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Q. No.In a qualitative analysis, \(Bi^{3+}\) is detected by the appearance of a precipitate of \(BiO(OH)(s)\).
Calculate pH when the following equilibrium exists at 298 K :
\(BiO(OH)(s) \rightleftharpoons BiO^+(aq) + OH^-(aq)\),
\(K = 4 \times 10^{-10}\)
(Given : \(\log 2 = 0.3010\))
1. 4.699
2. 8.714
3. 9.301
4. 5.286
Calculate pH when the following equilibrium exists at 298 K :
\(BiO(OH)(s) \rightleftharpoons BiO^+(aq) + OH^-(aq)\),
\(K = 4 \times 10^{-10}\)
(Given : \(\log 2 = 0.3010\))
1. 4.699
2. 8.714
3. 9.301
4. 5.286
Subtopic: pH calculation |
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Level 3: 35%-60%
NEET - 2026
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At 298 K, a certain buffer solution contains equal concentrations of X- and HX, Kb for X- is 10-10.
What is the pH of this buffer solution ?
1. 2
2. 10
3. 4
4. 6
What is the pH of this buffer solution ?
1. 2
2. 10
3. 4
4. 6
Subtopic: pH calculation | Buffer |
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Given below are certain reactions. Identify the reaction for which \(K_p \neq K_c .\)
| 1. | \( \mathrm{H}_2(\mathrm{~g})+I_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{~g})\) |
| 2. | \( \mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{~g}) \) |
| 3. | \( \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) \) |
| 4. | \( \mathrm{H}_2 \mathrm{O}(\mathrm{~g})+\mathrm{CO}(\mathrm{~g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g}) \) |
Subtopic: Kp, Kc & Factors Affecting them |
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For the reaction \(A(g) \rightleftharpoons 2B(g),\) the backward reaction rate constant is higher than the forward reaction rate constant by a factor of \(2500\) at \(1000~K \).
\(K_p\) for the reaction at \(1000~ K\) is:
[ Given: \({R= 0.0831~ L ~\text{atm mol}^{-1} }K^{-1}]\)
\(K_p\) for the reaction at \(1000~ K\) is:
[ Given: \({R= 0.0831~ L ~\text{atm mol}^{-1} }K^{-1}]\)
| 1. | \(0.033 \) | 2. | \(0.021 \) |
| 3. | \(83.1 \) | 4. | \(2 .077 \times 10^5\) |
Subtopic: Kp, Kc & Factors Affecting them |
51%
Level 3: 35%-60%
NEET - 2025
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Phosphoric acid ionizes in three steps, with their ionization constant values \(\mathrm{K}_{\mathrm{a}_1}, \mathrm{~K}_{\mathrm{a}_2} \text { and } \mathrm{K}_{\mathrm{a}_3} \text {, }\)respectively, while \(K\) is the overall ionization constant. Which of the following statements are true for the ionization of phosphoric acid?
Choose the correct answer from the options given below :
1. B, C and D only
2. A, B and C only
3. A and B only
4. A and C only
| A. | \(\log \mathrm{K}=\log \mathrm{K}_{\mathrm{a}_1}+\log \mathrm{K}_{\mathrm{a}_2}+\log \mathrm{K}_{\mathrm{a}_3}\) |
| B. | \(\mathrm{H}_3 \mathrm{PO}_4\) is a stronger acid than \(\mathrm{H}_2 \mathrm{PO}_4^{-}\) and \(\mathrm{HPO}_4^{2-} .\) |
| C. | \(\mathrm{K}_{a_1} >\mathrm{~K}_{\mathrm{a}_2}>\mathrm{K}_{\mathrm{a}_3} \) |
| D. | \(\mathrm{K}_{\mathrm{a}_1}=\frac{\mathrm{K}_{\mathrm{a}_3}+\mathrm{K}_{\mathrm{a}_2}}{2}\) |
1. B, C and D only
2. A, B and C only
3. A and B only
4. A and C only
Subtopic: Ionisation Constant of Acid, Base & Salt |
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Which of the following parameters can determine the higher yield of \(\mathrm{NO}\) in the reaction, \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\) ?
