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  • Weak Acids and Equilibrium - Division of Chemical Education . . .
    When solving problems involving weak acids, it may appear that one assumption is made that is small compared with the initial concentration of HOAc In fact, two assumptions are made The second assumption is hidden in the way the problem is set up
  • When calculating [H3O+] for weak acid solutions, we can often . . .
    The approximation method used for calculating [H3O+] for weak acid solutions is based on the assumption that the ionization of the acid is minimal This assumption is valid for weak acids, where the initial concentration of the acid, HA, is significantly greater than the concentration of the ionized parts, H3O+ and A-
  • Gen Chem Quiz 8 (Ch 15: 22-29, Ch 16: 1-11) Flashcards
    when calculating the [H3O+] for a polyprotic acid, the second ionization step can often be neglected explain why this is valid -for most polyprotic acids, Ka1 is much larger than Ka2
  • Weak Acid and Base Equilibria - umb. edu
    Why? We have seen that the calculation of [H3O +] and pH for solutions of strong acids and base To carry out a calculation of all species present in a solution of a pure weak acid in water requires use of the equilibrium constant for the acid’s hydrolysis, called Ka In similar fashion,
  • Problem 20 When calculating [H3O+] for weak. . . [FREE . . . - Vaia
    Since [HA]initial remains relatively constant and close to its starting value, the hydronium ion concentration can be calculated by taking the square root of the product of Ka and the initial concentration of the weak acid ([HA]initial): [H3O+] ≈ √(Ka * [HA]initial)
  • Solved 1. (1 pt) Which ion forms a basic solution when . . .
    In most solutions containing a strong or weak acid, the autoionization of water can be neglected when calculating [H3O+] (this is why we assume the initial [H3O+]≈0 in the ICE table) Explain why this assumption is valid: a) ( 1 pt) by comparing the Kw and There are 2 steps to solve this one 1 b) H3O+
  • Bases - Simplifying Assumptions in Acid-Base Reactions for . . .
    (ii) The weak acid assumption: In pH calculations involving weak acids we ASSUME that the amount of H–A “lost” to ionization (“x”) is small and thus that [H– A]equil will not change much from (HA)initial (i not much HA ‘goes away) This lets us pretend that [H–A]equil is unchanged from (HA)initial





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