DPP Volumetric Analysis JH Sir-3593

COURSE NAME : UMANG (UP)

TARGET

CHEMISTRY

JEE (ADVANCED) : 2014

DPP

DAILY PRACTICE PROBLEMS

DATE : 29.07.2013 to 03.08.2013

DPP NO. 39

* Marked Questions are having more th an one correct option. DPP No. # 39 1.

Maganese achieves its maximum oxidation state in which of these compounds : (A) MnO2 (B) Mn3O4 (C) KMnO4 (D) K2MnO4

2.

Oxidation number of underlined elements in N2O5, SO23 –, NH+4 are : (A) + 5, + 2, – 3 (B) + 6, – 2, + 3 (C) + 6, + 2, – 3

3.

4.

Phosphorous has the oxidation state of + 3 in : (A) Phosphorus acid (H3PO3) (C) Metaphosphoric acid (HPO3)

(D) + 5, + 4, – 3

(B) Orthophosphoric acid (H3PO4) (D) Pyrophosphoric acid (H4P2O7)

Which statement is wrong : (A) Oxidation number of oxygen is + 1 in peroxides (B) Oxidation number of oxygen is + 2 in oxygen difluroide (C) Oxidation number of oxygen is

!

1 in superoxides 2

(D) Oxidation number of oxygen is – 2 in most of its compounds 5.

The oxidation number and covalency of sulphur in the sulphur molecule (S8) are respectively : (A) 0 and 2

6.

(B) + 6 and 8

The oxidation number of oxygen in F2O is : (A) + 1 (B) – 2

(C) 0 and 8

(D) + 6 and 2

(C) + 2

(D) – 3

7.

Calculate individual and average oxidation number (if required) requir ed) of the marked element elem ent and also draw the structure of the following compounds or molecules : (1) Na2S2O3 (2) Na2S4O6 (3) H2SO5 (4) H2S2O8 (5) H2S2O7 (6) S8 2 – (7) HNO4 (8) C3O2 (9) OsO4 (10) PH3 (11) CrO4 (12) Cr2O72 – (13) CrO2Cl2 (14) CrO5 (15) Na2HPO4 (16) FeS2 (17) C6H12O6 (18) NH4NO3

8.

Calculate individual and average oxidation number (if required) requir ed) of the marked element elem ent and also draw the structure of the following compounds or molecules : (1) FNO3 (2) CaOCl2 (3) XeO3F2 (4) LiAlH4 (5) Na3AlF6 (6) P4 (7) O3 (8) I (IO3)3 (9) Fe3O4 (10) CsI3 (11) KO3 (12) O2F2 (13) H2SiF6 (14) H3PO3 (15) POCl3 (16) Si(OH)4 (17) Mg2C3 (18) CaC2 (19) Be2C

ETOOS ACADEMY Pvt. Ltd F-106, Road No.2 Indraprastha Industrial Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, +91-744-242-5022, 92-14-233303

PAGE NO. # 1

ANSWER KEY DPP No. # 39 1.

(C)

7.

(1) + 2 (6, – 2)

(2) + 5/2 (5, 5, 0, 0)

(3) + 6

(4) + 6 (+ 6, + 6)

(5) + 6 (+ 6, + 6)

(6) 0

(7) + 5

(8) 4/3 (+ 2, + 2, 0)

(9) + 8 (10) – 3 (11) + 6

(12) + 6 (+ 6, + 6)

(13) + 6

(14) + 6

(15) + 5

(16) + 2

(17) 0

(1) + 5

(2) 0 ( – 1, + 1)

(3) + 8

(4) + 3

(5) + 3

(6) 0 (0, 0, 0, 0) (7) 0 (0, – 1, + 1)

(8) + 3, + 5

(9)

8.

(11)

2.

!

(D)

1 3

(14) + 3

(17)

!

4 (0, ! 4, 0) 3

3.

(A)

4.

(A)

5.

8 ( "2, " 3) 3

(A)

(10)

6.

!

