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Water ionizes by the equation H₂O(1) ⇒ H+ (aq) + OH-(aq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH-]: Kw = [H+][OH-] Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. Part A What is the H+ concentration for an aqueous solution with pOH = 4.05 at 25 °C? Express your answer to two significant figures and include the appropriate units. View Available Hint(s) ▶ O μA ? [H+] = Value Units Submit
Water ionizes by the equation H₂O(1) H+ (aq) + OH¯(aq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH-]: Kw = [H+][OH-] Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. Part B Arrange the following aqueous solutions, all at 25 °C, in order of decreasing acidity. Rank from most acidic to most basic. To rank items as equivalent, overlap them. ▸ View Available Hint(s) Reset Help 0.0023 M HCI 0.0018 M KOH pH = 5.45 Most acidic O The correct ranking cannot be determined. pOH = 8.55 Most basic
Water ionizes by the equation H₂O(1) ⇒ H+ (aq) + OH¯(aq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH-]: Kw = [H+][OH-] Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. Most acidic Most basic The correct ranking cannot be determined. Part C At a certain temperature, the pH of a neutral solution is 7.54. What is the value of Kw at that temperature? Express your answer numerically using two significant figures. ► View Available Hint(s) 15| ΑΣΦ ? Submit Kw =