Which of the following represents the correct pH of a 10-7 M HCl in doubly distilled air-free water?
6.6990
7.0000
7.3010
6.3980
The solubihty of AgI in NaI solution is less than that in pure water because
Agl forms complex with Nal
of common ion effect
solubility product of AgI less
the temperature of the solution decreases
B.
of common ion effect
Solubility is decreased due to common ion effect
Ag Ag+ + I-
NaI Na+ + I-
I- is common ion in both the reaction.
Hydrogen ion concentration in mol/L in a solution of pH = 5.4 will be
3.98 × 108
3.88 × 106
3.68 × 10-6
3.98 × 10-6
XY2 dissociated as XY2(g) XY(g) + Y (g) When the initial pressure of XY2 is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction assuming that the volume of the system remains unchanged.
50
100
166.6
400.0
For the following equilibrium, N2O4 2NO2 in the gaseous phase, NO2 is 50% of the total volume when equilibrium is set up. Hence, per cent of dissociation of N2O4 is
50%
25%
66.66%
33.33%
1 mL of 0.01 N HCl is added to 999 mL solution of 0.1 N Na2SO4. The pH of the resulting solution will
2
7
5
1
The equilibrium constants for the reaction,
Br2 2Br → 1
at 500 K and 700 K are 1 × 10-10 and 1 × 10-5 respectively. The reaction is
endothermic
exothermic
fast
slow