14.6a | How does HS− acts as a Brønsted-Lowry base?
14.4f | How does HS− acts as a Brønsted-Lowry acid?
Which of the following can act as both Bronsted acid and Bronsted base?....
14.3a | How does H3O+ act as a Brønsted-Lowry acid?
14.4c | How does H2S acts as a Brønsted-Lowry acid?
14.4e | How does H2PO4− acts as a Brønsted-Lowry acid?
Both HCO3 and HS are amphoteric Write an equation to show how each substance can act as an acid,
14.10c | How to identify the conjugate acid-base pairs in HS− + H2O → H2S + OH−
14.3f | How does HSO4− acts as a Brønsted-Lowry acid?
14.5e | How does S2− acts as a Brønsted-Lowry base?
14.5f | How does H2PO4− acts as a Brønsted-Lowry base?
Assertion : A substance that can either act as an acid a base is called ampholyte. Reason
Which of the following can act as an acid and as a base? | Redox Master Series | Master stroke
14.3e | How does NH4+ act as a Brønsted-Lowry acid?
14.2 | Write equations that show H2PO4− acting both as an acid and as a base
Chapter 15 Intro to Acids and Bases
Bronsted-Lowry Theory of Acids and Bases
