According to the Bronsted-Lowry concept,an acid is a substance which:

What do you understand by the term 'auto-protolysis' of water? What is its significance?

Identify the conjugate acid and conjugate base for the $HCO_3{ }^{-}$ ion,respectively.

Phosphoric acid ionizes in three steps with their ionization constant values $K_{a_1}, K_{a_2}$ and $K_{a_3}$ respectively,while $K$ is the overall ionization constant. Which of the following statements are true?
$A.$ $\log K = \log K_{a_1} + \log K_{a_2} + \log K_{a_3}$
$B.$ $H_3PO_4$ is a stronger acid than $H_2PO_4^{-}$ and $HPO_4^{2-}$
$C.$ $K_{a_1} > K_{a_2} > K_{a_3}$
$D.$ $K_{a_1} = \frac{K_{a_3} + K_{a_2}}{2}$
Choose the correct answer from the options given below

What is the nature of an aqueous solution of ammonia?

Which of the following is a $Br\text{ø}nsted-Lowry$ acid?