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11 Nov 2019
K = [H^+][OH^-]/[H_2 O] or K[H_2 0] = [H^+][OH^-] [H^+][OH^-] is known as the ion-product constant for water or K_w . It's possible to calculate K_w using Gibbs Free Energy concepts, but for now know that the equilibrium constant for water K_w = 1 times 10^-14 mol^2/dm^2. (Brackets around a molecular formula denote molarity or concentration in solution) Show how pure water has a pH of 7 using the definition of the log and K_w. One caveat: Recall from class that transcendental functions (logs, exponents, trig functions) must not have any units in their argument. How do you manage this in your calculation? A solution has a pH of 6.8. The number of H+ ions is doubled. What is the resultant pH? A solution has a pH of 4. What is the pOH? (Let pOH be defined as pOH = -log (a_OH-))
K = [H^+][OH^-]/[H_2 O] or K[H_2 0] = [H^+][OH^-] [H^+][OH^-] is known as the ion-product constant for water or K_w . It's possible to calculate K_w using Gibbs Free Energy concepts, but for now know that the equilibrium constant for water K_w = 1 times 10^-14 mol^2/dm^2. (Brackets around a molecular formula denote molarity or concentration in solution) Show how pure water has a pH of 7 using the definition of the log and K_w. One caveat: Recall from class that transcendental functions (logs, exponents, trig functions) must not have any units in their argument. How do you manage this in your calculation? A solution has a pH of 6.8. The number of H+ ions is doubled. What is the resultant pH? A solution has a pH of 4. What is the pOH? (Let pOH be defined as pOH = -log (a_OH-))
Jarrod RobelLv2
19 Feb 2019