問題一覧
1
Those substances which dissociate into their ions on dissolving in water
electrolyte
2
Those substances which dissociate into ions in their solutions
electrolyte
3
Which type of electrolyte is AgNO3
strong
4
Which type of electrolyte is sodium acetate
strong
5
Which type of electrolyte is ammonium chloride
strong
6
Which type of electrolyte is KCN
strong
7
Which type of electrolyte is ammonium hydroxide
weak
8
Which type of electrolyte is HCN
weak
9
Which type of electrolyte is magnesium hydroxide
weak
10
Which type of electrolyte is copper hydroxide
weak
11
Which type of electrolyte is barium hydroxide
weak
12
Which type of electrolyte is AgCl
weak
13
Amy equilibrium involving ions is called
ionic equilibrium
14
On dilution degree of dissociation of weak electrolyte
increases
15
On dilution concentration n of weak electrolyte
decreases
16
2
17
3
18
0.31
19
0.095
20
2
21
If a strong electrolyte containing at least one common ion is added to a solution of weak electrolyte then degree of dissociation of weak electrolyte
decreases
22
In an Aqueous solution of HCN,NaCl aqueous solution is mixed then common ion effect will take place or not
no
23
10-⁴
24
2
25
2
26
Water is a very weak electrolyte which undergo self ionization
true
27
In pure H2O at 25°C concentration of [H+]
is
10-⁷
28
In pure H2O at 25°C value of Kw is
10-¹⁴
29
pH scale was given by sorenson
t
30
Calculate pH of pure water at 25°C
7
31
Calculate pH of 0.01M HCl at 25°C
2
32
Calculate pH of 10-¹⁰M HCl(aq) solution at 25°C
7
33
Value of log 5
0.7
34
Calculate pH of 10-²M NaOH(aq) solution at 25°C
2
35
Calculate pH of 10-⁷M NaOH(aq) solution at 25°C
7.3
36
Calculate pH of 10-⁸M HCl(aq) solution at 25°C
6.97
37
Calculate pH of 10-⁸M KOH(aq) solution at 25°C
7.03
38
Calculate pH of 10-⁷M HNO3(aq) solution at 25°C
6.7
39
Calculate pH of 10-¹⁰M NaOH(aq) solution at 25°C
7
40
3
41
2
42
Calculate concentration of [H+] in a solution if pH of solution is 2.4
4*10-³
43
Calculate concentration of [H+] in a solution if pH of solution is 3.3
5*10-⁴
44
3
45
4
46
Calculate pH of 0.1M Acetic acid (Ka=10-⁵) solution at 25°C
3
47
Calculate pH of 0.01M Ammonium hydroxide (Kb=10-⁶) solution at 25°C
10
48
Calculate pH of 0.01M NaOH(aq) solution at 25°C
2
49
Calculate pH of 0.005M sulphuric acid solution at 25°C
3
50
Calculate pH of 0.1M Ammonium hydroxide (Kb=10-⁶) solution at 25°C
11
51
1
52
3
53
If Ka1& Ka2 values differ by 10³ or more than the smaller k will be neglected
t
54
3
55
4
56
4
57
1
58
2
59
Refresh
t
60
Recheck
t
61
4
62
Salt hydrolysis is reverse reaction of
neutralization
63
The breaking up of salt in presence of water to generate respective acid or base is called
salt hydrolysis
64
Weaker part of a salt undergo _____ and stronger part decide the_____ of solution
hydrolysis,pH
65
4
66
3
67
1
68
4
69
3
70
The solution which pH does not change on addition of small amount of acid or base are called as
buffer
71
Weak acid with its salt with strong base constitutes
acidic buffer
72
Weak base with its salt with strong acid constitutes
basic buffer
73
3
74
2
75
Theory given by
arhennius
76
Theory given by
bronsted
77
Theory given by
Lewis
78
Conjugate base of weak acid is strong base and vice versa
t
79
4
80
3
81
Addition of sodium acetate solution to acetic acid causes the following change
pH increases
82
4
83
4
84
yes
85
2
86
2
87
4
88
On increasing temperature of a weak acid dissociation_____ and pH _____
increases ,decreases
89
100 ml of 0.1M acetic acid started with 0.1M sodium hydroxide.
