2.5 mL of 2/5 M weak monoacidic base (Kb = 1 × 10-12 at 25°C) is titrated with 2/15 M HCl in water at 25°C. The concentration of H+ at equivalence point is (Kw= 1 × 10-14 at 25°C)
3.7 × 10-13 M
3.2 × 10-7 M
3.2 × 10-2 M
2.7 × 10-2 M
The concentration of CO2 which will be in equilibrium with 2.5 × 10-2 mol L-1 of CO at 100°C for the reaction will be
0.5 × 10-2 mol L-1
12.5 × 10-2 mol L-1
2 × 10-2 mol L-1
None of these
The pKα of a weak acid, HA is 4.80. The Kb of a weak base BOH is 4.78. The pH of an aqueous solution of the corresponding salt BA , will be
7.01
9.22
9.58
4.79
The pH value of blood does not change appreciably by a small addition of an acid or base, because the blood -
is a body fluid
can be easily coagulated
contains iron as a part of the molecule
contains serum protein that acts as buffer
The values of Kp1 and Kp2 for the reactions and are in ratio of 9:1.If degree of dissociation of x and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio of
3:1
1:9
36:1
1:1
Solubility product constant (Ksp) of salts of types MX , MX2 and M3X at temperature ' T ' are 4.0 × 10-8 , 3.2 × 10-14 and 2.7 × 10-15 respectively. Solubilities (mol dm-3) of the salts at temperature ' T ' are in the order
MX > MX2 > M3X
M3X > MX2 > MX
MX2 > M3X > MX
MX > M3X > MX2
then the formation constant of [Ag(NH3)2]+ is
6.08 × 10-6
6.08 × 106
6.08 × 10-9
0.1 mole of CH3NH2 (Kb = 5 × 10-4 ) is mixed with 0.08 mole of HCl and diluted to one litre. What will be the H+ concentration in the solution?
8 × 10-2 M
8 × 10-11 M
1.6 × 10-11 M
8 × 10-5 M
Which of the following is most soluble ?
Bi2S3(KSP=1×10-70)
MnS(KSP=7×10-16)
CuS(KSP=8×10-37)
Ag2S(KSP=6×10-51)
The solubility of sparingly soluble salt, AB2 in water is 1.0 × 10-5 mol L-1 .Its solubility product will be
4 × 10-10
1 × 10-15
1 × 10-10
4 × 10-15