(C)

(18) – 3, + 5

1 3

(12) + 1 (+ 1, + 1)

(13) + 4

(15) + 5

(16) + 4

(18) – 1 ( – 1, – 1)

(19) – 4

ETOOS ACADEMY Pvt. Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303

PAGE NO. # 2

TARGET

CHEMISTRY


DPP



DATE : 05.08.2013 to 10.08.2013

DPP NO. 40 TO 42


Identify the reactants, if any, oxidized or reduced. (a) NaH + H2O !" NaOH + H2 (b) 2FeCl3 + H 2S !" 2FeCl2 + S + 2HCl (c) 3Mg + N2 !" Mg 3N2 (d) AgCN + CN – !" Ag(CN)2 – (e) SnCl2 + Br2 !" SnCl 2.Br 2 !" (f) AlCl3 + K Al + 3KCl (g) 2CuSO4 + 4KI !" Cu 2I2 + K 2SO 4 + I2 (h) NH4NO 2 !" N 2 + 2H 2O (i) CaC2 + 2H2O !" Ca(OH)2 + C2H2 (j) SnS2 + S –2 !" SnS 3 –2 (k) 3O2 !" 2O 3

2.

Select the oxidants and reductants in the given reactions . (a) Ag(NH3) 2+ + 2H+ Ag + + 2NH4+ !" (b) KIO3 + 5KI + 6HCl !" 3I 2 + 6KCl + 3H 2O (c) 2CuSO4 + SO2 + 2KBr + 2H2O !" 2CuBr + 2H2SO 4 + K 2SO 4 (d) C2H4 + Br 2 !" C2H4Br 2 (e) 2I – + H 2O2 !" 2OH – + I 2 (f) Si + 2KOH + H2O !" K2SiO 3 + 2H 2 (g) 2Cu+2 + 4I – !" Cu 2I2 + I2

3.

Balance the following equation using desired medium – (a) C2H5OH + Cr2O72 – + H+ !" Cr 3+ + C2H4O + H2O (b)

Sn(OH)3 – + Bi(OH)3 + OH –

(c)

IO 3 – + N 2H4 + HCl

(d)

Hg 2Cl 2 + NH3

(e)

Zn + NO3 – + H +

(f)

I2 + NO3 – + H+

(g)

MnO 4 – + SO22 – + H2O

(h)

H2O2 + ClO2 + OH –

(i)

ClO – + CrO 2 – + OH –

(j)

Cl 2 + KOH

!"

!" Hg

!"

!"

!"

!" Sn(OH)

2 – 6

+ Bi

N2 + ICl2 – + H2O

+ HgNH2Cl + NH 4Cl

Zn 2+ + NH4+ + H2O

IO 3 – + NO 2 + H2O !"

!"

!"

MnO 2 + SO 42 – + OH –

ClO 2 – + O2 + H2O Cl – + CrO42 – + H2O

KClO 3 + KCl + H 2O ETOOS ACADEMY Pvt. Ltd

F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303

PAGE NO. # 1

DPP No. # 41 Balance the following equation using desired m edium 1.

H2O2 + KMnO4

MnO 2 + KOH + O 2 + H2O

2.

HNO 2 + KMnO4 + H 2SO 4

3.

N2H4 + AgNO 3 + KOH

4.

P + HNO3

5.

K2Cr 2O7 + HCl

6.

MnO 4 – + C 2O42 – + H+

7.

Cr 2O72 – + C 2O42 – + H +

8.

KMnO 4 + H 2S + H2SO 4

9.

Cu(NH3)4Cl 2 + KCN + H2O

10.

Ag + KCN + H 2O + O2

!" KAg(CN)

11.

Fe 3O4 + MnO4 – + H2O

!"

12.

C2H5OH + MnO4 – + OH –

13.

Cr 2O72 – + SO32 – + H +

14.

ClO 3 – + SO 2 + H +

15.

Mn 2+ + S 2O82 – + H 2O

!"

!"

!"

!"

HNO 3 + KMnO 4 + K 2SO 4 + H2O

N2 + Ag + KNO3 + H2O

HPO 3 + NO + H2O KCl + CrCl3 + H 2O + Cl2

!"

!"

CO 2 + Mn2+ + H 2O Cr 3+ + CO 2 + H2O

!"

!"

!"

K2Cu(CN)3 + NH 3 + KCNO + NH 4Cl + KCl 2

+ KOH

Fe 2O3 + MnO2 + OH –

!"