i)Calculate pH at half neutralization point
Or
Calculate pH when half of acids gets neutralized
1
90
Relation between solubility product and solubility for:
Hydrolysis of magnesium chloride
1
91
Calculate relation between solubility and solubility product for barium phosphate
1
92
Calculate solubility of silver chloride in pure water (Ksp=4x10-⁶)
1
93
Calculate solubility of silver chloride in (Ksp=4x10-⁶)
in 0.1M NaCl solution
1
94
Calculate solubility of silver iodide in 0.01N NaI solution ( Ksp=10-⁹)
1
95
3
96
Solubility product of BaCl2 is 4x10- ⁹ its solubility in moles per litre would be
1
97
Solubility product of AgCl is 2.8x 10-¹⁰ at 25°C calculate solubility of salt in 0.1M AgNO3 solution in moles /litre
1) 2.8x10-⁹
2)2.8x10-¹⁰
3) 3.2x10-⁹
4)3.2x10-¹²
1
98
Calculate solubility of barium chloride in 0.01 M NaCl solution in moles per litre
(Ksp=4x10-¹⁰)
1) 2x10-⁹
2)2.8x10-¹⁰
3) 4x10-⁶
4)3.2x10-¹²
3
99
Calculate solubility of Mg(OH)2 in 0.1 M NaOH solution
1) 10-¹⁰
2)10-⁹
3) 10-⁸
4)10-⁶
1
100
1) yes
2) no
2
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66問 • 1年前問題一覧
1
Those substances which dissociate into their ions on dissolving in water
electrolyte
2
Those substances which dissociate into ions in their solutions
electrolyte
3
Which type of electrolyte is AgNO3
strong
4
Which type of electrolyte is sodium acetate
strong
5
Which type of electrolyte is ammonium chloride
strong
6
Which type of electrolyte is KCN
strong
7
Which type of electrolyte is ammonium hydroxide
weak
8
Which type of electrolyte is HCN
weak
9
Which type of electrolyte is magnesium hydroxide
weak
10
Which type of electrolyte is copper hydroxide
weak
11
Which type of electrolyte is barium hydroxide
weak
12
Which type of electrolyte is AgCl
weak
13
Amy equilibrium involving ions is called
ionic equilibrium
14
On dilution degree of dissociation of weak electrolyte
increases
15
On dilution concentration n of weak electrolyte
decreases
16
2
17
3
18
0.31
19
0.095
20
2
21
If a strong electrolyte containing at least one common ion is added to a solution of weak electrolyte then degree of dissociation of weak electrolyte
decreases
22
In an Aqueous solution of HCN,NaCl aqueous solution is mixed then common ion effect will take place or not
no
23
10-⁴
24
2
25
2
26
Water is a very weak electrolyte which undergo self ionization
true
27
In pure H2O at 25°C concentration of [H+]
is
10-⁷
28
In pure H2O at 25°C value of Kw is
10-¹⁴
29
pH scale was given by sorenson
t
30
Calculate pH of pure water at 25°C
7
31
Calculate pH of 0.01M HCl at 25°C
2
32
Calculate pH of 10-¹⁰M HCl(aq) solution at 25°C
7
33
Value of log 5
0.7
34
Calculate pH of 10-²M NaOH(aq) solution at 25°C
2
35
Calculate pH of 10-⁷M NaOH(aq) solution at 25°C
7.3
36
Calculate pH of 10-⁸M HCl(aq) solution at 25°C
6.97
37
Calculate pH of 10-⁸M KOH(aq) solution at 25°C
7.03
38
Calculate pH of 10-⁷M HNO3(aq) solution at 25°C
6.7
39
Calculate pH of 10-¹⁰M NaOH(aq) solution at 25°C
7
40
3
41
2
42
Calculate concentration of [H+] in a solution if pH of solution is 2.4
4*10-³
43
Calculate concentration of [H+] in a solution if pH of solution is 3.3
5*10-⁴
44
3
45
4
46
Calculate pH of 0.1M Acetic acid (Ka=10-⁵) solution at 25°C
3
47
Calculate pH of 0.01M Ammonium hydroxide (Kb=10-⁶) solution at 25°C
10
48
Calculate pH of 0.01M NaOH(aq) solution at 25°C
2
49
Calculate pH of 0.005M sulphuric acid solution at 25°C
3
50
Calculate pH of 0.1M Ammonium hydroxide (Kb=10-⁶) solution at 25°C
11
51
1
52
3
53
If Ka1& Ka2 values differ by 10³ or more than the smaller k will be neglected
t
54
3
55
4
56
4
57
1
58
2
59
Refresh
t
60
Recheck
t
61
4
62
Salt hydrolysis is reverse reaction of
neutralization
63
The breaking up of salt in presence of water to generate respective acid or base is called
salt hydrolysis
64
Weaker part of a salt undergo _____ and stronger part decide the_____ of solution
hydrolysis,pH
65
4
66
3
67
1
68
4
69
3
70
The solution which pH does not change on addition of small amount of acid or base are called as
buffer
71
Weak acid with its salt with strong base constitutes
acidic buffer
72
Weak base with its salt with strong acid constitutes
basic buffer
73
3
74
2
75
Theory given by
arhennius
76
Theory given by
bronsted
77
Theory given by
Lewis
78
Conjugate base of weak acid is strong base and vice versa
t
79
4
80
3
81
Addition of sodium acetate solution to acetic acid causes the following change
pH increases
82
4
83
4
84
yes
85
2
86
2
87
4
88
On increasing temperature of a weak acid dissociation_____ and pH _____
increases ,decreases
89
100 ml of 0.1M acetic acid started with 0.1M sodium hydroxide.
i)Calculate pH at half neutralization point
Or
Calculate pH when half of acids gets neutralized
1
90
Relation between solubility product and solubility for:
Hydrolysis of magnesium chloride
1
91
Calculate relation between solubility and solubility product for barium phosphate
1
92
Calculate solubility of silver chloride in pure water (Ksp=4x10-⁶)
1
93
Calculate solubility of silver chloride in (Ksp=4x10-⁶)
in 0.1M NaCl solution
1
94
Calculate solubility of silver iodide in 0.01N NaI solution ( Ksp=10-⁹)
1
95
3
96
Solubility product of BaCl2 is 4x10- ⁹ its solubility in moles per litre would be
1
97
Solubility product of AgCl is 2.8x 10-¹⁰ at 25°C calculate solubility of salt in 0.1M AgNO3 solution in moles /litre
1) 2.8x10-⁹
2)2.8x10-¹⁰
3) 3.2x10-⁹
4)3.2x10-¹²
1
98
Calculate solubility of barium chloride in 0.01 M NaCl solution in moles per litre
(Ksp=4x10-¹⁰)
1) 2x10-⁹
2)2.8x10-¹⁰
3) 4x10-⁶
4)3.2x10-¹²
3
99
Calculate solubility of Mg(OH)2 in 0.1 M NaOH solution
1) 10-¹⁰
2)10-⁹
3) 10-⁸
4)10-⁶
1
100
1) yes
2) no
2