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
0.1 M solution of which one of these substances will be basic ?
Sodium borate
Calcium nitrate
NH4Cl
Sodium sulphate
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
Which one of the following is true for any diprotic acid H2X?
Ka2=Ka1
Ka2>Ka1
Ka2< Ka1
Ka2= 1 / Ka1
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%
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 M
0.40 M
0.0050 M
0.12 M
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 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 conjugate acid of NH2- is ______ .
N2H4
NH4 +
NH2 OH
NH3