!"

!"

KHSO 4 + MnSO4 + S + H 2O

C2H3O – + MnO2 + H2O

Cr 3+ + SO 42 – + H2O

ClO 2 + HSO4 –

!"

MnO 4 – + HSO4 – + H+

DPP No. # 42 *

Equivalent weight of any substance is the weight in gram which combines with 1 gram of hydrogen, 8 grams of oxygen, 35.5 grams of Cl and 108 grams of Ag.

*

Equivalent weight =

1.

The equivalent weight of a metal is 36. What weight of the metal would give 9.322 gm of its chloride?

2.

On heating 5 × 10 –3 equivalent of CaCl 2.xH 2O, 0.18 gm of water is obtained, what is the value of x ?

3.

The equivalent weight of a metal is double that of oxygen. How many times is the weight of its oxide greater than the weight of the metal ?

4.

0.224 gm of a metal when dissolved in dilute acid liberates 285 cc of hydrogen, measured at 17ºC and 78 cm of mercury pressure. Find the equivalent weight of the metal.

5.

1.82 g of a metal required 32.5 mL of N HCl to dissolve it. What is equivalent weight of metal ?

6.

The equivalent weight of a metal is 30. W hat volume of chlorine would be liberated at 27ºC and 750 mm pressure by 0.6 gm of the metal ? [Aqueous tension at 27ºC = 26.6 mm]

7.

The molecular formula of an oxide of an element X is XmOn what is the equivalent weight of themetal? [Given atomic weight of X = a]

8.

12 g of an element combines with 32 g of oxygen. What is the equivalent weight of the element if the equivalent weight of oxygen is 8 ?

9.

Equivalent weight of sulphur in SCl2 is 16, what is the equivalent weight of S in S2Cl 2 ? [S = 32 , Cl = 35.5]

10.

1.60 gm of a m etal were dissolved in HNO3 to prepare its nitrate. The nitrate was strongly heated to give 2 g oxide. Calculate equivalent weight of metal.

11.

From 3.36 gm of Fe, 4.80 gm of iron oxide is obtained. What is the equivalent weight of Fe?

12.

1.0 g of metal nitrate gave 0.86 g of metal sulphate. Calculate equivalent weight of metal.

13.

An element forms two oxides, the weight ratio composition in them, A : O = x : y in the first oxide and y : x in the second oxide. If the equivalent weight of A in the first oxide is 10.33, Calculate the equivalent weight of A in the second oxide.

Molecular weight ' n' factor


PAGE NO. # 2

ANSWER KEY DPP No. # 40 1.

Rxn. No. (a) Oxidized : NaH, Reduced : H2O,

(b) (c) H2S, Mg, FeCl3, N2

2.

(a) (c) (e) (g)

3.

(a) 3C2H5OH + Cr 2O72 – + 8H + !" 2Cr 3+ + 3C 2H4O + 7H2O

not CuSO 4-oxidant, SO2 reductant H2O2-oxidant, I – reductant Cu ++-oxidant, I – reductant

(d) none, none,

(e) (f) SnCl2, K, Br2, AlCl3,

(g) (h) KI, NH4+, CusO4, NO 2 – ,

(i) none, none,

(j) (k) none none. none, none

(b) KIO 3-oxidant, I – reductant (d) Br 2-oxidant, C2H4 reductant (f) KOH-oxidant, Si reductant

(b) 3Sn(OH)3 – + 2Bi(OH) 3 + 3OH – !" 3Sn(OH)62 – + 2Bi (c) IO3 – + N 2H4 + 2HCl !" N 2 + ICl2 – + 3H 2O (d) 2Hg2Cl 2 + 4NH 3 !" 2Hg + 2HgNH 2Cl + 2NH 4Cl (e) 4Zn + NO3 – + 10H + !" 4Zn2+ + NH4+ + 3H 2O (f) I2 + 10NO3 – +8H + !" 2IO 3 – + 10NO2 + 2H2O (g) 2MnO4 – + 3SO22 – + H2O !" 2MnO2 + 3SO42 – + 2OH – (h) H2O2 + 2ClO2 + 2OH – !" 2ClO2 – + O 2 + 2H2O (i) 3ClO – + 2CrO2 – + 2OH – !" 3Cl – + 2CrO42 – + H2O (j) 3Cl2 + 5KOH !" KClO3 + 5KCl + 3H 2O

DPP No. # 41 1.

