A diprotic acid (H₂A) has pKa values of 4.20 (pKal) and 8.40 (pKa2). Which of the equalities is true when the pH is 4.20? [HA] = [A²-] [H₂A] = [A²-] O [H₂A] = [HA] What is the predominant species of H₂A at pH 2.52? HA H₂A OA²- What is the predominant species of H₂A at pH 10.50? HA™ Which of the equalities is true when the pH is 8.40? [H₂A] = [HA] [HA] = [A²-] O [H₂A] = [A²-] What is the predominant species of H₂A at pH 7.01? A²- H₂A HA™

Which of the following statements is true? A. A weak acid solution can be diluted with enough water to produce a solution with a pH greater than 7.00 at 25°C. B. Diluting a weak acid solution by a factor of ten will always decrease its pKa by 1. C. A weak base solution will always have a lower concentration of OH‒ than a strong base solution. D. A weak base solution will always have a pH of 7.00 or greater at 25°C.   D. Correct   Why is C false and not true??

Common aspirin is acetylsalicylic acid, which has the structure shown below and a pka of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin (6.5 mg x102) mg is dissolved in 8 ounces of water. -H H H

A monoprotic weak acid (HA) has a pKa value of 4.896. Calculate the fraction of HA in each of its forms (HA, A¯) at pH 6.262. 28.34 x10 -8 2.834 x10 AHA = dA- = What is the quotient [A] at pH 6.262? [HA] [A*] [HA] 21.17

Oxalic acid (HOOC-COOH) is the simplest diprotic carboxylic acid. Its commercial uses include bleaching straw and leather and removing rust and ink stains. Calculate the equilibrium values of [H2C2O4], [HC2O4- ], and [C2O42- ], and find the pH of a 0.150M H2C2O4 solution using Ka values from appendix C in your textbook.

The unstable weak acid 2-germaacetic acid (GeH3COOH) is derived structurally from acetic acid (CH3COOH) by having a germanium atom replace one of the carbon atoms. At 25°C, a 0.050 M solution of 2-germaacetic acid has a pH of 2.42. Compute the K1 of 2-germaacetic acidand compare it with that of acetic acid.

A 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic acid.

What is the pH of a solution that is 0.200 M ammonia (NH3) and 0.150 M ammonium chloride (NH4Cl)?  The Kb of NH3 is 1.8 × 10-5   Part D:  What is the pKa of NH4+? Report your answer to two digits past the decimal.

A 0.200 M solution of diethylamine, a substance used in insecticides and fungicides, is only 3.9% ionized at 25°C. Calculate the pKb of diethylamine and the pKa of its conjugate acid, the diethylammonium ion. Round to two decimal places.   pKb = ? pKa = ?

A 2.00 L aqueous solution of a monoprotic weak acid, HA, with a concentration of 0.750 M has a pH of 1.90 at 65 °C. Calculate the [H3O+], [OH-], Ka value and pKa of the acid at equilibrium.