The concentration of [H+] and concentration of [OH- ] of a 0.1M aqueous solution of 2% ionised weak monobasic 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 statements about pH and H+ ion concentration is incorrect ?
addition of one drop of concentrated HCl in NH4OH solution decreases pH of the solution.
A solution of the mixture of one equivalent of each of CH3COOH and NaOH has a pH of 7 .
pH of pure neutral water is not zero .
A cold and con.H2SO4 has lower H+ ion concentration than a dilute solution of H2SO4
Calculate the pOH of a solution at 250C that contains 1.0×10-6 M of hydronium ions .
7.00
4.00
9.00
1.00
At 250C, the dissociation constant of a base, BOH is 1.0 ×10-12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be ________ .
2.0 ×10-6 mol L-1
1.0 ×10-5 mol L-1
1.0 ×10-6 mol L-1
1.0 ×10-7 mol L-1
The conjugate acid of NH2- is ______ .
N2H4
NH4 +
NH2 OH
NH3
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
A Physician wishes to prepare a buffer solution at pH =3.58 that efficiently resist changes in pH yet contains only small concentration of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use ?
m-chlorobenzoic acid (pKa=3.98)
P-Chlorocinnamic acid(pKa = 4.41)
2,5 -dihydroxy benzoic acid (pKa=2.97)
Acetoacetic acid(pKa=3.58)
Solubility of a M2S type salt is 3.5 ×10-6, then find out its solubility product
1.7 ×10-6
1.7×10-16
1.7 ×10-18
1.7 ×10-12
The dissociation equilibrium of a gas AB2 can be represented as : 2AB2(g) 2AB(g) +B2(g) The degree of dissociation is 'x' and is small compared to 1.The expression relating the degree of dissociation (x) with equilibrium constant Kp and total pressure p is _______ .
(2Kp/ p)
(2Kp / p)1/3
(2Kp / p)1/2
(Kp / p)
Solubility of MX2 type electrolytes is 0.5 ×10-4 mol / L, then find out Ksp of electrolytes.
5×10-12
25×10-10
1×10-13
5×10-13