3H 2O2 + 2KMnO4 !" 2MnO2 + 2KOH +3O 2 + 2H 2O

2.

5HNO 2 + 2KMnO4 + 3H 2SO 4 !" 5HNO3 + 2KMnO4 + K 2SO 4 + 3H2O

3.

N2H4 + 4AgNO3 + 4KOH !" N 2 + 4Ag + 4KNO 3 + 4H2O

4.

3P + 5HNO3 !" 3HPO 3 + 5NO + H2O

5.

K2Cr 2O7 + 8HCl !" 2KCl + 2CrCl 3 + 7H2O + 3Cl2

6.

2MnO 4 – + 5C2O42 – + 16H+ !" 10CO2 + 2Mn2+ + 8H 2O

7.

Cr 2O72 – + 3C 2O42 – + 14H+ !" 2Cr 3+ + 6CO 2 + 7H 2O

8.

2KMnO 4 + 5H2S + 4H2SO 4 !" 2KHSO 4 + 2MnSO4 + 5S + 8H 2O

9.

2Cu(NH3)4Cl 2 + 7KCN + H 2O !" K2Cu(CN)3 + 6NH3 + KCNO + 2NH 4Cl + 2KCl

10.

4Ag + 8KCN + 2H 2O + O2 !" 4KAg(CN)2 + 4KOH

11.

6Fe 3O4 + 2MnO4 – + H 2O !" 9Fe2O3 + 2MnO2 + 2OH –

12.

3C 2H5OH + 2MnO4 – + OH – !" 3C 2H3O – + 2MnO2 + 5H 2O

13.

Cr 2O72 – + 3SO 32 – + 8H + !" 2Cr3+ + 3SO 42 – + 4H2O

14.

2ClO3 – + SO 2 + H+ !" 2ClO2 + HSO 4 –

15.

2Mn 2+ + 5S2O82 – + 8H 2O !" 2MnO4 – + 10HSO4 – + 6H

DPP No. # 42 1.

4.6935 gm

2.

x= 4

3.

1.5

4.

9.105

5.

56

6.

0.2584 lit

7.

m × a/2n

8.

3

9.

32

10.

32

11.

18.67

12.

38

13.

6.2


PAGE NO. # 3

TARGET

CHEMISTRY


DPP



DATE : 12.08.2013 to 17.08.2013

DPP NO. 43 & 44


White phosphorus re acts caustic soda, the products are PH3 and NaH2PO2. The reaction is an example of : (A) Oxidation

2.

(B) Reduction

The reaction 3 ClO – (aq) !" ClO 3 – (aq) + 2Cl – (aq) is an example of : (A) Oxidation

3.

(B) Reduction

"

V 2O3

"

"

Na +

(C) Zn2+

"

(D) CrO42 –

Zn

(B) MnO4 – + C2O42 –

Mg 3N2

(C) CuSO4 + KI

"

Cr 2O72 –

"

2CuI + I2 + K 2SO 4

(D) AgCl + NH3

"

"

Mn 2+ + CO 2

[Ag(NH3) 2]Cl

Which of the following can show disporoportionation reaction : (A) ClO4 –

6.

(B) Na

Which of the following is not a redox reaction? (A) Mg + N2

5.*

(C) Disproportionation (D) Decomposition

Which of the following changes does not involve either oxidation or reduction : (A) VO2+

4.

(C) Disproportionation (D) Neutralisation

(B) Cl –

(C) ClO2 –

(D) ClO3 –

Identify the oxidant and the reductant in the f ollowing reactions : (a) KMnO4 + KCl + H2SO 4 !" MnSO 4 + K 2SO 4 + H 2O + Cl2 (b) FeCl2 + H 2O2 + HCl !" FeCl3 + H 2O (c) Cu + HNO 3 (dil) !" Cu (NO3)2 + H 2O + NO (d) Na2HAsO 3 + KBrO3 + HCl !" NaCl + KBr + H 3AsO 4 (e) I2 + Na 2S2O3 !" Na 2S4O6 + NaI

7.

