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Draw a titration curve for the reaction of CH3NH2 with HCL.

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 125CP: Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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Draw a titration curve for the reaction of CH3NH2 with HCL.

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The pH of a buffer solution containing 0.5 mole/litre of CH3COOH and 0.5 mole/litre CH3COONa has been found to be 4.76. What will be the pH of this solution after 0.1 mole/litre HCl has been added to the buffer? Assume that the volume is unchanged. Ka = 1.75 × 10– 5
25) Which of the following reagents would NOT make an effective buffer solution? HNO2 and LiNO2 H3PO4 and NaH2PO4 HNO3 and NaNO3 HC2H3O2 and KC2H3O2
If an identical titration is performed with the strong acid HCl, explain why the pH at the equivalence point would be neutral in the case of the HCl titration but not in that of CH3COOH. In order to support the explanations, quote the hypothetical value obtained for the titration of CH3COOH ([CH3COOH] = 0.1082 mol/L at equilibrium) and identify the species present at the equivalence point for the 2 acids.
explain each of the following cases. a) when we treat 1 mol / liter of hydrochloric acid, the pH increases. There comes a cast that the pH reaches a certain value and does not change anymore. Why does this happen? b) Methyl orange can be used to determine the final titration point of nitric acid with ammonia solution, while phenophthalein is not used in this case. Why? c) pH of 10-8 mol / l HCl is not 8. Why?
Write the formula for a reagent that dissolves SnS2, but not SnCl-2
Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to prepare buffered solutions. Calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500.0 mL of a pH = 6.60 buffer so that the buffer has a total of arsenic-containing species equal to 0.25 M, that is, so that: [(CH3)2AsO2H] + [(CH3)2AsO2] = 0.25 M
What is the pH of a solution containing 0.50 moles of benzoic acid and 0.75 moles of sodium benzoate if the pka is 4.19?
Ideal NaOH titrant preparation requires boiling the solvent H2O. Why
A 100.0-mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 M NaOH. What is the value of α2 at the second equivalence point? 99.6×10−2 3.45×10−3 2.87×10−4 3.46×10−11 1.20×10−9
An analytical chemist is titrating 198.6 mL of a 0.7200M solution of formic acid (H₂CO₂) with a 0.7700M solution of KOH. The p K of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 209.6 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.
3. A sample may contain NaOH, NaHCO3 and Na2CO3, alone or in some combination along with inert material. A 567.8 mg sample was dissolved and titrated with 0.1503 M HCl 23.14 mL of HCl was used to reach the phenolphthalein endpoint and an additional 16.90 mL to reach the methyl red end point. a) What are the composition of the sample? b) Calculate the percentage of each titrated component.
A student needs to prepare a buffer made from CH3COOH and CH 3 COOK with pH 4.360. If Ka for CH3COOH is 1.80 × 10-5, what ratio of [CH3COOH] is required? [CH3COO] [CH3COOH] [CH3COO-]