The hydrogen ion concentration of a 10-8 M HCl aqueous solution at 298k (kw = 10-14 ) is ___________ .
1.0×10-6 M
1.0525×10-7 M
9.525×10-8 M
1.0×10-8 M
The rapid change of pH near the stoichiometric point of an acid base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In-) forms of the indicator given by the expression
log [In-] / [HIn] = pKIn-pH
log [HIn] / [In-] = pKIn-pH
log [HIn] / [In-] = pH-pKIn
log [In-] / [HIn] = pH -pKIn
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 .
3:1
1:9
36:1
1:1
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
H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group in qualitative analysis but not those belonging to the fourth group. It is because
Presence of HCl decreases the sulphide ion concentration.
Presence of HCl increases the sulphide ion concentration.
Solubility product of group 2nd sulphides is more than that of group iv silphides
Sulphides of group iv cations are unstable in HCl
Which has highest pH ?
CH3COOK
Na2CO3
NH4Cl
NaNO3
The Strongest conjugate base is ____ .
NO3-
Cl-
SO4 2-
CH3COO-
The compound whose aqueous solution has the highest pH is ______ .
NaCl
NaHCO3
NH4 Cl
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
The hydride ion H- is strong base than its hydroxide ion OH-. Which of the following reactions will occur if sodium hydride (NaH) is dissolved in Water ?
2H-(aq) + H2O(l)→H2O+H2 +2e-
H-(aq) + H2O(l)→OH-+H2
H - + H2O(l) → no reaction
None of the above
