Q.1 Define each of the following ?
i) Arrhenius acid
ii) Bronsted-Lowry acid
Q.2 Which of the following value, a stronger conjugate base has
a) Ka <1 b) Ka > 1 c) Ka = 1
Q.3 Weak acids are :
a) Partially dissociate with low ka value, b) Fully dissociate with low Ka value , c) Partially dissociate with high ka value d) Fully dissociate with high Ka value
Q.4 Write down the balance equation of the following acids and base in water.
a) HClO4(aq) + H2O(aq)
b) CH3COOH(aq) + H2O(aq)
Q.5. Identified the acid(a), base(b) , the conjugate base(cb) and the conjugate acid(ca) of the following reactions.
a) H2SO4(aq) + H2O(aq) H3O+ (aq) + HSO4(aq)
b) HOCl(aq) + C6H5NH2(aq) OCl(aq) + C6H5NH3+
c) H2O(aq) + HONH3(aq) HONH2 (aq) + H3O+ (aq)
Q.6 Give the order from strongest to weakest strength, of the following chemicals.
H2O, Ka = 1.0 x 10-14; HOCl, Ka = 3.5 x 10 -8; HNO3 , Ka >> 1
NH4 + Ka = 5.6 x 10-10
Q.7 In this reaction
HSO4- (aq) +
What are conjugate acid - base pairs:
Q.8 What is concentration of H+ in a 2.5 M HCl solution
a) 0 M b) 1.25 M c) 2.5 M d) 5.0 M
Q.9 Calculate the pH and [OH] of 5 x 10-3 M of HClO4 solution
Q.10 Calculate the [H+] and [OH-] for solution, Identify each solution is acidic, neutral or basic. If; a) pH = -1.0
b) pOH = 5.0