1. Which of the following species will form a buffer? For the one(s) that is/are not buffers,state why they do not fit that mold. For the solution(s) that is/are buffers, find the pH.(a) 0.350 M perchloric acid with 0.300 M potassium perchlorate(b) 0.200 M hydrosulfuric acid with 0.0001 M sodium sulfite(c) 0.750 M phosphoric acid with 0.400 M lithium phosphate(d) 0.750 M phosphoric acid with 0.400 M lithium dihydrogen phosphate

What is a buffer?A buffer solution contains a weak acid and its conjugate base or a weak base and…

Answered: 1. Which of the following species will…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 14QAP: A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to...

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An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
You are required to prepare a buffer (pH sodium propionate. The concentration of the propionate must the concentration of the acid be? K, = 1.3 × 105 5.30) using propionic acid and 0.6M. Which one
You are asked to prepare a pH = 3.00 buffer solution startingfrom 1.25 L of a 1.00 M solution of hydrofluoric acid(HF) and any amount you need of sodium fluoride (NaF).(a) What is the pH of the hydrofluoric acid solution priorto adding sodium fluoride? (b) How many grams of sodiumfluoride should be added to prepare the buffer solution?Neglect the small volume change that occurs when the sodiumfluoride is added.
A 250.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate. (a) What is the initial pH of this solution? (b) What would you expect to happen to the pH if 0.0050 mol of HCl were added the buffer from part (a)? Explain your answer. Explain your answer in terms of acetic acid and sodium acetate. (c) What would you expect to happen to the pH if 0.0050 mol of NaOH were added the buffer from part (a)? Explain your answer in terms of acetic acid and sodium acetate.
The drawing below represents a buffer composed of equal concentrations of a weak acid, HX, and its conjugate base, X-'. The heights of the columns are proportional to the concentrations of the components of the buffer. (a) Which of the three drawing (1), (2), or (3) represents the buffer after the addition of a strong acid? Explain. (b) Which of the three represents the buffer after the addition of a strong base? Explain. HX X HX X- HX X HX X (1) (2) (3) Copyright © 2006 Pearson Prentice Hall, Inc.
To fill a 500 mL volumetric flask, 40 g of ammonium chloride (NH4Cl) and 3.2 g of ammonia (NH3) are added along with water. Given the Kb of NH3 is 1.8 × 10−5, the pH of this buffer is...
A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x 104) and 1.00M potassium fluoride, KF. The total volume was 250 mL. (a) What ions and molecules are present in the solution? List them in order of decreasing concentration: Decreasing order of Concentration (b) What is the pH of the buffer solution described above? (c) What is the pH of 100. mL of the buffer solution if you add 100. x 10-3 g of NaOH? Assume negligible change in volume. (USEFUL INFORMATION: MM NaOH = 39.997 g mol-1)
A buffer solution contains 0.345 M NAHSO3 and 0.436 M Na,SO3. If 0.0273 moles of perchloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding perchloric acid) pH =

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