Balance the following redox equations and determine the valency factor (n-factor) for oxidant and reductant involved in the reactions : (i) K2Cr 2O7 + H2O2 + H2SO 4 !" K2SO 4 + Cr 2(SO 4)3 + H2O + O2 (ii) Zn + NaNO3 + NaOH !" Na 2ZnO 2 + H 2O + NH3 (iii) Al !" [Al(OH)4] – + H 2

(basic)

(iv) Cu3P + Cr2O72 – !" Cu 2+ + H 3PO 4 + Cr3+ + H2O

(acidic)

(v) ClO3 – + Fe2+ + H + !" Cl – + Fe3+ + H2O (vi) N2O4 + BrO 3 – !" NO 3 – + Br – (vii) S2O32 – + Sb2O5 !" SbO + H 2SO 3 (viii) Cr 2O72 – + I – + H + !" Cr 3+ + I 2 + H2O (ix) IO4 – + I – + H + !" I2 + H 2O


PAGE NO. # 1

DPP No. # 44 1.

In the reaction 2S2O32 – + I 2 !" S4O62 – + 2I –, the equivalent wt. of S4O62 – is equal to : (A) Mol wt.

2.

(B) Mol. wt./2

(D) Mol. wt./6

Equivalent weight of NH 3 in the change N !" NH 3 is : (A) 17/6

3.

(C) 2 × Mol. wt.

(B) 17

(C) 17/2

(D) 17/3

The molecular weight of the compounds (a) Na2SO4, (b) Na3PO4. 12H2O and (c) Ca3(PO 4)2 respectively are X, Y and Z. T he correct set of their equivalent weights will be :

4.

(A) (a)

Y Z X (b) (c) 3 6 2

(B) (a) x (b)

Y Z (c) 3 3

(C) (a)

Z X (b) Y (c) 3 2

(D) (a) X (b) Y (c) Z

In the following reaction : 3Fe + 4H2O !" Fe 3O4 + 4H2, if the atomic weight of iron is 56, then its equivalent weight will be : (A) 42

5.

(B) 21

(C) 63

(D) 84

When one mole NO3 – is converted into 1 mole NO2, 0.5 mole N2 and 0.5 mole N 2O respectively, it accepts x, y and z mole of electrons. Then, x, y and z are respectively : (A) 1, 5, 4

6.

(B) 1, 2, 3

(C) 2, 1, 3

(D) 2, 3, 4

In the equation, SnCl2 + 2HgCl 2 !" Hg 2Cl 2 + SnCl4 : The equivalent weights of Stannous chloride (molecular weight = 190) will be : (A) 190

7.

(B) 95

(C) 47.5

(D) 154.5

(C) 329

(D) None of these

In the reaction 2CuSO 4 + 4KI !" 2CuI + I2 + 2K2SO 4 the equilvalent weight of CuSO4 will be : (A) 79.75

8.

(B) 159.5

In the f ollowing half-reaction, hydrazine is oxidized to N2. N2H4 + OH – !" N2 + H2O + e – The equivalent weight of N2H4 (hydrazine) is : (A) 8

(B) 16

(C) 32

(D) 64


PAGE NO. # 2

ANSWER KEY DPP No. # 43 1. 6.

(C) (a)

2.

(C)

(+ 7)

3.

(D)

4.

( – 1)

5.*

(CD)

(+ 2)

KMnO 4 + KCl + H 2SO 4

!"

(+ 7)

(0)

MnSO 4 + K 2SO 4 + H2O + Cl2 (+ 2)

KMnO 4 (oxidant)

!"

( – 1)

MnSO 4 (reduction half) (0)

KCl (reducant) (b)

(D)

(+ 2)

!"

( – 1)

Cl 2 (oxidant half) (+ 3)

FeCl2 + H 2O2 + HCl

( – 2)

!"

FeCl3 + H2O

!"

FeCl3 (oxidation half)

!"

H2O2 – (reduction half)

(+ 2)

(oxidant half)

(+ 3)

FeCl2 (reductant) ( – 1)

H2O2 (oxidant) (c)

(0)

(+5)

2+

Cu + HNO3 (dil)

!"

