A 50.0 mL sample may contain the following compounds, alone or in some combination, along with inert material. If the sample used 12.1 ml of 0.1533 M NAOH in the methyl orange end point, an additional 15.1 mL to reach the phenolphthalein end point, what is the molar concentration of the strong acid in the sample? * HCIO, KH;PO4 H3PO4

A 50.0 mL sample may contain the following compounds, alone or in some combination, along with inert material. If the sample used 12.1 ml of 0.1533 M NAOH in the methyl orange end point, an additional 15.1 mL to reach the phenolphthalein end point, what is the molar concentration of the strong acid in the sample? * HCIO, KH;PO4 H3PO4

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 86E: A solution has a pH of 4.5. What would be the color of the solution if each of the following...

See similar textbooks

Similar questions

A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
A sample may contain NaOH, sodium carbonate and sodium bicarbonate, alone or in compatible combination. Titration of a 50.00 mL aliquot of the sample to a phenolphthalein end point required 8.50 mL of 0.0905 M HCl. A second 50.00 mL aliquot required 22.40 mL of the HCl when titrated to a methyl red end point. Calculate the molar concentration of the base component/s
Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2 CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. A sample of NaOH (sodium hydroxide) contains a small amount of Na2 CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCI. Ar additional 0.700 mL of 0.100 M HCI is required to reach the methyl orange endpoint. What is the percentage of NaCO; by mass in the sample? Express your answer to three significant figures and include the appropriate units.
Calculate the pH of a solution prepared by mixing 1.50 g of imidazole with 1.50 g of imidazole hydrochloride and diluting to 100.0 mL. The pK, of imidazole hydrochloride is 6.993. pH = pH == 6.81 Incorrect Calculate the pH of the solution if 1.70 mL of 1.03 M HCIO, are added. 6,72 Incorrect volume: How many milliliters of 1.03 M HCIO, should be added to 1.50 g of imidazole to give a pH of 6.993? 6.73 Invert Curstinn San ml.
Please answer the following questions regarding the titration curve shown below. 14 12 10 8 PH 4 2 о ° 5 10 15 20 25 30 35 40 45 50 55 60 mL titrant added (a) Choose which of the following is true about the analyte in this titration. It is a monoprotic acid. It is a diprotic acid. It is a triprotic acid. It is a monoprotic base. It is a diprotic base. It is a triprotic base. None of the above. (b) If the titrant has a molarity of 0.1500 M and there are 40.00 mL of analyte present, what is the molarity of the analyte? 0.1500 X M 4.0 (c) If 0.5256 g of analyte were dissolved in 40.00 mL of water to perform this titration, what is the molecular mass of the analyte? 1577 4.0 × g/mol
Question 35 Identify the indicator that has two endpoints. (Refer to Fig. 14.19 in the ebook) 1 phenolphthalein 2 alizarin (3) m-nitrophenol 4 alizarin yellow R 5 phenol red Question 36 -/1 -/1 Calculate the [OH] in a 0.79 M NH2OH solution. Hydroxylamine, NH2OH, is a weak base with a Kb of 1.1 × 10-8 8.7 x 10-9 M 2 4.03 3 9.97 9.3 x 10-5 M
How many moles of B (weak base) would need to be added to 507 mL of 0.28 M BHCl (the acidic salt) to produce a solution with a pH equal to 9.05? Report your answer to the thousandths place. The Kb of the weak base (B) is 4.7 × 10-6 Please explain each step, i want to learn how to solve it myself!
An analytical chemist is titrating 186.4 mL of a 0.3400M solution of methylamine (CH3NH₂) with a 0.6900M solution of HIO3. The pK² of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 98.0 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 1 X Ś
Tryptamine (C10H12N2) is a stimulant found in chocolate. Its molecular structure is shown below. The associated graph shows the % of the basic form of tryptamine as a function of pH. Estimate the pK, of this base. O O O O A 10.2 B 5.0 C 9.0 D 3.8 a=%A 100 75 50 25 HN 8 -NH2 10 11 12 PH Fullsc
An analytical chemist is titrating 211.2 mL of a 0.5700M solution of aniline (C6H5NH₂) with a 0.7200M solution of HNO3. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.1 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 P X S
An analytical chemist is titrating 170.2 mL of a 0.7700M solution of aniline (C H,NH,) with a 0.3200M solution of HIO3. The p K, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 214.4 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. pH = |