Muscle physiologists study the accumulation of lactic acid [CH₃CH(OH)COOH] during exercise. Food chemists study its occured in sour milk, beer, wine, and fruit. Industrial micro-biologists study its formation by various bacterial species from carbohydrates. A biochemist prepares a lactic acid–lactate bufferby mixing 225 mL of 0.85 M actic acid (Ka=1.38X10⁻⁴) with 435 mL of 0.68 M sodium lactate. What is the buffer pH?

Muscle physiologists study the accumulation of lactic acid [CH₃CH(OH)COOH] during exercise. Food chemists study its occured in sour milk, beer, wine, and fruit. Industrial micro-biologists study its formation by various bacterial species from carbohydrates. A biochemist prepares a lactic acid–lactate bufferby mixing 225 mL of 0.85 M actic acid (Ka=1.38X10⁻⁴) with 435 mL of 0.68 M sodium lactate. What is the buffer pH?

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

Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.112QP

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Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate inmuscles during intense exercise. A chemist prepares a buffer using 225 mL of 0.85 M lactic acid (Ka =1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer?
A buffer consists of 0.50 M NaH₂PO₄ and 0.40 M Na₂HPO₄.Phosphoric acid is a triprotic acid (Kₐ₁=17.2X10⁻³, Kₐ₂=26.3X10⁻⁸, and Kₐ₃=34.2X10⁻¹³). (a) Which Kₐ value is most important to this buffer? (b) What is the buffer pH?
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.223 M CsOH. With 0.00172 moles of C₅H₅NH⁺ and 0.00268 moles of C₅H₅N in the beaker, what would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium? please explain step by step
Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.241 M CsOH. With 0.00151 moles of C₅H₅NH⁺ and 0.00289 moles of C₅H₅N in the beaker, what would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?
What mass (in g) of sodium formate, HCOONA, must be added to 10.0 L of a 0.483 Maqueous solution of HCOOH to produce a buffer solution with a pH of 3.40? Ka (HCOOH) = 1.9 x 10-4 O 84.5 O 14.2 O 3.82 O 1.88 157
You have 150 mL of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric acid is needed to prepare buffer with pH=9.5?
You are asked to prepare a buffer for an experiment. You have access to the following dolutions of acid/base pairs: 1. Propanic Acid (CH3CH2COOH) / Sodium Propanoate (NaCH3CH2COO) with Ka = 1.4 x 10^-5 2. Potassium Hydrogensulfite (KHSO3) / Potassium Sulfite (K2SO3) with Ka = 6.2 x 10^-8 3. Chloroacetic acid (CH2ClCOOH) / Sodium Chlocoacetate (NaCH2ClCOOO) with Ka = 1.4 x 10^-2 Your buffer needs to be at a pH of 4.5. Which acid/base pair do you choose and why? Be very specific!
You want to prepare 100.0 mL of a buffer solution with a pH of 4.95 by mixing appropriate volumes of 0.10 M CH3CO2H and 0.10 M NaCH3CO2. How many milliliters (mL) of the acetic acid and sodium acetate solution are needed? (CH3CO2H has Ka = 1.8 x 10–5) (A) 75.0 mL of 0.10 M CH3CO2H + 25.0 mL of 0.10 M NaCH3CO2; (B) 62.0 mL of 0.10 M CH3CO2H + 38.0 mL of 0.10 M NaCH3CO2; (C) 38.0 mL of 0.10 M CH3CO2H + 62.0 mL of 0.10 M NaCH3CO2; (D) 25.0 mL of 0.10 M CH3CO2H + 75.0 mL of 0.10 M NaCH3CO2;
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 1.09 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) What is the pH of the buffer after 0.750 mol of H⁺ have been added?
50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the solution. Is it a buffer?
A benzoic acid-sodium benzoate buffer is prepared by dissolving a certain amount of sodium benzoate, NaC6H5CO2 (molar mass = 144.1 g/mol) in a 1.25-L of solution that contains 0.025 M benzoic acid, C6H5COOH (Ka = 6.3 x 10-5). How many grams of sodium benzoate must be added so that the resulting solution has a pH of 4.00? (A) 1.82 g (B) 2.84 g (C) 5.71 g (D) 7.14 g

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ISBN:

9781305580343

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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