The pH of an acidic buffer solution is given by pH = pKa+ log(conjugate base/ weak acid)
The pH of an acidic buffer solution in this case is given by pH = pKa+ log(sodium lactate/ lactic acid)
The pH of the given buffer solution = -log(1.4*10^-4) + log(0.10/0.12) = 3.77
What is the pH of a buffer that is 0.12 M in lactic acid (HC3H503) and 0.10 m in sodium lactate? For lactic acid, K...
2. (a) Determine the pH of 0.10 M lactic acid (HC3HSO3) (b) What is the pH of a buffer that is 0.12 M. lactic acid and 0.10 M sodium lactate (NaC3H5O3)? For lactic acid. Ka = 1.4 x 10-4. (10)
10. (a) Determine the pH of 0.10 M lactic acid (HC3H5O3) (b) What is the pH of a buffer that is 0.12 M lactic acid and 0.10 M sodium lactate (NaC2H5O3)? For lactic acid. Ka - 1.4 x 104. (10) 11. Hydrazine, N2H4, is a weak base. Write the equation for the reaction of hydrazine with water and write the expression for Kb. (5) Na Hj
1. What is the pH of a buffer mixture composed of 0.12-M lactic acid (HCsHs0, K, 14 x 10) and 0.10-M sodium lactate (NaCsHsOs) Can be solved via ICE diagram or by Henderson-Hasselbalch ] Initial - Change Equilibrium a) Solved directly from the equation b) Using the Henderson-Hasselbalch Equation 2. Preparing a buffer. How many moles of (solid) NH&CI must be added to 1.0-L of 0.10-M NHs to form a buffer whose pH is 9.00? [The Kb 1.8x 10s for...
10Consider a buffer prepared by mixing 15 mL of a .300 M lactic acid (Ka= 1.4x10^-4) and 15 mL of .300 M potassium lactate. Calculate the pH. 2) Calculate the pH of a buffer when 15mL of a 0.150 M sodium hydroxide is mixed with 15 mL of a .300 M lactic acid
5. Calculate the pH of buffer formed by mixing 85 mL of 0.12 M lactic acid with 95 mL of 0.16 M sodium lactate (K, for lactic acid is 1.4 x 10-) a. 3.77 b) 4.03 ) 3.56 d) 4.23 e) 3.66 6. 18 2.5mL of 0.30M AgNO3 is mixed with 7.5mL of 0.015M Na2SO4, should a precipitate of Ag2SO4 form? (Ksp - 1.2x10-5 a) Q - Ksp the system is at equilibrium and the solution is saturated b) Q<Ksp,...
A buffer made with 100.00 mL of 0.95 M lactic acid (Ka=1.4x10-4) and 200.00 mL of 0.50 M lactate has a final volume of 1.0 L. What is the pH of this buffer?
3. What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.14 M in sodium lactate? The K, of lactic acid is 1.68 x 10-4.
Calculate the percent ionization of 0.115 M lactic acid in a solution containing 7.5×10^-3 M sodium lactate. Ka of lactic acid=1.4x10^-4
A buffer contains 0.010 mol of lactic acid and 0.050 mol of sodium lactate per liter. (a) calculate the pH of the buffer. (b) calculate the pH when 100ml of 0.02 M NaOH is added to 500mL of the buffer. (c) What pH would you expect if you added the same quantity of NaOH to 500mL of pure water?
Lactic acid is a simple organic acid that is somewhat stronger than acetic acid. The lactate ion is the conjugate base of lactic acid and is one product of animal (including human) metabolism. Ka for lactic acid is 1.38 x 10-4. If the resting amount of lactate in blood is 2.0 mM and typical blood pH is 7.40, what is the lactic acid concentration in blood? Calculate the pH of a 0.0100 M solution of lactic acid. Calculate the pH...