# <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be: 1. 4 2. 16 3. 2 4. 1

Subtopic:  Introduction To Equilibrium |
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The number of ${\mathrm{H}}^{\oplus }$ ions present in 1 ml of a solution whose pH= 4 , is given as:

(${N}_{A}=$ $Avogadro\text{'}s$ $number$)

1. ${10}^{-7}{N}_{A}$

2. ${10}^{-8}{N}_{A}$

3. ${10}^{-16}{N}_{A}$

4. ${10}^{-14}{N}_{A}$

Subtopic:  Acids & Bases - Definitions & Classification | pH calculation |
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If the pH of an acidic buffer is 5.7 and ${\mathrm{pK}}_{\mathrm{a}}$ is 5 then the ratio of $\frac{\left[\mathrm{Salt}\right]}{\left[\mathrm{Acid}\right]}$ will be:

 1 3 2 4 3 5 4 6
Subtopic:  Buffer |
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Assertion: At equilibrium, ${\mathrm{K}}_{}={\mathrm{Q}}_{\mathrm{c}}.$

Reason: When  the reaction mainly goes in the forward direction.

 1 Both assertion & reason are true and the reason is the correct explanation of the assertion. 2 Both assertion & reason are true but the reason is not the correct explanation of the assertion. 3 Assertion is a true statement but the reason is false. 4 Both assertion and reason are false statements.
Subtopic:  Kp, Kc & Factors Affecting them |
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Assertion: ${H}^{-}$ acts as both Bronsted Lowry base as well as Lewis base.

Reason: It acts as both ${H}^{\oplus }$ acceptor and a lone pair donor.

1. Both assertion & reason are true and the reason is the correct explanation of the assertion.

2. Both assertion & reason are true but the reason is not the correct explanation of the assertion.

3. Assertion is a true statement but the reason is false.

4. Both assertion and reason are false statements.

Subtopic:  Acids & Bases - Definitions & Classification |
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The concentration of $\left[{\mathrm{H}}^{+}\right]$ ion in a solution containing 0.1 M HCN and 0.2 M NaCN will be:

(${\mathrm{K}}_{\mathrm{a}}$ for HCN = $6.2×{10}^{-10}$)

1. 3.1$×{10}^{10}$

2. $6.2×{10}^{5}$

3. $6.2×{10}^{-10}$

4. $3.1×{10}^{-10}$

Subtopic:  Buffer |
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For the following reaction,
H2(g)+I2(g)2HI(g) $at$ $250°C,$

The effect on the state of equilibrium on doubling the volume of the system will be:

 1 Shift to the reactant side 2 Shift to the product side 3 No effect on the state of equilibrium 4 Liquefaction of HI

Subtopic:  Le Chatelier's principle |
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Reaction quotient for the reaction, ${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)⇌2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$ is given by , $\mathrm{Q}$ $=$ $\frac{{\left[{\mathrm{NH}}_{3}\right]}^{2}}{\left[{\mathrm{N}}_{2}\right]{\left[{\mathrm{H}}_{2}\right]}^{3}}$ .The reaction will proceed from right to left if Kc value is:

 1 QKc 4 Q=Kc
Subtopic:  Introduction To Equilibrium |
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An acid buffer solution can be prepared by mixing the solutions of:

1. Sodium chloride and sodium hydroxide

2. Sulphuric acid and sodium sulphate

3. Ammonium chloride and ammonium nitrate

4. Ammonium acetate and acetic acid

Subtopic:  Buffer |
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The basic buffer solution among the following is:

1. ${\mathrm{NH}}_{4}\mathrm{Cl}+{\mathrm{NH}}_{4}\mathrm{OH}$

2. $\mathrm{NaCl}+\mathrm{NaOH}$

3. ${\mathrm{NH}}_{4}\mathrm{Cl}+{\mathrm{CH}}_{3}\mathrm{COOH}$

4. ${\mathrm{CH}}_{3}\mathrm{COONa}+{\mathrm{CH}}_{3}\mathrm{COOH}$

Subtopic:  Buffer |
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