Cu (NO3)2 + H 2O + NO

Cu (reductant)

!"

Cu (NO3)2 (oxidation half)

(0)

2+

+5

+2

HNO 3 (oxidant) (d)

+3

!"

NO (reduction half)

+5

– 1

Na 2HAsO3 + KBrO3 + HCl

+5

Na 2HAsO3 (reductant)

!"

+5 !"

KBr

+2

+ 2.5

I2+ Na 2S2O3

!"

0

– 1

Na 2S4O6 + NaI – 1

I2 (oxidant)

!"

+2

NaI (reduction half) +2.5

Na 2S2O3(reducant) 7.

H3AsO 4 (oxidation half) – 1

KBrO 3 (oxidant) 0

+5

NaCl + KBr + H 3AsO 4

!"

+3

(e)

2+

!"

Na 2S4O6(oxidant half)

(i) K2Cr 2O7 + 3H 2O2 + 4H2SO 4 !" K2SO 4 + Cr2(SO 4)3 + 7H 2O + 3O2 v.f. = 6 v.f. = 2 (ii) 4Zn + NaNO 3 + 7NaOH = 4Na2ZnO 2 + 2H2O + NH 3 v.f. = 2 v.f. = 8 (iii) 2OH – + 6H2O + 2Al !" 3H2 + 2(Al(OH) 4] – v.f. = 3 2 – (iv) 6Cu3P + 11Cr 2O7 + 124H+ !" 18Cu 2+ + 6H3PO 4 + 22Cr3+ + 53H2O v.f. = 11 v.f. = 6 + – (v) 6H + ClO3 + 6Fe2+ !" Cl – + 6Fe3+ + 3H 2O v.f. = 6 v.f. = 1 (vi) 3N2O4 + BrO3 – + 3H2O !" 6NO 3 – + Br – + 6H + v.f. = 2 v.f. = 6 2 – (vii) 3S2O3 + 2Sb2O5 + 6H+ + 3H2O !" 4SbO + 6H2SO 3 v.f. = 4 v.f. = 6 2 – (viii) Cr 2O7 + 6I – + 14H + !" 2Cr 3+ + 3I2 + 7H 2O v.f. = 6 v.f. = 1 – – (ix) IO4 + 7I + 8H+ !" 4I 2 + 4H2O v.f. = 7 v.f. = 1

DPP No. # 44 1. 8.

(B) (A)

2.

(D)

3.

(A)

4.

(B)

5.

(A)

6.

(B)

7.

(B)


PAGE NO. # 3


TARGET

CHEMISTRY


DPP


DATE : 26.08.2013 to 31.08.2013

DPP NO. 45 & 47


Suppose a compound contains atoms A, B and C. The oxidation num ber of A is +2, B is +5 and C is – 2. The possible formula of the compound would be : (A) ABC 2 (B) A2(BC 3)2 (C) A3(BC 4)2 (D) A3(B 4C) 2

2.

50 mL of 5.6% KOH (w/v) is added to 50 mL of a 5.6% HCI (w/v) solution. The resulting solution will be (A) neutral (B) alkaline (C) strongly alkaline (D) acidic

3.

Number of moles of electrons taken up when 1 mole of NO3! ions is reduced to 1 mole of NH2OH is : (A) 2 (B) 4 (C) 5 (D) 6

4.

As 2O3 is oxidised to H 3AsO 4 by KMnO4 in acidic medium. Volume of 0.02M KMnO4 required for this purpose by 1mmol of As2O3 will be : (A) 10 mL (B) 20 mL (C) 40 mL (D) 80 mL

5.

A 25-mL HCl solution conta ining 3.65 g HCl/L is neutralized by 50 mL an NaOH solution. Again, 25 mL of the same NaOH solution neutralized by 50 mL of an H2SO 4 solution of unknown strength.The normality of the H2SO 4 solution is (A) 0.25 N (B) 0.025 N (C) 0.05 N (D) 0.50 N

6.

