your answer a and b both are right if you want answer of a and b pls comment in comment box.
3. Answer the following questions about the general weak acid, HA (aq): a. Calculate the percent dissociation of 0.500 M HA if the K, value of HA is 6.88 x 106 b. If the percent dissociation of 0.100 M solution of HA is 3.59%, calculate the K value for HA. c. If the pH of a 0.0100 M solution of HA is 4.55, calculate the K value of HA. NOTE: The acid, HA in parts a, b, and c, is...
K.- b. Calculate the K, value of a 0.060 M solution of a monoprotic acid with (H) - 27 x 10" M. K,
24. (25 points) A buffer solution was prepared by dissolving 0.500 mol formic acid and 0.060 mol sodium formate in enough water to make 1 L of solution, K, for formic acid is 1.80 x 104 a) Calculate the pH of the solution. b) If this solution was diluted to 10 times its volume, what would be the pH.
A) the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.2×10−3 is 1.89. Find the percent dissociation of this solution. B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.13. Find the percent dissociation of this solution.
A. What is the pH of an aqueous solution with a hydrogen ion concentration of H] = 8.8 x 10-'M? pH = B. What is the hydroxide ion concentration, (OH), in an aqueous solution with a hydrogen ion concentration of [H+] = 8.8 x 10-'M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) =H(aq) + (aq) The equilibrium concentrations of the reactants and products are [HA] = 0.300 M, H+] = 4.00...
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+ (aq) + A (aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, K ? Answer in scientific...
Using Henderson-Hasselbalch equation, Calculate the pH of a buffer solution that is 0.060 M formic acid (HCHO) and 0.150 M potassium formate (KCHO2). Remember that Kg = 1.8 X 10-4 for formic acid. O 1.45 O 2.36 09.12 4.13 O 0.0125 7.00
7. If H,PO, has K, -6.83 x 10, and Hco, has K,-5.8x 10", which is the weaker acid? Circle your answer and explain how you know. (Ipt 8. For a solution with pH 9.74, calculate the following: (3pa) [H'] [OH] pOH- 9. (2pas total) a. A solution of a weak acid with concentration 0.11 M. is 8.8 % ionized. Calculate its K, value. K, b. Calculate the K, value of a 0.060 M solution of a monoprotic acid with [H']...
Using Henderson-Hasselbalch equation, Calculate the pH of a buffer solution that is 0.060 M formic acid (HCHO2) and 0.150 M potassium formate (KCHO2). Remember that Ka = 1.8 X 10-4 for formic acid. Group of answer choices A 1.45 B 2.36 C.9.12 D.4.13 E. 0.0125 F. 7.00
please help. 1. (3 polnts) A 0.0730 M solution of a monoprotic acid is 1.07 % ionized. What is the pH of the solution? a. b. Calculate the K, of the acid. 2. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? 3. (2 points) Determine the percent ionization of a 0.0028 M HA solution. (K, of HA 1.4 x 10") 4. (4 points) Lysine is...