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Each of HS^(-) and NH(3) can act as both...

Each of `HS^(-)` and `NH_(3)` can act as both Bronsted acid and Bronsted 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. The given species can accept as well as donate proton, so they can act as both acid and base.
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CHHAYA PUBLICATION-EQUILIBRIUM-QUESTION ANSWER ZONE FOR BOARD EXAMINATION (very short answer type)
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  2. In case of the reaction A(2)(g) +4B(2)(g) hArr 2AB(4)(g), the change i...

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  3. How will equilibrium of the reaction, H(2)(g)+I(2)(g)hArr 2HI(g) be af...

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  4. Each of HS^(-) and NH(3) can act as both Bronsted acid and Bronsted ba...

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  5. In the reaction I(2)+I^(-)toI(3)^(-), which one acts as a Lewis base?

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  6. The pK(a) values of the three weak acids HA, HB and HC are 4.74, 3.75 ...

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  7. X and Y are two aqueous solutions of acid HA with concentrations 0.1 M...

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  8. Which one of the following two acids will have a higher concentration ...

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  9. Show that [OH^(-)] gt sqrt(K(w)) in an alkaline solution.

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  10. Will the concentration of H(3)O^(+) ions in pure water at 0^(@)C be mo...

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  11. At a certain temperature, what is the value for the sum of pH annd pOH...

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  12. Show that in pure water, pH=pOH=(1)/(2)pK(w).

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  13. An acid bottle is labelled 'pH=5'. Is this acid a weak acid?

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  14. At a certain temperature, K(w) of pure water=10^(-12) what will be the...

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  15. pH of an aqueous 0.1(M) CH(3)COOH solution is 2.87. state whether pH o...

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  16. At 25^(@)C, the ionisation constant (K(a)) of weak acid HA is 10^(-6)....

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