Ionisation constant of CH3COOH is 1.7×10-5 and concentration of H+ ions is 3.4×10-4. Then, find out initial concentration of CH3COOH molecules.
3.4 × 10-4
3.4 × 10-3
6.8 × 10-4
6.8 × 10-3
A weak acid HA, has a Ka of 1.00 ×10-5. If 0.100 mole of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to
99.0%
1.00 %
99.9%
0.100%
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
In which of the following the solubility of AgCl will be minimum ?
0.1 m NaNO3
Water
0.1 m NaCl
0.1 m NaBr
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25, then find out pKb of NH4OH
9.25
4.75
3.75
8.25
Which of the following molecules acts as a Lewis acid ?
(CH3)3B
(CH3)2O
(CH3)3P
(CH3)3N
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
What is the [OH-] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?
0.10 MNumber of milliequivalents of HCl =20×0.050×1=1Number of milliequivalents of Ba(OH)2 = 2×30×0.10=6[OH-] of final solution = milliequivalents of Ba(OH)2 - milliequivalents of HCl / Total volume = 6 - 1 / 50=0.1 M
0.40 M
0.0050 M
0.12 M
The strongest conjugate base is
NO3-
Cl-
SO4 2-
CH3COO-
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