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Each of HCO(3)^(-) and HPO(4)^(2-) can a...

Each of `HCO_(3)^(-) and HPO_(4)^(2-)` can act both as Bronsted acid and base-why? Write the formula of conjugate base and conjugate acid in each case.

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According to Bronsted-Lowry concept, an acid is a proton donor and a base is a proton acceptor. Since the given species are capable of accepting and donating proton, they can act as an acid as well as a base.

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CHHAYA PUBLICATION-EQUILIBRIUM-WARM UP EXERCISE
  1. Identify the Lewis acids and Lewis bases in the reaction below: AlF(...

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  2. All Lewis bases are in fact Bronsted bases-Explain.

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  3. Each of HCO(3)^(-) and HPO(4)^(2-) can act both as Bronsted acid and b...

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  4. State and exaplain Ostwald's dilution law.

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  5. Of the two solutions of acetic acid with concentrations 0.1(N) and 0.0...

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  6. Write down the limitations of Ostwald's dilution law.

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  9. A weak tribasic acid, H(3)A, in its aquous solution ionises in the fol...

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  10. A weak tribasic acid, H(3)A, in its aquous solution ionises in the fol...

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  11. At a certain temperature, the ratio of ionisation constants of weak ac...

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  12. Are the ionisation constant and ionic product of water the same? Expla...

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  13. Find [OH^(-)] in pure water if [H(3)O^(+)] in it is x mol*L^(-1). Also...

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  14. Why is the ionic product of water at 50^(@)C greater than that at 25^(...

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  15. Why does the concentration of OH^(-) ions in pure water increase with ...

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  16. At 25^(@)C what is the concentration of H(3)O^(+) ions in an aqueous s...

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  19. By what factor will the concentration of H(3)O^(+) ions in an aqueous ...

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