ATURAN ELEKTROLISIS

 

KATODA (-) → Lihat ion (+) saja. Apapun jenis katodanya gak berpengaruh !

No

ION

Reaksi

Cara Hafal

Tempat

1. LARUTAN (Aq)

IA (Li+, Na+,K+,Rb+,Cs+,Fr+)

IIA (Be2+,Mg2+,Ca2+, Sr2+,Ba2+,Ra2+)

Al3+, Mn2+

2H2O + 2e → 2 OH + H2

Air jadi basa Ha ha Jempol Kiri
2. LEBURAN/LELEHAN/CAIRAN (l)

IA (Li+, Na+,K+,Rb+,Cs+,Fr+)

IIA (Be2+,Mg2+,Ca2+, Sr2+,Ba2+,Ra2+)

Al3+, Mn2+

Lx+ + x e → L

Ion jadi logam Telunjuk Kiri
3. Ion Asam ( H+ )

2 H+ + 2 e → H2

Asam jadi Ha ha Jari Tengah Kiri
4. Logam selain IA,IIA, Al3+, Mn2+

(Zn2+, Fe3+,Cr3+,Cu2+, Ag+ dsb)

Lx+ + x e → L

Ion jadi logam Jari Manis Kiri

 

ANODA (+)→ Perhatikan jenis Anodanya dulu : (INERT atau Reaktif ?)

No

ION

Reaksi

Cara Hafal

Tempat

A. Anoda INERT (C,Pt,Au)      
1. Ion VIIA ( F, Cl, Br, I, At )

2 X → X2 + 2e

X men jadi X two Jempol Kanan
2. Basa (OH)

4OH → 2H2O + O2 +4e

Basa karena air O O Telunjuk Kanan
3. Ion Poli atom (SO42-, CO32-, PO43-, NO3, dsb)

2H2O → 4H+ + O2 + 4e

Air jadi asam O O Jari Tengah Kanan
B. Anoda Reaktif (Selain C,Pt,Au),misalnya anoda :

Zn, Ag, Cu, Cr, Al, Ni, Fe dsb

L → Lx+ + xe

Contoh, Anoda:

Zn → Zn2+ + 2e

Ag → Ag+ + e

Cu → Cu2+ + 2e

Cr → Cr3+ + 3e

Al → Al3+ + 3e

Ni → Ni2+ + 2e

Fe → Fe3+ + 3e

Anunya jadi ion Jari Manis Kanan

 

Hukum Faraday I

F = mol x Valensi

F = mol H+ = mol OH = 2 x mol H2

F= mol e

; C = i x t

 

Hukum Faraday II

Pada arus sama/ muatan sama berlaku : mol 1 x valensi 1 = mol 2 x valensi 2

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