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1

AIPMT 2001

Solubility of M2S salt is 3.5 $$\times$$ 10$$-$$6 then find out solubility product.
A
1.7 $$\times$$ 10$$-$$6
B
1.7 $$\times$$ 10$$-$$16
C
1.7 $$\times$$ 10$$-$$18
D
1.7 $$\times$$ 10$$-$$12

Explanation

M2S ⇌ 2M+ + S2–

Ksp = [M+]2[S2–] = (2s)2(s) = 4s 3

Ksp = 4(3.5 × 10–6)3 = 1.7 × 10–16
2

AIPMT 2001

In HS$$-$$, I$$-$$, R $$-$$ NH2, NH3 order of proton accepting tendency will be
A
I$$-$$ > NH3 > R $$-$$ NH2 > HS$$-$$
B
NH3 > R $$-$$ NH2 > HS$$-$$ > I$$-$$
C
R $$-$$ NH2 > NH3 > HS$$-$$ > I$$-$$
D
HS$$-$$ > R $$-$$ NH2 > NH3 > I$$-$$

Explanation

Strong base has higher tendency to accept the proton. Increasing order of base and hence the order of accepting tendency of proton is

R $$-$$ NH2 > NH3 > HS$$-$$ > I$$-$$
3

AIPMT 2000

Equilibrium constant Kp for following reaction
MgCO3(s) $$\rightleftharpoons$$ MgO(s) + CO2(g)
A
Kp = PCO2
B
Kp = PCO2 $$\times$$ $${{{P_{C{O_2}}} \times {P_{MgO}}} \over {{P_{MgC{O_3}}}}}$$
C
Kp = $${{{P_{C{O_2}}} + {P_{MgO}}} \over {{P_{MgC{O_3}}}}}$$
D
Kp = $${{{P_{MgC{O_3}}}} \over {{P_{C{O_2}}} + {P_{MgO}}}}$$

Explanation

Kp = PCO2

As solids do not exert pressure, so their partial pressure is taken as unity.
4

AIPMT 2000

Which statement is wrong about pH and H+?
A
pH of neutral water is not zero.
B
Adding 1 N solution of CH3COOH and 1 N solution of NaOH, pH will be seven.
C
[H+] of dilute and hot H2SO4 is more than concentrated and cold H2SO4
D
Mixing solution of CH3COOH and HCl. pH will be less than 7.

Explanation

CH3COOH is weak acid while NaOH is strong base, so one equivalent of NaOH can not be neutralized with one equivalent of CH3COOH. Hence the solution of one equivalent of each does not have pH value as 7. Its pH will be towards basic side as NaOH is a strong base hence conc. of OH will be more than the conc. of H+.

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