The acid-dissociation constant for chlorous acid, HClO2, at 25C˚ is 1.0×10-2 . Calculate the concentration of H+ if the initial concentration of acid is 0.100 M

Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)

11.) Acid strength decreases in the series HI > HSO4– > HF > HCN. Place the conjugate bases of these acids inorder of decreasing base strength.

What is the percent ionization of a monoprotic weak acid solution that is 0.113 M? The acid-dissociation (or ionization) constant, Ka, of this acid is 8.93×10−8.

A 0.2000 M solution of hydrofluric acid is only partially ionized. Using measurements of the pH of the solution, [H+] was determined to be 3.184 x 10^-2. Calculate the acid dissociation constant of hydroflouric acid.

Consider a 1.0-L solution that is initially 0.640 M NH3 and 0.610 M NH¼CI at 25 °C. What is the pH of this solution after 0.104 moles of NaOH have been added? The Kb of NH3 is 1.8x10. Enter your response to three significant figures using decimal notation.

The pH of a solution of Ba(OH)2 is 10.95 at 25 °C.

HClO is a weak acid (?a=4.0×10−8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.076 M in NaClO at 25 °C?

The pH of a 0.64M solution of acrylic acid (HC3H₂CO₂) is measured to be 2.22. Calculate the acid dissociation constant K of acrylic acid. Be sure your answer has the correct number of significant digits. a K₁ = 0 Ка 0 ? x10 X Ś

What is the percent ionization of a monoprotic weak acid solution that is 0.124 M? The acid-dissociation (or ionization) constant, Ką, of this acid is 8.93 × 10-8. percent ionization: %