Lactic acid, HC3H5O3 , is a weak acid in aqueous solution, Ka = 1.4 × 10−4 .
Calculate Kb for the lactate ion, C3H5O –
The product of Ka and Kb gives us the dissociation constant for water which is 1 x 10-7.
⇒ Ka x Kb = Kw = 1 x 10-7
Here, Ka = 1.4 × 10−4
⇒ Kb = 1 x 10-7 / 1.4 × 10−4 = 0.7143 x 10-3 = 7.143 x 10-4
Lactic acid, HC3H5O3 , is a weak acid in aqueous solution, Ka = 1.4 × 10−4...
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)
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
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. Consider the following equilibrium for the dissociation of lactic acid, HC3H5O3 (a weak acid): HC3H5O3 (aq) + H2O (l) → H3O+ (aq) + C3H5O3- (aq) If the Ka of lactic acid is 1.40E-4, calculate the value of ΔGo (in kJ/mole) for this reaction at 25.0oC.
Problem 15.50 The equilibrium constant Kn for the neutralization of lactic acid (HC3H5O3) and urea (CH4N2O) is 2.1�10?4. Part A What is Kb for urea? Ka of lactic acid is 1.4�10?4. Express your answer using two significant figures. Kb =
Lactic acid is found in muscles after exercising and has a Ka = 1.4 x 10-4. A 350.0 mL solution contains 0.060 moles of lactic acid and 0.040 moles of sodium lactate. What is the pH of the solution after the addition of 0.015 moles of HNO3?
A lactic acid solution is prepared by dissolving 0.67 g of lactic acid (HC3H5O3) in 100.00 mL of water. The pH is found to be 2.50. Calculate the Ka for lactic acid.
A lactic acid/lactate ion buffer solution contains 0.43 MHC3H5 03 and 0.80 MC,H50,-, respectively. The Ka value of lactic acid is 1.4 × 10-4. Calculate the pH of this buffer. Express the pH numerically.
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...
12. Lactic acid (HC3H5O3) is present in sour milk It is a monoprotic acid. In a 0.100 M solution of lactic acid, the pH is 2.44 at 25°C. Calculate Ka and pKa for lactic acid at that temperature. (10)