Equilibrium Test

Result

Equilibrium Test - 64

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Weekly Quiz Competition

Question 1
1 / -0

A hydrogen electrode placed in a buffer solution of NaCl and HCN in the ratio of X:Y and Y:X has an oxidation electrode potential values $${E_1}\,\,and\,\,{E_2}$$ volts respectively at $${25^0}C$$. The pKa value of HCN is

A
$$\frac{{({E_1} + {E_2})}}{{0.118}}$$

B
$$ - \frac{{({E_1} + {E_2})}}{{0.118}}$$

C
$$\frac{{({E_1} - {E_2})}}{{0.118}}$$

D
$$\frac{{({E_2} - {E_1})}}{{0.118}}$$

Solution
Question 2
1 / -0

In a buffer solution the ratio of concentration of $${\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl}}\,\,{\text{and}}\,{\text{N}}{{\text{H}}_{\text{4}}}{\text{OH}}\,\,{\text{is}}\,\,{\text{1:1}}$$ when it changes in 2:1 what will be the value of pH of buffer:-

A
Increase

B
Decrease

C
No effects

D
N. O. T.

Solution
Question 3
1 / -0

For the Chemical reaction $${{\text{A}}_{{\text{2}}\left( {\text{g}} \right)}}{\text{ + }}{{\text{B}}_{{\text{2}}\left( {\text{g}} \right)}} \rightleftharpoons {\text{2A}}{{\text{B}}_{\left( {\text{g}} \right)}}$$ the amount of AB at equilibrium is affected by

A
Temperature and pressure

B
Temperature only

C
Pressure only

D
Temperature, pressure and Catalyst
Question 4
1 / -0

Which of the following may be regarded as buffer solution?

A
50 ml of 0.1 M acetic acid + 50 ml of 0.05 M $$NaOH$$

B
50 ml of 0.05 ammonia + 50 ml of 0.1 M $$HCl$$

C
25 ml of 0.1 M acetic acid + 50 ml of 0.1 M $$NaOH$$

D
50 ml of 0.1 ammonia + 50 ml of 0.05 M $$HCl$$
Question 5
1 / -0

If the degree of ionization of water is 1.8 x $$10^{-9}$$ at a given temperature. Its ionic product will be

A
1.8 x $$10^{-16}$$

B
1 x $$10^{-14}$$

C
1 x $$10^{-16}$$

D
1.67 x $$10^{-14}$$

Solution
Question 6
1 / -0

$$2{H_2}O\leftrightharpoons {H_3}{O^ + } + O{H^ - },{K_w} = 1\times {10^{ - 14}}$$ at $${25^ \circ }C$$ hence $$K_a$$ is :

A
$$1\times 10^{-14}$$

B
$$18\times 10^{-17}$$

C
$$5.55\times 10^{-3}$$

D
$$1.00\times 10^{-7}$$
Question 7
1 / -0

The dissociation constant of a weak acid is $$1.0 \times { 10 }^{ -5 }$$, the equilibrium constant for its reaction with strong base is

A
$$1.0 \times { 10 }^{ -5 }$$

B
$$1.0 \times { 10 }^{ 9 }$$

C
$$1.0 \times { 10 }^{ 7 }$$

D
$$1.0 \times { 10 }^{ 14 }$$

Solution
Question 8
1 / -0

At $$90^{ \circ }C$$, pure water has $$[{ H }_{ 3 }O^{ + }]={ 10 }^{ -6.7 }\ mol/lit$$. What is the value of $${ K }_{ W }$$ at $${ 90 }^{ \circ }C :-$$

A
$${ 10 }^{ -6 }$$

B
$${ 10 }^{ -12 }$$

C
$${ 10 }^{ -14 }$$

D
$${ 10 }^{ -13.4 }$$

Solution
Question 9
1 / -0

If $$1M$$ $$C{H_3}COONa$$ is added to $$1M$$ $$C{H_3}COOH$$, then:

A
$$pH$$ of the solution increases

B
$$pH$$ decreases

C
$$pH$$ does not change

D
cannot be predicted
Question 10
1 / -0

One litre of water contains $$10 ^ { - 7 }$$ mole of $$H ^ { + }$$ ions. Degree of ionisation of water is:

A
$$1.8 \times 10 ^ { - 7 } \%$$

B
$$0.8 \times 10 ^ { - 9 } \%$$

C
$$3.6 \times 10 ^ { - 9 } \%$$

D
$$3.6 \times 10 ^ { - 7 } \%$$

Solution

$$1$$ litre of water contains $$1000/18$$ mole.

So degree of ionization $$=\dfrac {10^{-7}\times 18}{1000}=1.8\times 10^{-7}\%$$

Option A is correct.