The solubility product of a salt having general formula MX2 , in water is 4 × 10-12 . The concentration of M2+ ions in the aqueous solution of the salt is
4.0 × 10-10 M
1.6 × 10-4 M
1.0 × 10-4 M
2.0 × 10-6 M
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 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
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 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
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 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 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
The pKα of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid ionised is
4.5
2.5
9.5
7.0