H8. +(a)A laboratory technician dissolved 6.797 g of compound W (a non-electrolyte) in 15.00 mL ofethylene glycol in a boiling tube and heated the sample. If the boiling point of the mixture wasfound to be 201.4 °C, what is the molar mass of W?(b)A buffer is prepared by adding together 600 mL of 1.64 M hydrocyanic acid and 850 mL of0.98 M sodium cyanide. Given that the new pH of the buffer is 9.01 after 25 mL of sulfuric acidis added, calculate the concentration of the sulfuric acid.

The elevation in boiling point on addition of non-electrolyte to a pure liquid is a colligative…

A laboratory technician dissolved 6.797 g of compound W (a non-electrolyte) in 15.00 mL of ethylene glycol in a boiling tube and heated the sample. If the boiling point of the mixture was found to be 201.4 °C, what is the molar mass of W? A buffer is prepared by adding together 600 mL of 1.64 M hydrocyanic acid and 850 mL of 0.98 M sodium cyanide. Given that the new pH of the buffer is 9.01 after 25 mL of sulfuric acid is added, calculate the concentration of the sulfuric acid.

A laboratory technician dissolved 6.797 g of compound W (a non-electrolyte) in 15.00 mL of ethylene glycol in a boiling tube and heated the sample. If the boiling point of the mixture was found to be 201.4 °C, what is the molar mass of W? A buffer is prepared by adding together 600 mL of 1.64 M hydrocyanic acid and 850 mL of 0.98 M sodium cyanide. Given that the new pH of the buffer is 9.01 after 25 mL of sulfuric acid is added, calculate the concentration of the sulfuric acid.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 54QAP: Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a...

See similar textbooks

Similar questions

Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
11 (a) Define a buffer solution (b) What are the components of (1) an acidic buffer 2 (ii) a basic buffer ? (b) Using the equation below, explain what happens to maintain the pH of the solution: + A C Hw HA (9) when an acid is added (1) when a base is added (ii) (iii) Give one example each of a buffer in both living and non-living systems
A buffer is prepared by mixing 204 mL of 0.452 M HCl and0.500 L of 0.400 M sodium acetate. (a) What is the pH? (b) How many grams of KOH must be addedto 0.500 L of the buffer to change the pH by 0.15 units?
The following diagram represents a buffer composed ofequal concentrations of a weak acid, HA, and its conjugatebase, A-. The heights of the columns are proportionalto the concentrations of the components of the buffer.(a) Which of the three drawings, (1), (2), or (3), representsthe buffer after the addition of a strong acid? (b) Which ofthe three represents the buffer after the addition of a strongbase? (c) Which of the three represents a situation thatcannot arise from the addition of either an acid or a base?
Determine the pH during the titration of 58.3 mL of 0.310 M acetic acid (K, 1.8x10) by 0.310 M NaOH at the following points. (Assume the titration is done at 25 °C. (a) Before the addition of any NaOH 2.63 (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 87.5 mL of NaOH
Which of the following combination of solutions will form a buffer solution? (A) 50.0 mL of 0.20 M NH3 + 50.0 mL of 0.10 M HCl; (B) 50.0 mL of 0.20 M NH3 + 50.0 mL of 0.10 M NaOH; (C) 50.0 mL of 0.20 M HCl + 50.0 mL of 0.10 M NH3; (D) 50.0 mL of 0.20 M NaOH + 50.0 mL of 0.10 M HCl.
A buffer contains 0.15 mol of propionic acid (C2H5COOH)and 0.10 mol of sodium propionate (C2H5COONa) in 1.20 L.(a) What is the pH of this buffer? (b) What is the pH of thebuffer after the addition of 0.01 mol of NaOH? (c) What isthe pH of the buffer after the addition of 0.01 mol of HI?
Does the pH increase or decrease, and does it do so to a largeor small extent, with each of the following additions?(a) 5 drops of 0.1 M NaOH to 100 mL of 0.5 M acetate buffer(b) 5 drops of 0.1 M HCl to 100 mL of 0.5 M acetate buffer(c) 5 drops of 0.1 MNaOH to 100 mL of 0.5 MHCl(d) 5 drops of 0.1 MNaOH to distilled water
(a) Calculate the pH of a solution that is 0.50 M acetic acid and 0.91 M sodium acetate. (b) How would you prepare 250.0 mL of this buffer solution if you have a stock solution of 3.0 M acetic acid and another stock solution of 1.5 M sodium acetate?
Acetic acid and a salt containing its conjugate base, such as sodium acetate, form buffer solutions that are effective in the pH range 3.7-5.7. (a) In resisting a pH change, which buffer component would react with NaOH? Explain. (b) What happens to the buffer activity when this component is exhausted?
11 (a) Define a buffer solution (b) What are the components of (i) an acidic buffer ? (ii) a basic buffer ?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS