The pH of a 0.131 M solution of a weak acid, HA, has been measured (pH = 5.37). Using this information, calculate the acid dissociation constant, Ka of HA? Present your answer in the form x.xE±x Hint: Write a balanced chemical equation for the dissociation of the acid and consider the relative amounts of products and reactants expected from the stoichiometry.
D Question 28 1 pts A buffer consists of 0.150 M acid, HA, and 0.200 M of its conjugate base, A". HA has a K, of 4.84x 10?, what is the pH after adding 0.068 moles of HNO3 to 1.00L of the solution? Assume the addition of HNO3 does not impact the volume Remember that only the decimal places in a pH represent significant figures. Enter your pH with three decimal places
An acid HA has a Ka of 10-7. The pH of a 0.1 M solution of its conjugate base is: options: 7 5 10 13
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...
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, Ka? Answer in scientific notation. Answer: A...
1) A 0.224 M solution of a weak acid (HA) is made. The Ka for this acid is 7.73 ⋅ 10-5 . -What is the pH of this solution? -What is the pOH of this solution? 2)A 0.238 M solution of a weak base (B:) is made. The Kb for this acid is 7.34⋅10-3. -What is the pOH of this solution? -What is the pH of this solution?
Question 1 5 pts If 27.2 mL of 0.102 M acid with a pKg of 5.44 is titrated with 0.1 M NaOH solution, what is the pH of the titration mixture after 11.3 mL of base solution is added? 5 pts Question 2 If 20.7 mL of 0. 102 M acid with a pKa 4.33 is titrated with 0.107 M NAOH solution, what is the pH of the acid solution before any base solution is added? Question 3 5 pts...
What is the pH of a 6.85 × 10−3 M weak acid solution, HA, if Ka = 4.5 × 10−6? Group of answer choices 1.2 4.8 9.1 3.8 6.5 What is the pOH of 4.50 × 10−4M HBr? Group of answer choices 10.7 6.7 1.7 12.3 3.3 What is the pH of a 9.67 × 10−3M solution of NaOH? Group of answer choices 13.0 4.6 12.0 9.4 2.0 A 6.5 × 10-2 M solution of a weak acid, HA, has...
A 0.013 M solution of a weak acid (HA) has a pH of 4.38. What is the K, of the acid? Ka = 10 (Enter your answer in scientific notation.)
A 0.200 M solution of an acid, HA, has a pH = 3.1. What is the value of the ionization constant, Ka, for this acid?