10. (a) Determine the pH of 0.10 M lactic acid (HC3H5O3) (b) What is the pH...
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)
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, Ka= 1.4x10-4 a 3.77 6.3.85 OC 10.33 d. 1.20
Lactic acid, HC3H5O3 , is a weak acid in aqueous solution, Ka = 1.4 × 10−4 . Calculate Kb for the lactate ion, C3H5O –
A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H5O3-) are both 0.600 M. What is the resulting pH if 10.0 mL of 1.00 M HCL is added to 0.500 of the buffer solution? (ka of HC3H5O3= 1.4 x 10^-4)
Lactic acid, HC3H5O3, is a substance found in sour milk products such as yogurt, and is produced naturally by fermentation in body cells during normal metabolism and exercise The Ka for lactic acid is 38 x 10-4. Its sodium salt, sodium lactate, NaC3H5O3, is used in foods as a preservative and acidity regulator. It is also used in shampoo products as an effective humectant and moisturizer. Determine the pH of a solution prepared by adding 4.5 grams of sodium lactate...
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...
11a) 1.00 moles of lactic acid (HC3H5O3, Ka = 1.4 x 10-4) and 1.00 moles of sodium lactate (NaC3H5O3) are dissolved in water resulting in a solution with a final volume of 550 mL. What is the pH of the solution after the addition of 0.080 moles of HCI? a. 0.80 b. 1.8 C. 2.8 d. 3.8
A buffer is prepared by adding 0.15 mol of lactic acid, CH3CHOHCOOH, and 0.20 mol of sodium lactate, Na+CH3CHOHCOO - , to sufficient water to make 1.0 L of buffer solution. The Ka of lactic acid is 1.4 x 10 - 4. Calculate the pH of the buffer.
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
What is the pH of a 1.00 L solution containing 0.295 M lactic acid, HC3H5O3 (pKa = 3.86) and 0.295 M sodium lactate, NaC3H5O3, upon the addition of 0.055 mol HCl? Assume no significant volume change occurs.