Advertisements
Advertisements
Question
What will be the conjugate bases for the following Bronsted acids:
HF, H2SO4 and \[\ce{HCO^-_3}\]?
Advertisements
Solution
The conjugate bases should have one proton less in each case and therefore the corresponding conjugate bases are F−, \[\ce{HSO^-_4}\] and \[\ce{CO^2-_3}\] respectively.
RELATED QUESTIONS
Water acts as Bronsted acid as well as a Bronsted base. Give one example each to illustrate this statement.
Give Lewis's definition of acids and bases.
Complete the following statement by selecting the correct alternative from the choices given:
The conjugate acid of `"HPO"_4^(2-)` is :
Give a reason for the following:
Zn2+ salts are white but Cu2+ salts are blue in colour.
\[\ce{BF3}\] does not have proton but still acts as an acid and reacts with \[\ce{NH3}\]. Why is it so? What type of bond is formed between the two?
A reaction between ammonia and boron trifluoride is given below: \[\ce{NH3 + BF3 -> H3N : BF3}\] Identify the acid and base in this reaction. Which theory explains it? What is the hybridisation of B and N in the reactants?
Match the following species with the corresponding conjugate acid:
| Species | Conjugate acid |
| (i) \[\ce{NH3}\] | (a) \[\ce{CO^{2-}3}\] |
| (ii) \[\ce{HCO^{-}3}\] | (b) \[\ce{NH^{+}4}\] |
| iii) \[\ce{H2O}\] | (c) \[\ce{H3O+}\] |
| (iv) \[\ce{HSO^{-}4}\] | (d) \[\ce{H2SO4}\] |
| (e) \[\ce{H2CO3}\] |
Acidity of BF3 can be explained on the basis of which of the following concepts?