\([ Given: \Delta \mathrm{H}\) of the reaction \(=+180.7 \mathrm{~kJ} \mathrm{~mol}^{-1} ]\)
A. higher temperature
B. lower temperature
C. higher concentration of \(\mathrm{N}_2\)
D. higher concentration of \(\mathrm{O}_2\)
Choose the correct answer from the options given below:
1. B, C, D only
2. A, C, D only
3. A, D only
4. B, C only
\([ Given: \Delta \mathrm{H}\) of the reaction \(=+180.7 \mathrm{~kJ} \mathrm{~mol}^{-1} ]\)
A. higher temperature
B. lower temperature
C. higher concentration of \(\mathrm{N}_2\)
D. higher concentration of \(\mathrm{O}_2\)
Choose the correct answer from the options given below:
1. B, C, D only
2. A, C, D only
3. A, D only
4. B, C only
Subtopic: Le Chatelier's principle |
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For the reaction \(2 \mathrm{A} \rightleftharpoons \mathrm{B}+\mathrm{C}; ~\mathrm{K}_{\mathrm{c}}=4 \times 10^{-3}\).
At a given time, the composition of the reaction mixture is : \([\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=2 \times 10^{-3} \mathrm{M} \text {. }\)
In light of the above facts, which of the following is correct?
At a given time, the composition of the reaction mixture is : \([\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=2 \times 10^{-3} \mathrm{M} \text {. }\)
In light of the above facts, which of the following is correct?
| 1. | Reaction has a tendency to go in the forward direction. |
| 2. | Reaction has a tendency to go in the backward direction. |
| 3. | Reaction has gone to completion in the forward direction. |
| 4. | Reaction is at an equilibrium. |
Subtopic: Kp, Kc & Factors Affecting them | Le Chatelier's principle |
58%
Level 3: 35%-60%
NEET - 2024
Hints
In which of the following equilibria,\(\text{K}_\text{p}\) and \(\text{K}_\text{c}\) are NOT equal?
| 1. | \(\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{(\mathrm{g})}\) |
| 2. | \(\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}\) |
| 3. | \(2 \mathrm{BrCl}_{(\mathrm{g})} \rightleftharpoons \mathrm{Br}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}\) |
| 4. | \(\mathrm{PCl}_{5(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}\) |
Subtopic: Kp, Kc & Factors Affecting them |
79%
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Hints
Consider the following reaction in a sealed vessel at equilibrium:
\(2 \text{NO}_{(\text{g})} \rightleftharpoons \text{N}_{2(\text{g})} +\text{O}_{2\text{(g)}}\)
[Given: \(\text{N}_2=3.0 \times 10^{-3} \text{M}, \text{O}_2=4.2 \times 10^{-3} \text{M}\) and \(\text{NO}=2.8 \times 10^{-3} \text M\)]
If 0.1 mol L-1 of NO(g) is taken in a closed vessel, what will be the degree of dissociation (\(\alpha\)) of NO(g) at equilibrium?
1. 0.0889
2. 0.00717
3. 0.717
4. 0.00889
\(2 \text{NO}_{(\text{g})} \rightleftharpoons \text{N}_{2(\text{g})} +\text{O}_{2\text{(g)}}\)
[Given: \(\text{N}_2=3.0 \times 10^{-3} \text{M}, \text{O}_2=4.2 \times 10^{-3} \text{M}\) and \(\text{NO}=2.8 \times 10^{-3} \text M\)]
If 0.1 mol L-1 of NO(g) is taken in a closed vessel, what will be the degree of dissociation (\(\alpha\)) of NO(g) at equilibrium?
1. 0.0889
2. 0.00717
3. 0.717
4. 0.00889
Subtopic: Introduction To Equilibrium |
Level 3: 35%-60%
NEET - 2024
Hints
Consider the given reaaction:
\(\mathrm{PCl}_5 \leftrightharpoons\mathrm{PCl}_3+\mathrm{Cl}_2\)
At equilibrium at \(500 \mathrm{~K},\) the concentration of \(\mathrm{PCl}_5=1.40~ \mathrm{M} \text {, }\) concentration of \(\mathrm{Cl}_2=1.60~ \mathrm{M} \text {, }\) concentration of \(\mathrm{PCl}_3=1.60 \mathrm{M}\). Calculate \(K_c\):
1. 2.00
2. 2.6
3. 1.83
4. 3.4
\(\mathrm{PCl}_5 \leftrightharpoons\mathrm{PCl}_3+\mathrm{Cl}_2\)
At equilibrium at \(500 \mathrm{~K},\) the concentration of \(\mathrm{PCl}_5=1.40~ \mathrm{M} \text {, }\) concentration of \(\mathrm{Cl}_2=1.60~ \mathrm{M} \text {, }\) concentration of \(\mathrm{PCl}_3=1.60 \mathrm{M}\). Calculate \(K_c\):
1. 2.00
2. 2.6
3. 1.83
4. 3.4
Subtopic: Kp, Kc & Factors Affecting them |
88%
Level 1: 80%+
NEET - 2024
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