At 25°C, what are the molar H3O+ and OH- concentrations in 0.0300 M HOCl? 0.0600 M butanoic acid? 0.100 M ethylamine?

At 25 °C,25 °C, how many dissociated H+H+ ions are there in 343 mL343 mL of an aqueous solution whose pH is 11.41?

A 1.00 M solution of acetic acid, CH 3COOH has a [H 30 *] = 4.2 x 10 3 M. What is the percent dissociation?

What is [H+] in a 0.270 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10-5)?

Calculate the pH, pOH, and the fraction of protonated acid for the 0.1 M solution of lactic acid (see Table 4.4 for pk3 values, also attached below).

What is the pH of 0.075 M methylammonium bromide, CH3NH3Br?  (Kb of CH3NH2 = 4.4 × 10−4.)

Determine the |H*, pH, and pOH of a solution with an OH- of 8.5 x 10-13 M at 25 °C. [H*] = M pH = РОН

Study the chemical equations that show how each substance behaves when dissolved in water. Then classify each substance as a Brønsted-Lowry acid, Brønsted-Lowry base, or as neither an acid nor a base. Substance Behavior in water (CH, ),NH (CH, ),NH + H,0= OH + (CH,),NH; СаCl, + H,0 — Н,О + Са2+ + 2CI- HF + H,O = H,0* +F CaCl, HF CH, COOH + H,O=H,0* + CH,C0 co, + H,0 =OH¯ + HCO, CH, COOH co? NH NH + H,0 NH; + H;O* Brønsted-Lowry acid Brønsted-Lowry base Neither an acid nor a base Answer Bank CaCl, co3- (CH,),NH CH;COOH NH† HF

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 {}.)

What is the pOH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?