EXERCISE II -111. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine,CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to saltto obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methylammonium chloride should he add to get the desired pH ? Kp = 5.00 x 1042. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite,NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of thesolution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104%3D3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL ofa buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC?Assume no change in volume.

Since you have posted multiple questions, we are entitled to answer the first only. 1) Given: Volume…

A chemist,, Wishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH3NH2, and its salt, CH3NH;CI. (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 ? Kp = 5.00 x 104 %3D

A chemist,, Wishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH3NH2, and its salt, CH3NH;CI. (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 ? Kp = 5.00 x 104 %3D

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...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

EXERCISE II -11
1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine,
CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (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 ? Kp = 5.00 x 104
2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite,
NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the
solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0
mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104
%3D
3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of
a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC?
Assume no change in volume.

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so Please don't provide handwritten solution,
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