Acid
-Base / Chemical Equilibrium
1. The pH of solution which contain 0.001 M H+
A.4
B. 3
C. 11
D. 1
2. The concentration of H+
ion in water
A. 0.0000001 mol/dm3
B. 0.0001 mol/dm3
C. 0.00001 mol/dm3
D. 0.001 mol/dm3
3. Conjugate acid of weak base is
the
A. Weakest acid
B.Strongest acid
C.Moderate
D.None of above
4. The pH of buffer is equal pKa
when concentration of salt is
A. Concentration
of salt and concentration of acid is
equal
B. Concentration
of salt is twice of concentration of acid
C. Concentration
of salt is half than concentration of acid
D. Concentration
of salt is less than concentration of acid
5. When the equilibrium constant
is greater than one . The equilibrium mixture contain concentration
A.
Reactant
is greater than product
B.
Product is greater than reactant
C.
Product is equal than reactant
D.
Product is twice of reactant
6. A ratio between concentrations
of reactant and product has greater than equilibrium constant at particular temperature.
The reaction proceed in a
A.
Dynamic Equilibrium
state
B.
Before the equilibrium state
C.
After the equilibrium
D.
None of above
7. The solubility of a sparingly
soluble salt is “S”
CdCl2 ↔Cd2+
+ Cl-1
The solubility product of salt
A.
S2
B.
2S3
C.
S3
D.
4S3
8. The equilibrium constant of reaction
at particular temperature is 0.25M
2HI ↔ H2
+ I2
The equilibrium
constant for will be
A . 0.25
B.
0.5
C.
4
D.
2.5
9. In Neutralization reaction of
strong acid HCl and strong base NaOH. 10 ml of 0.1M HCl required ___________of 0.05M of NaOH to complete
neutralization
A . 10 ml
B. 5 ml
C. 15 ml
D. 20 ml
10. How many milliliter of 0.05M NaOH
required to titrate of 0.1M HCl
A . 5ml
B. 10 ml
C. 20 ml
D. 15 ml
11.
Mixing 0.1 mol of NaOH, 0.1 mol of CH3COOH in 1 lit of water yields a solution, which:
A.
is acidic
B.
is neutral
C.
is basic
D.
may be acidic, basic or neutral depending upon temperature
12. The dissociation constant of
Pure water is 14
A.
Increases with increase in temperature
B.
Decreases with increase in temperature
C.
Is constant & is independent of
temperature
D.
increase in low temperature range but decreases in high temperature range
13.What
will be the change in the pH of water if 10-3 mol of NaOH is added
to 1.0 dm3 of water at 250C
A.
Increased by 3
B.
Increased by 4
C.
Decreased by 2
D.
Decreased by 4
14. When 1.0 cm3 of a weak acid solution is added
to 100cm3 of a buffer solution
A. the
volume of the resulting mixture will be 100cm3
B. there
will be almost no change in the pH of solution
C. the
pH of the solution will increase noticeably
D. the
pH of the solution will decrease noticeably
15. Which salt does not form an acidic solution in water?
A. MgCl2
B. Na2CO3
C. FeCl3
D. NH4NO3
16. Which species cannot act as a lewis acid ?
A. BF3
B. AlCl3
C. NH3
D. Fe2+
17. Three acids HA, HB & HC have the following Ka values
i. Ka of HA = 1 x 10-5
ii. Ka of HB = 2 x 10-5
iii. Ka HC =1 x
10-6
What is the correct increasing order of acidic strength?
A. HA<
HB<, HC
B. HC<
HA< HB
C. HC<
HB< HA
D. HB<
HA< HC
18. Which of the
following reagents could be added together to make a buffer solution?
A. NaOH
and CH3COOH
B. CH3COONa
and CH3COOH
C. NaOH & NaCH3COO
D.
NH4Cl and NH3
19. Suppose that the equilibrium A(aq) + 2B(aq) ↔ C (aq) , is
established from the original concentrations: [A]=[B]=[c]=0.10M at equilibrium
it is found that [C] =0.040M. What is the value of the equilibrium constant ,Kc
A. 1.1
B.
5.2
C. 0.19
D. 0.88
20. At a temperature
of about 4250C ,the equilibrium mixture contain [H2] =0.10 ,[I2]= 0.10 and
[HI]= 0.70. If suddenly 0.050 mol/dm3 of H2,
0.050 mol/dm3 of I2 0.350 mol/dm3 of HI were added , the
result would be that
A. more HI would from
B. the equilibrium would be shifted to the right
C. More H2 and I2 would from
D. No net Chemical change would occur
21. According to Le Chatelier’s principle , an increase in
temperature would result in all of following
EXCEPT :
A. an increase in the value of K
B. an increase in the value of rate
constant
C. an increase in the percentage decomposition
of N2O5
D. an increase in the value of
Activation energy
22. Given : 2A(g) + B(g) ↔ C (g)
. If the equilibrium is established by starting
with equal numbers of moles of B and of C , no A . At equilibrium it is
always true that :
A. [A]=[B]
B. [B] =[C]
C. [A] >[C]
D. [B]>[C]
23. Which of the following reaction has tendency to go to completion?
23. Which of the following reaction has tendency to go to completion?
A. H2 (g) + O2(g) ↔ 2H2O(g) K= 1.7x 1027
B. N2 + O2 ↔ 2NO K=
5.0 x 10-31
C. 2HF ↔ +
F2 + H2 K=
1.0x 10-13
D. 2NOCl ↔ 2NO + Cl2
K= 1.7x 10-4
24. The term “Ka for the ammonium ion” refers
directly to
A. NH3 + H2O ↔ NH+4 + OH-
B. NH3 + H3O+ ↔ NH+4 + H2O
C. NH+4 + H2O ↔ NH3
+ H3O+
D. NH+4 + OH-
↔ NH3
+ H2O
25. Which of the following solutions has the smallest [H3O+]?
A. 0.10M
HCl
B. 0.10M
H2SO4
C. 0.10M
HNO3
D. 0.10M
NH4Cl
sir pleasse send me the answer to these mcqs
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