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Basiskennis chemie 2
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Zuren
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Inhoudsopgave
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Theorie
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Zie voor de de theorie van deze opgaven
hier
.
Berekenen van de pH
[H
+
] naar pH
1.
[
H
+
]
=
3
,
69
⋅
10
−
12
{\displaystyle {\ce {[H+] \ = \ 3,69.10^{-12}}}}
11
,
43
{\displaystyle 11,43}
2.
[
H
+
]
=
4
,
78
⋅
10
0
{\displaystyle {\ce {[H+] \ = \ 4,78.10^{0}}}}
−
0
,
68
{\displaystyle -0,68}
3.
[
H
+
]
=
6
,
73
⋅
10
−
14
{\displaystyle {\ce {[H+] \ = \ 6,73.10^{-14}}}}
13
,
17
{\displaystyle 13,17}
4.
[
H
+
]
=
1
,
92
⋅
10
E
00
{\displaystyle {\ce {[H+] \ = \ 1,92.10^{E00}}}}
−
0
,
28
{\displaystyle -0,28}
5.
[
H
+
]
=
9
,
13
⋅
10
−
13
{\displaystyle {\ce {[H+] \ = \ 9,13.10^{-13}}}}
12
,
04
{\displaystyle 12,04}
6.
[
H
+
]
=
2
,
10
⋅
10
−
3
{\displaystyle {\ce {[H+] \ = \ 2,10.10^{-3}}}}
2
,
68
{\displaystyle 2,68}
7.
[
H
+
]
=
1
,
00
⋅
10
−
9
{\displaystyle {\ce {[H+] \ = \ 1,00.10^{-9}}}}
9
,
00
{\displaystyle 9,00}
8.
[
H
+
]
=
2
,
70
⋅
10
−
7
{\displaystyle {\ce {[H+] \ = \ 2,70.10^{-7}}}}
6
,
57
{\displaystyle 6,57}
9.
[
H
+
]
=
9
,
01
⋅
10
−
5
{\displaystyle {\ce {[H+] \ = \ 9,01.10^{-5}}}}
4
,
05
{\displaystyle 4,05}
10.
[
H
+
]
=
2
,
10
⋅
10
−
11
{\displaystyle {\ce {[H+] \ = \ 2,10.10^{-11}}}}
10
,
68
{\displaystyle 10,68}
11.
[
H
+
]
=
6
,
52
⋅
10
−
2
{\displaystyle {\ce {[H+] \ = \ 6,52.10^{-2}}}}
1
,
19
{\displaystyle 1,19}
12.
[
H
+
]
=
5
,
00
⋅
10
−
13
{\displaystyle {\ce {[H+] \ = \ 5,00.10^{-13}}}}
12
,
30
{\displaystyle 12,30}
13.
[
H
+
]
=
3
,
48
⋅
10
0
{\displaystyle {\ce {[H+] \ = \ 3,48.10^{0}}}}
−
0
,
54
{\displaystyle -0,54}
14.
[
H
+
]
=
7
,
90
⋅
10
−
14
{\displaystyle {\ce {[H+] \ = \ 7,90.10^{-14}}}}
13
,
10
{\displaystyle 13,10}
15.
[
H
+
]
=
9
,
90
⋅
10
−
2
{\displaystyle {\ce {[H+] \ = \ 9,90.10^{-2}}}}
1
,
00
{\displaystyle 1,00}
Bereken de concentratie waterstof-ionen in wetenschappelijke notatie met twee cijfers achter de komma
pH naar
[
H
+
]
{\displaystyle {\ce {[H^{+}]}}}
16.
pH
=
5
,
16
{\displaystyle {\ce {pH \ = \ 5{,}16}}}
c
H
+
=
6
,
92
10
−
6
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 6{,}92\,10^{-6}\ mol.L^{-1}}}}
17.
pH
=
6
,
69
{\displaystyle {\ce {pH \ = \ 6{,}69}}}
c
H
+
=
2
,
04
10
−
7
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 2{,}04\,10^{-7}\ mol.L^{-1}}}}
18.
pH
=
9
,
43
{\displaystyle {\ce {pH \ = \ 9{,}43}}}
c
H
+
=
3
,
72
10
−
10
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 3{,}72\,10^{-10}\ mol.L^{-1}}}}
19.
pH
=
2
,
69
{\displaystyle {\ce {pH \ = \ 2{,}69}}}
c
H
+
=
2
,
04
10
−
3
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 2{,}04\,10^{-3}\ mol.L^{-1}}}}
20.
pH
=
12
,
79
{\displaystyle {\ce {pH \ = \ 12{,}79}}}
c
H
+
=
1
,
62
10
−
13
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 1{,}62\,10^{-13}\ mol.L^{-1}}}}
21.
pH
=
0
,
29
{\displaystyle {\ce {pH \ = \ 0{,}29}}}
c
H
+
=
5
,
13
10
−
1
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 5{,}13\,10^{-1}\ mol.L^{-1}}}}
22.
