknown Solution K2A %3D 13 12 pH 11 10 9. 8. D 6. 4 --O E 3 F 1 25 50. 75 100. mL of 1.00 M HCI added O CI- O H2A O K+ O A2- O HA
A buffer with a pH of 9.71 is to be prepared from NH3 and NH4Cl. What ratio of base to saltwould you use? KB(NH3)=1.8x10‒5 (give your answer to 3 sig figs)
A 120-mL buffer solution is prepared from 0.90 M HA (K, = 0.00029) and 0.90 M NaA. Calculate the pH after 10.8 mL of 0.23 M NaOH is added to the buffer. answer to two decimal places.
Please don't provide handwritten solution
Bromthymol blue has a Ka value of 1.0 \times 10-7, is yellow in its HIn form and blue in its In form. Suppose we put a few drops of this indicator in a strongly acidic solution. If the solution is then titrated with NaOH, at what pH will the indicator color change first be visible?
You are given a solution of 0.20M CoCl3, 0.15M SnCl2, 0.35M CuCl2, and 0.25M AgCl.Giventhe following table, calculatethe hydroxide concentration needed to precipitate each metal individually so they can be recovered. You do not want more than one metal to precipitate at one time or when you filter the precipitate you will get a mixture.(Optional; calculate the volume of a 0.25M NaOH solution needed to cause this precipitation) b.) Hydroxide needed to precipitate Sn(OH)2 c.) Hydroxide needed to precipitate Cu(OH)2 d.) Hydroxide needed to precipitate AgOH
A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…
Calculate the pH during the titration with NaOH after addition of: a) 50.00 mL of 0.1000 mol L-1 NaOH to 50.00 mL of 0.1000 mol L-1 CH3COOH (Ka= 1.75 x 10-5). b) Based on the table below, which indicator (A, B or C) is most appropriate to monitor this titration? Explain. Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2
A 250.0 mL 0.100 M buffer solution at pH 7.0 is to be prepared. The following reagents are available in the laboratory: 1.0 M H3PO4, 1.0 M NaH2PO4, solid Na2HPO4 (MM = 141.96), and solid Na3PO4 (MM = 163.94). Constants: pKa1 = 2.30, pKa2 = 7.21, pKa3 = 12.10 A. What are the amounts (in M) of the acidic and basic components in the buffer? B. What are the amounts (in g or mL) of the reagents needed to prepare the buffer?