1. A chemist, , wishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH3NH2, ánd its salt, CH3NH2, and its salt, CH;NH3CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? K = 5.00 x 10*

1. A chemist, , wishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH3NH2, ánd its salt, CH3NH2, and its salt, CH;NH3CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? K = 5.00 x 10*

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

An analytical chemist is titrating 102.2 mL of a 0.1400 M solution of dimethylamine ((CH,) NH) with a 0.7900 M solution of HNO,. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 19.5 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check 2021 McGraw-Hil Terms of Use
Determine the pH during the titration of 62.0 mL of 0.342 M formic acid (K,- 1.8x104) by 0.342 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 93.0 mL of KOH
Determine the pH during the titration of 59.7 mL of 0.392 M hypochlorous acid (K₂ = 3.5×10-8) by 0.392 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 13.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.6 mL of KOH Submit Show Approach Show Tutor Steps
Be sure to answer all parts. For the titration of 40.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide, determine the pH when: (a) 40.0 mL of base has been added. (b) 60.0 mL of base has been added. (c) 80.0 mL of base has been added.
An analytical chemist is titrating 204.9 ml of a 0.2200M solution of cyanic acid (HCNO) with a 0.7300.M solution of KOH. The pK, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 50.06 ml, of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. DH-0
How many mol of HCI would have to be added to 0.504 L of a 1.416 M B: in order to obtain a buffer with a pH of 9.53? (The Kb for B: is 1.03 10-5). Assume there is no volume change.
a) A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol) b) 10 mL is accidentally spilled into the buffer solution from part a. Determing the new pH of the solution.
6. After adding NH3 (g) to a buffer solution consisting of the conjugate acid/base pair: NH4*/NH3 (without changing the solution volume), which of the following statements is true? K, (NH¼*) = 5.6 x 10 1º. a) The pH of the solution will decrease. b) The concentration of H3O* will increase. c) The concentration of NH4 will increase. d) none of the above
When 35 mL of 0.20 M acetic acid and 35 mL of 0.10 M calcium hydroxide are combined, the pH of the resulting solution will be : ..... A. Less than 7B. Equal to 7C. Greater than 7
1. Calculate the pH changes during the titration of 0.100 M HCl with 50.00 mL of 0.0500 M KOH when the following volumes of the titrant is added: (a) The volume of the titrant required to reach the equivalence point (b) Select five (5) different volumes of the titrant before the equivalence point. (c) At equivalence point (d) Select five (5) different volumes of the titrant after the equivalence point (e) Plot the titration curve using MS Excel Spreadsheet (f) Plot the 1st order and 2nd order titration curve
Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 21.2 mL of 0.109 M HBr by 0.109 M KOH at the following points: (a) Before the addition of any KOH (b) After the addition of 10.6 mL of KOH (c) At the equivalence point (d) After adding 27.3 mL of KOH
How much HCl (in moles) must be added to 1 L of a buffer solution that is 0.84Min ammonia and0.96M in ammonium chloride to result in a buffer solution of pH 8.56? Assume volume to remain constant.