None 2. What is the pH of a buffer that is 1.0 M in tris (hydroxymethyl) aminomethanehydrochloride in 1.0 M tris (hydroxymethyl) aminomethane, (pKa of trishydrochloride = 8.072)?NHNH₂A. 8.072B. 7.372CHOCH,"HOCH+ HC. 7.777CH₂OHCH₂OHHOCH2HOCHD. 9.377BHB="tris"PK = 8.075Tris(hydroxymethy Daminomethane

Answered: 2. What is the pH of a buffer that is…

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 26QAP: You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio...

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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?
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.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
A buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium formate, NaCHO2. Calculate the pH. What would be the pH of 85 mL of the buffer to which 8.6 mL of 0.15 M hydrochloric acid had been added?
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.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
A chemistry graduate student is given 100. mL of a 1.80M trimethylamine ((CH N solution. Trimethylamine is a weak base with K,=7.4 x 10 *. What (CH3), NHC1 should the student dissolve in the (CH3),N solution to turn it into a buffer with pH =10.99? mass of You may assume that the volume of the solution doesn't change when the (CH, NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
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
What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.23 M C6H5COOH and 0.47 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. *Can you explain how the molarity of the sodium acetate equals the molarity of the acetate ion?
A chemistry graduate student is given 500. mL of a 1.50M trimethylamine ((CH,) N solution. Trimethylamine is a weak base with K,=7.4 ×10 mass of (CH,) NHCI should the student dissolve in the (CH,) N solution to turn it into a buffer with pH =11.39? You may assume that the volume of the solution doesn't change when the (CH,) NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 10
Be sure to answer all parts. Tris [tris(hydroxymethyl)aminomethane] is a common buffer for studying biological systems. (K = 5.01 × 10 and pK = 8.3) (a) Calculate the pH of the Tris buffer after mixing 11.0 mL of 0.20 M HCl solution with 25.0 mL of 0.10 M Tris. (b) This buffer was used to study an enzyme-catalyzed reaction. As a result of the reaction, 0.00019 mol of H* was produced. What is the pH of the buffer at the end of the reaction? (c) What would be the final pH if no buffer were present?
A chemistry graduate student is given 300, ml of a 0.80M trimethylamine ((CH,) N) solution. Trimethylamine is a weak base with K,-7.4 x 10. What mass of (CH, NHCI should the student dissolve in the (CH)N solution to turn it into a buffer with pH 11.45? You may assume that the volume of the solution doesn't change when the (CH, NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

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