The total volume of 0.1 M KMnO4 solution that are needed to oxidize 144 mg of ferrous oxalate and 152 mg of ferrous sulphate in a mixture in acidic medium is : (A) 5 mL (B) 2 mL (C) 8 mL (D) None of these

7.

The equivalent weight of a metal is double than of oxygen. How many times is the weight of it’s oxide greater than the weight of the metal ? (A) 1.5 (B) 2 (C) 3 (D) 4

8.

How much mass of K2C2O4 is require for complete oxidation in titration with 0.2 M, KMnO4 . The volume of KMnO4 used in acidic medium is 500 ml and calculate the volume of CO2 obtained at S.T.P. in the reaction.

9.

The percent yield for the following reaction carried out in carbon tetrachloride (CCI4) solution is 80% Br2 + CI2 " "# 2BrCI (a) What amount of BrCI would be formed from the reaction of 0.025 mol Br 2 and 0.025 mol CI2? (b) What amoumt of Br2 is left unchanged?

10.

–

24 ml of a solution of Fe2+ ions was titrated with a solution of the oxidizing agent Cr2O72 . 40 ml of 0.02 M K2Cr2O7 solution was required.What is the molarity of the Fe2+ solution.


PAGE NO. # 1

DPP No. # 46 1.

25 mL of 2N HCl, 50 mL of 4N HNO3 and x mL of 2M H2SO4 are mixture together and the total volume is made up to 1 L after dilution. 50 mL of this acid mixture completely reacted with 25 mL of a 1N Na2CO3 solution. The value of x is : (A) 250 mL (B) 62.5 mL (C) 100 mL (D) None of these

2.

One mole of H2SO 4 will exactly neutralize (A) 4 moles of an ammonia solution (C) 3 moles of Al (OH) 3

(B) 1 mole of Ba(OH)2 (D) 0.5 mole of Ba(OH)2

3.

When ferrous oxalate is titrated against K2Cr 2O7, meq of Fe2+ , C 2O42! and Cr 2O72! in this redox reaction are x, y and z respectively. Then (A) x = y (B) x + y = z (C) x + 2y = z (D) 2x + 6y = 6z

4.

What volume of 2N K 2Cr 2O7 solution is required to oxidise 0.81 g of H 2S in acid medium? (A) 47.8 ml (B) 23.8 ml (C) 40 ml (D) 72 ml

5.

The number of moles of KMnO4 that will be needed to react with one mole of sulphite ion in acid solution is (A) 4/5 (B) 3/5 (C) 1 (D) 2/5

6.

4 mole of a mixture of Mohr’s salt and Fe2(SO4)3 requires 500 mL 1M K2Cr2O7 for complete oxidation in acidic medium. The mole % of the Mohr ’s salt in the mixture is : (A) 25 (B) 50 (C) 60 (D) 75

7.

A solution of Na2S2O3 is standardized iodometrically against 0.167 g of KBrO3. This process requires 50 mL of the Na2S2O3 solution. What is the normality of the Na2S2O3 ? (A) 0.2 N (B) 0.12 N (C) 0.72 N (D) 0.02 N

8.

In an iodometric estimation, the following reaction occur 2Cu2+ + 4I " I2 + 2Na2S2O3 " "# Cu2I2 ; "# 2NaI + Na2S4O6 0.12 mole of CuSO4 was added to excess of KI solution and the liberated iodine required 120 m L of hypo. The molarity of hypo solution was : (A) 2 (B) 0.20 (C) 0.1 (D) 1.0 –

9.

It requires 20 ml of 1 M X3+ to titrate 10 ml of 2 M Sn 2+ to Sn4+ . What is the oxidation state of the 'X' in the product.

10.

25 ml of a solution of H2S (it convert into S) was titrated with a solution of the oxidizing agent Cr2O72 . 100 ml of 0.01 M K2Cr2O7 solution was required. What is the molarity of the H2S solution ?

11.

How many ml of 0.3M K2Cr 2O7 (acidic) is required for complete oxidation of 10 ml of 0.1 M FeC2O4 solution.

12.

Calculate the mass of oxalic acid which can be oxidized by 100ml of MnO4 solution, 10ml of same solution of MnO4 is capable of oxidizing 50ml of 1 N I to I2.

–

–

–

13.

