What is the mole ratio of ammonia (with a pкb of 4.75) to ammonium chloride in a buffer with a pH of 9.07 ?

Given: pH = 9.07pKb = 4.75Base = NH3Acid = NH4Cl: The ammonium ion (NH4+) in NH4Cl is the conjugate…

Answered: What is the mole ratio of ammonia (with…

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 11QAP: A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M...

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The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
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.
What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?
What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pKa of the acid is 5.7. How many grams of ammonium sulfate ((NH4 )2SO4 )) would you need to add to 425 mL of 0.28 M ammonia (NH3 ) to obtain a buffer solution with a pH of 9.45. Assume that the volume doesn’t change when you add the salt. Ka for the ammonium ion is 5.8 x 10-10 . (be careful with how the reaction for ammonium is written as well as stoichiometry) A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 M formic acid (HCOOH). (Ka of HCOOH is 1.8 x 10-4 ) a. Calculate the initial pH of this buffer. b. What is the pH after the addition of 0.0050 mol HCl? c. How about after the addition of 0.0050 mol NaOH? [For parts b and c, assume that volume doesn’t change in the addition process and that neutralization proceeds to completion]
The pKa of acetic acid, HC2H3O2, is 4.74. What is the pH of a buffer in which [HC2H3O2] = 0.20 M and [NaC2H3O2] = 0.20 M?
What ratio of concentrations of NaH2PO4 and Na2HPO4 in solution would give a buffer with pH = 7.65?
What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate base? The pKa for the acid is 5.53.
a)What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4? (b) If 1.0 mL of 10.0 M NaOH is added to a liter of the buffer prepared in (a),how much will the pH change? (c) If 1.0 mL of 10.0 M NaOH is added to a liter of pure water at pH 7.0, whatis the final pH? Compare this with the answer in (b).
A chemist has synthesized a monoprotic weak acid and wants to determine its pKa value. To do so, they dissolved 2.00 mmol of the solid acid in 100.0 mL of water and then titrated the resulting solution with 0.0500 M NaOH. After20.0 mL of added NaOH, the pH of the solution was 6.00. What is the pKa of the acid?(a) 5.85 (b) 7.02 (c) 9.90 (d) 6.00
A chemistry graduate student is given 100. mL of a 0.90M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 104. f (CH3)2NHCl should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 10.66? mass of You may assume that the volume of the solution doesn't change when the (CH3)2NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0x12 What X S ? EFET ol Ar
The pOH of an acidic buffer is 9.725. What is the Ka of the acid if the ratio of [ionized] to [unionized] is 1380?

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