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Q. No.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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Level 2: 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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Level 2: 60%+
NEET - 2026
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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 |
54%
Level 3: 35%-60%
NEET - 2026
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The correct order of solubility of the given salts in water at 298 K is :
| Salt | \(\mathbf{K_{sp}}\) at 298 K |
| AgBr | \(5.0 \times 10^{-13}\) |
| \(Zn(OH)_2\) | \(1.0 \times 10^{-15}\) |
| \(Hg_2Cl_2\) | \(1.3 \times 10^{-18}\) |
| 1. | \(Zn(OH)_2 > AgBr > Hg_2Cl_2\) |
| 2. | \(Hg_2Cl_2 > Zn(OH)_2 > AgBr\) |
| 3. | \(AgBr > Zn(OH)_2 > Hg_2Cl_2\) |
| 4. | \(Hg_2Cl_2 > AgBr > Zn(OH)_2\) |
Subtopic: Solubility Product |
Level 4: Below 35%
NEET - 2026
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In an acidic medium, 10 mL of 0.25 M oxalic acid is titrated with \(KMnO_4\) solution. If the volume of \(KMnO_4\) solution required to reach end point is 10 mL, the strength of the \(KMnO_4\) solution is:
| 1. | 0.15 M |
| 2. | 0.10 M |
| 3. | 0.20 M |
| 4. | 0.25 M |
Subtopic: Acids & Bases - Definitions & Classification | Salt Hydrolysis & Titration |
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Level 3: 35%-60%
NEET - 2026
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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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Level 2: 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 |
57%
Level 3: 35%-60%
NEET - 2025
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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 |
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The ratio of solubility of \(\mathrm{AgCl}\) in \(0.1~ \mathrm{M} ~\mathrm{KCl}\) solution to the solubility of \( \mathrm{Ag} \mathrm{Cl}\) in water is:
(Given: Solubility product of \(\mathrm{AgCl}=10^{-10}\) )
(Given: Solubility product of \(\mathrm{AgCl}=10^{-10}\) )
| 1. | \(10^{-4}\) | 2. | \(10^{-6}\) |
| 3. | \(10^{-9}\) | 4. | \(10^{-5}\) |
Subtopic: Solubility Product |
Level 3: 35%-60%
NEET - 2024
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At a given temperature and pressure, the equilibrium constant value for the equilibria are given below:
\(3A_2+B_2\rightleftharpoons 2A_3B, K_1\\ A_3B \rightleftharpoons \frac 3{2}A_2+\frac 1{2}B_2, K_2 \)
The relation between \(K_1\) and \(K_2\) is:
\(3A_2+B_2\rightleftharpoons 2A_3B, K_1\\ A_3B \rightleftharpoons \frac 3{2}A_2+\frac 1{2}B_2, K_2 \)
The relation between \(K_1\) and \(K_2\) is:
| 1. | \(K^2_1=2K_2\) | 2. | \(K_2= \dfrac { K_1 }{2}\) |
| 3. | \(K_1=\dfrac 1{\sqrt K_2}\) | 4. | \(K_2=\dfrac 1{\sqrt K_1}\) |
Subtopic: Introduction To Equilibrium |
69%
Level 2: 60%+
NEET - 2024
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