–

Butane, C4H10, burns with the oxygen in air to give carbon dioxide and water. What is the amount (in moles) of carbon dioxide produced from 0.15 mol C 4H10 ? C4H10(g) + O2(g) "# CO2(g) + H2O(g) (not balanced)

DPP No. # 47 1.

2.

A 10-volume H2O2 solution is equal to (A) 3% (w/v) H 2O2 (B) 30 g/L H2O2

(C) 1.76 N

(D) all of these

A 5.0-mL solution of H 2O2 liberates 0.508 g of iodine from an acidified Kl solution. The volume strength of the H2O2 solution at STP is approximately : (A) 4.00 (B) 4.5 (C) 6.05 (D) 5.5 ETOOS ACADEMY Pvt. Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303

PAGE NO. # 2

3.

What volume of O2 measured at standard conditions will be formed by the action of 100 m l of 0.5 N KMnO 4 on hydrogen peroxide in an acid solution? The skeleton equation for the reaction is KMnO 4 + H 2SO 4 + H2O2 # K 2SO 4 + MnSO4 + H2O + O2 (A) 0.12 l (B) 0.28 l (C) 0.56 l (D) 1.12 l

4.

100 ml of 0.1M NaAl(OH)2CO 3 is neutralised by 0.25 N HCl t o form NaCl, AlCl3 and CO2. Volume of HCl required is (A) 10 mL (B) 40 mL (C) 100mL (D) 160 mL

5.

100 mL of 0.1N I2 oxidizes Na2S2O3 in 50 ml solution to Na 2S4O6. The normality of this hypo solution against KMnO4 (which oxidizes it to Na 2SO 4) would be (A) 0.1 (B) 0.2 (C) 1.0 (D) 1.6.

6.

Which of the following has two unpaired electrons ? (A) Si, Mg (B) S, Mg (C) S, Si

(D) S, Fe.

Total number of electrons contained in all the p-orbitals of bromine is: (A) 5 (B) 17 (C) 19

(C) 23

The number of unpaired electrons in Mn2+ is: (A) 5 (B) 3

(D) 1

7.

8.

9.*

(C) 4

1M 100 ml NaCl is mixed with 3M 100 ml HCl solution and 1M 200 ml CaCl2 solution. Find the ratio of the concentration of cation and anion. (A) The ratio of concentration of cation and anion = 3/4M (B) The ratio of concentration of cation and anion = 2 M (C) [Cl ] = 2 M (D) [Cl ] = 3/2 M –

–

Subjective 10. The reaction Cl2(g) + S2O32- # SO 42- + Cl- is to be carried out in basic medium. Starting with 0.15 mol of Cl2, 0.01 mol S2O32- and 0.3 mol of OH -, how many moles of OH- will be left in solution after the reaction is complete. Assume no other reaction occurs. 11.

A piece of brass weighing 304.8 mg was dissolved and prepared for iodometric titration. Excess K$ was added and the liberated iodine required 30.0 ml of 0.08 M hypo. Find the % of Cu in the brass.

ANSWER KEY : DPP No. # 45 1. 8.

(C) 2. (D) 3. (D) 41.5 gm K2CO 4 ; 11.2 lt CO 2 .

9.

(a)

4.

(C)

5.

(B)

6.

(C)

7.

(A)

(D) 12.

6. (D) 22.5 g 13.

7. (B) 0.60 mol CO2

(D)

6.

7.

Br2 + CI2 " "# 2BrCI 1 mol 1mol 2mol 0.025 0.025 0.050 mol BrCI = 0.050 mol

(b) Theoretical yield of

0.05 % 80 = 0.04 mole 100 Br2 left unreacted = 0.025 – 0.02 = 0.005 mol.

actual yield is = 10.

0.2 M.

DPP No. # 46 1. 8.

(B) (D)

2. 9.

(B) +1

3. 10.

(B) 4. 0.12 M. 11.

(B) 5. 1.67 ml .

DPP No. # 47 1. 8.

(D) (A)

2. 9.*

(B) (AC)

3. 10.

(C) 4. (D) 0.2 moles OH . 11.

5. 50%

(C)

(B)


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DPP Volumetric Analysis JH Sir-3593

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