The pH of a 0.10 M solution of a weak acid was determined to be 4.0 once equilibrium was established at 25°C. What would the pH of the same solution be if equilibrium was established at 75°C?                     HA(aq)   ↔   H+(aq)   +   A−(aq)   +   35.5 kJ

Calculate the pH and the pOH of an aqueous solution that is 0.020 M in HCl(aq) and 0.060 M in HBr(aq) at 25 °C. pH = pOH = x10 TOOLS

Assuming the base completely dissociates in water, what is the pH of a 5.20 g/L solution of Ba(OH)2 (aq)? pH:

Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pK, = 4.75) with 0.131 M NaOH. CH;COOH(aq)+NaOH(aq) · CH, COO (aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH : Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =

Swimming pool disinfectants produce hypochlorous acid upon dissolution. The weak acid ionizes as follows:  HClO (aq) ⇄  H+ (aq) + ClO‒ (aq)            Ka=3.0 x 10 ‒8 As strong oxidizing agents, both acid and its conjugate base kill bacteria. However, too high [HClO] is irritating to swimmers’ eyes and too high [ClO‒] will cause the ions to decompose in sunlight. The recommended pH to circumvent both problems is 7.8. Determine the ratio of the weak acid and its conjugate base at this pH.

Part A Water ionizes by the equation =H+(aq) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H*] and [OH ]: What is the H† concentration for an aqueous solution with pOH = 2.73 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H*][OH¯] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. ? [H*] = Value Units

A solution  NaOH(aq)  contains  6.6  g  NaOH(s)  per  100.0  mL of solution. Calculate the pH and the pOH of the solution at  25  °C