pH
=
14
,
00
{\displaystyle {\ce {pH \ = \ 14{,}00}}}
c
H
+
=
1
,
00
10
−
14
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 1{,}00\,10^{-14}\ mol.L^{-1}}}}
23.
pH
=
0
,
38
{\displaystyle {\ce {pH \ = \ 0{,}38}}}
c
H
+
=
4
,
17
10
−
1
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 4{,}17\,10^{-1}\ mol.L^{-1}}}}
24.
pH
=
12
,
61
{\displaystyle {\ce {pH \ = \ 12{,}61}}}
c
H
+
=
2
,
45
10
−
13
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 2{,}45\,10^{-13}\ mol.L^{-1}}}}
25.
pH
=
2
,
94
{\displaystyle {\ce {pH \ = \ 2{,}94}}}
c
H
+
=
1
,
15
10
−
3
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 1{,}15\,10^{-3}\ mol.L^{-1}}}}
26.
pH
=
9
,
13
{\displaystyle {\ce {pH \ = \ 9{,}13}}}
c
H
+
=
7
,
41
10
−
10
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 7{,}41\,10^{-10}\ mol.L^{-1}}}}
27.
pH
=
7
,
00
{\displaystyle {\ce {pH \ = \ 7{,}00}}}
c
H
+
=
1
,
00
10
−
7
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 1{,}00\,10^{-7}\ mol.L^{-1}}}}
28.
pH
=
4
,
87
{\displaystyle {\ce {pH \ = \ 4{,}87}}}
c
H
+
=
1
,
35
10
−
5
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 1{,}35\,10^{-5}\ mol.L^{-1}}}}
29.
pH
=
11
,
06
{\displaystyle {\ce {pH \ = \ 11{,}06}}}
c
H
+
=
8
,
71
10
−
12
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 8{,}71\,10^{-12}\ mol.L^{-1}}}}
30.
pH
=
1
,
39
{\displaystyle {\ce {pH \ = \ 1{,}39}}}
c
H
+
=
4
,
07
10
−
2
mol
⋅
L
−
1
{\displaystyle {\ce {c_{H^{+}}\ =\ 4{,}07\,10^{-2}\ mol.L^{-1}}}}
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Inhoudsopgave
Volgende pagina
![{\displaystyle {\ce {[H+] \ = \ 3,69.10^{-12}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/3dedf62bfeea03a1fb649c9c74fb5769966a3527)
![{\displaystyle {\ce {[H+] \ = \ 4,78.10^{0}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/7074a7b7947650f26239516e434f374e554a935e)
![{\displaystyle {\ce {[H+] \ = \ 6,73.10^{-14}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/3b727e08c417fb23ed7e2b7bf499c88dcfaf94c4)
![{\displaystyle {\ce {[H+] \ = \ 1,92.10^{E00}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/4ee47330e9981f7086c67d9b17b5950c537a04ff)
![{\displaystyle {\ce {[H+] \ = \ 9,13.10^{-13}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/f92ddeca84c788850fd62b63c519f04dda5fc278)
![{\displaystyle {\ce {[H+] \ = \ 2,10.10^{-3}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/be91b6525ad042f1e93f6f9ee52678a69e66ace3)
![{\displaystyle {\ce {[H+] \ = \ 1,00.10^{-9}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/3d2bf96ac8add1239da26f8d3d4cdd3a1c52e69a)
![{\displaystyle {\ce {[H+] \ = \ 2,70.10^{-7}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/2bf8daafdb6fabff36279b87cf42c2e540359cf0)
![{\displaystyle {\ce {[H+] \ = \ 9,01.10^{-5}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/c2a2ea61cf998cfdee3054e32356b746ae5bb8c8)
![{\displaystyle {\ce {[H+] \ = \ 2,10.10^{-11}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/feed0d15c69c4580d7fa03e85c4838170bcf725b)
![{\displaystyle {\ce {[H+] \ = \ 6,52.10^{-2}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/aaabed9349cb41112efeac07ada93008f66adc14)
![{\displaystyle {\ce {[H+] \ = \ 5,00.10^{-13}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/c80baad6cfc1f3fac732870f8f5228210920c8e0)
![{\displaystyle {\ce {[H+] \ = \ 3,48.10^{0}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/764ca09b3a740449499647a73a46487ca5ef38fa)
![{\displaystyle {\ce {[H+] \ = \ 7,90.10^{-14}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/b5c3283e6361b790109789b96119d40298a7146c)
![{\displaystyle {\ce {[H+] \ = \ 9,90.10^{-2}}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/2a7939c0a2b66e5ec510e7cd1b7d6aa477b416e6)
![{\displaystyle {\ce {[H^{+}]}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/a2fc1cc19d4f43c4a85cb5bd81944898b1fdbaba)