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SOLVED: Calculate the percent ionization for a 0.0194 M solution of the weak acid HIO with K= 1.75 x 10-5 Assume the mixture initially has 100 HIO particles. Drag the correct number
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![SOLVED: Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation: IO- HzO = HIO + OH- Kb for hypoiodite ion 4.37x10-4 Calculate the [H+]](https://cdn.numerade.com/ask_images/9d80eb482c1a4947a4ffb060669f0832.jpg "SOLVED: Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation: IO- HzO = HIO + OH- Kb for hypoiodite ion 4.37x10-4 Calculate the [H+]")
SOLVED: Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation: IO- HzO = HIO + OH- Kb for hypoiodite ion 4.37x10-4 Calculate the [H+]
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SOLVED: (5) Calculate the open cell potential, Ecell, if the half-reaction CuzO(s) + HzO(l) + 2 e 2 Cu(s) + 2 OH-(aq) is coupled to a Ag/AgCl reference electrode. Standard conditions apply
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SOLVED: Hypoiodous acid (HIO) is a weak acid that dissociates in water as follows: HIO(aq) + H2O(l) H3O+(aq) + IO−(aq). A 0.12 M solution of hypoiodous acid has a pH of 5.71.
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