St. Britto Hr. Sec. School - Madurai
12th Chemistry weekly Test - 1 ( Ionic Equilibrium )-Aug 2020
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Degree of dissociation \(\alpha \) is
\(\alpha =\frac { { { K }_{ a } } }{ C } \)
\(\alpha =\frac { { { C }^{ 2 } } }{ { K }_{ a } } \)
\(\alpha =\sqrt { \frac { { K }_{ a } } { { C } }} \)
\(\alpha =\sqrt { \frac { { C } }{ { K }_{ a } } } \)
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A solution which is resistant to changes of pH on addition of small amounts of an acid or a base is known as
buffer solution
true solution
isohydric solution
ideal solution
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H2 \({ PO }_{ 4 }^{ - }\) the conjugate base of
\({ PO }_{ 4 }^{ 3- }\)
P2O5
H3PO4
H\({ PO }_{ 4 }^{ 3- }\)
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According to ___ concept, BF3 acts as a acid.
Bronsted.
Arrhenius
Lewis
None of the above
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Dissociation constant ofNH40H is 1.8 x 10-5 the hydrolysis constant of NH4Cl would be
1.8 x 10-19
5.55 x 10-10
5.55 x 10-5
1.80 x 10-5
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Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.
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Calculate the pH of 1.5 x 10-3 M solution of Ba(OH)2.
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How is common ion effect related to the solubility of the electrolyte?
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When aqueous ammonia is added to CuSO4 solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, [Cu(H2O)4](aq)2+ + 4NH3(aq) \(\rightleftharpoons \) [Cu(NH3)4 ] (aq)2+, among H2O and NH3 Which is stronger Lewis base.
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Calculate the ionisation constant for the conjugate base of HF. Ionisation constant of HF at 298 K is 6.8 x I0-4
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The Kw of a neutral solution is 10-12 at a particular temperature. What are its pH and
pOHvalues? -
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What do you mean by auto ionisation of water?
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What is Henderson equation?
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Define buffer Index.
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Based on Arrhenius concept, define acid and bases and give an example for each.
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How will you calculate solubility product from molar solubility?
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For an aqueous solution of NH4Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)
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On hydrolysis of salts of strong acid and strong base, the solution obtained is neutral. Justify your answer with a suitable example.
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Derive the hydrolysis constant for the hydrolysis of salt of strong base and weak acid. Deduce its pH.
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Derive the relationship between pH and pOH.
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Derive Henderson - Hasselbalch equation.