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Using K values to predict reactions between different acids and bases.

Using K values to predict reactions between different acids and bases. HF + CH 3 COO - F - + CH 3 COOH. eg:. Given the following acid base equilibrium, is the forward or reverse reaction favoured ?. Compare the strengths of the two acids:. HF & CH 3 COOH. K A (HF) = 3.5x10 -4.

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Using K values to predict reactions between different acids and bases.

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  1. Using K values to predict reactions between different acids and bases. HF + CH3COO-F-+ CH3COOH eg: Given the following acid base equilibrium, is the forward or reverse reaction favoured? Compare the strengths of the two acids: HF & CH3COOH KA (HF) = 3.5x10-4 KA (CH3COOH) = 1.8x10-5 Because KA (HF) > KA (CH3COOH) the forward reaction is favoured. (at equilibrium there will be more products than reactants.) Note: you could also compare KB values for the two bases and you would get the same result.

  2. HCO3- + HSO3- ? HCO3- + HSO3-H2CO3 + SO32- eg: If HCO3- is combined with HSO3- a) Write the equation for the equilm reaction which results. KA (HCO3-) = 5.6x10-11 KA (HSO3-) = 1.0x10-7 KA (HSO3-) > KA (HCO3-) • HSO3- acts as an acid.

  3. HCO3- + HSO3- H2CO3 + SO32- b) In this equilm, are the reactants or products favoured? base acid acid base Compare acid in each direction KA (HSO3-) = 1.0x10-7 KA (H2CO3) = 4.3x10-7 KA (H2CO3) > KA (HSO3-) • Reactants are slightly favoured.

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