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The quiz is designed for Ionic Equilibrium chapter for JEE Main level.
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Question 1 of 15
1. Question
4 points% hydrolysis of 0.1M CH3COONH4 when Ka = Kb = 1.8 x 10-5 is
(a) 55 x 10-2 (b) 0.55 (c) 7.63 (d) 1.8 x 10-4
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Question 2 of 15
2. Question
4 pointsWhich of the following system is not a buffer system?
(a) NH3 and NH4NO3 (b) Na2HPO4 and NaH2PO4
(c) KNO2 and HNO2 (d) KHSO4 and H2SO4
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Question 3 of 15
3. Question
4 pointsThe weight of CH3COONa needed to add in 1 litre N/10 CH3COOH to obtain a buffer solution of pH value 4 is (Given Ka = 1.8 x 10-5)
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Question 4 of 15
4. Question
4 pointsA dilute HCl solution saturated with H2S has pH value 3 then the concentration of S2- is (Given K1 = 1 x 10-7, K2 = 1.3 x 10-13)
(a) 2 x 10-13 M (b) 2.4 x 10-13 M (c) 3 x 10-15 (d) 1.3 x 10-15 M
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Question 5 of 15
5. Question
4 pointsWhich is the strongest acid?
(a) H3AsO4 (b) H2AsO4– (c) HAsO42- (d) AsO43-
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Question 6 of 15
6. Question
4 pointsIn an aqueous solution of triprotic acid H3A, which is true?
(a) [H+] = 3[A3-] (b) [H+] > 3[A3-]
(c) [H+] < 3[A3-] (d) [H+] = [OH–]
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Question 7 of 15
7. Question
4 pointsIf K1 and K2 be first and second ionization constant of H3PO4 and K1 >> K2, which is incorrect?
(a) [H+] = [H2PO4–] (b) [H+] =
(c) K2 = [HPO42-] (d) [H+] = 3[A3–]
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Question 8 of 15
8. Question
4 pointsIf the ionic product of water varies with temperature as follows and the density of water be nearly constant for this range of temperature, the process H+ + OH– ⇌ H2O is
Temp. oC 0 10 25 40 50 KW 0.114 x 10-14 0.292 x 10-14 1.008 x 10-14 2.91 x 10-14 5.474 x 10-14 Correct
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Question 9 of 15
9. Question
4 pointsWhen equal volumes of following solution are mixed, precipitation of AgCl (Ksp = 1.8 x 10-10) will occur only with
(a) 10-4M ; Ag+ and 10-4M ; Cl– (b) 10-5M ; Ag+ and 10-5M ; Cl–
(c) 10-6M ; Ag+ and 10-6M ; Cl– (d) 10-10M ; Ag+ and 10-10M ; Cl–
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Question 10 of 15
10. Question
4 pointsWhen ionic hydrides react with water, the products are
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Question 11 of 15
11. Question
4 pointsNH4NO3 will be maximum soluble in
(a) HCOOH + HCOONa buffer (b) NH4OH + NH4Cl buffer
(c) H2OPO–4 + H3PO4 buffer (d) In pure water
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Question 12 of 15
12. Question
4 pointsWith increasing temperature KW values increases. So which of the following statement is true?
(a) H2O → H+ + –OH this reaction is exothermic in nature
(b) Water is a strong electrolyte
(c) With increase of temperature pH of pure water increases
(d) Dissociation of water into H+ and OH– is an endothermic process
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Question 13 of 15
13. Question
4 pointsBuffer capacity of maximum
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Question 14 of 15
14. Question
4 pointsWhich of the following is false at half neutralization point of an acidic buffer solution?
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Question 15 of 15
15. Question
4 points10 c.c. of a 0.1M NaOH solution is added to 50 c.c. of a 1.1M acetic acid solution. What will be the pH of the resulting solution ? [Ka = 1.8 x 10-5]
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