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
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
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
The solubility of a saturated solution of calcium fluoride is 2×10-4 mol / L . Its solubility product is,
12×10-2
14×10-4
22×10-11
32×10-12
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
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 a 10 M solution of HCl is
less than 0
Equal to 0
Equal to 1
Equal to 2
The pH of 0.1 M solution of a weak acid is 3. What is the value of the ionization constant for the acid?
0.1
10-3
10-5
10-7
The concentration of [H+] and concentration of [OH- ] of a 0.1M aqueous solution of 2% ionized weak mono basic acid is [ionic product of water = 1×10-14 ]
0.02×10-3 M and 5×10-11 M
1×10-3 M and 3×10-11 M
2×10-3 M and 5×10-12 M
3×10-2 M and 4×10-13 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)