What is the pH of a solution containing 0.16 mol L-1 of HCI and 0.828 mol L-1 of a weak acid with PKA = 4.63? Report your answer to at least 1 decimal place. Answer: What is the pH at which a buffer composed of HF and F" would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15.

What is the pH of a solution containing 0.16 mol L-1 of HCI and 0.828 mol L-1 of a weak acid with PKA = 4.63? Report your answer to at least 1 decimal place. Answer: What is the pH at which a buffer composed of HF and F" would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15.

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...

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A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
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.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
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?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
If a buffer solution contains 2.1 M acetic acid and 2.7 M sodium acetate, what is the pH of the buffer if the K, of the acetic acid is 1.8 x 10-5. Round to 2 decimal places. Your Answer: Answer
Which combination can be used to make a buffer with a pH of 4.2? The K, of benzoic acid, C6H5COOH, is 6.5×10-5 and the Ka of hydrocyanic acid, HCN, is 4.9x10-10. Item equation/constant: A pH=pK, +log НА Select one: O a. 50.0 mL of 0.500 M HCN and 50.0 mL of 0.500 M sodium hydroxide. O b. 50.0 mL of 0.500 M C6H;COOH and 25.0 mL of 0.500 M sodium hydroxide. O c. 50.0 mL of 0.500 M C H5COOH and 50.0 mL of 0.500 M sodium hydroxide. O d. 50.0 mL of 0.500 M HCN and 25.0 mL of 0.500 M sodium hydroxide.
A buffer solution contains 1.7 M acetic acid and 2.6 M sodium acetate. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution if 0.11 mol of NaOH is added to 1.00 L of the solution? (Assume there is no volume change.) Round to 2 decimal places. Your Answer: Answer