Praktikum Kimia Fisika II Tahun Akademik 2017/2018
PENENTUAN TETAPAN KESETIMBANGAN ASAM LEMAH SECARA KONDUKTOMETRI KONDUKTOMETRI I.
TUJUAN
1.
Untuk menentukan nilai Ka asam lemah
2.
Mempelajari daya hantar listrik larutan elektrolit kuat dan elektrolit lemah
II. LANDASAN TEORI 2.1
Konduktometri
Konduktometri merupakan metode analisis kimia berdasarkan daya hantar listrik suatu larutan. Daya hantar listrik (G) suatu larutan bergantung pada jenis dan konsentrasi ion di dalam larutan. Daya hantar listrik berhubungan dengan pergerakan suatu ion di dalam larutan ion yang mudah bergerak mempunyai daya hantar listrik yang besar. Daya hantar listrik (G) merupakan kebalikan dari tahanan (R), sehingga daya hantar listrik mempunyai satuan ohm -1. Bila arus listrik dialirkan ke dalam suatu larutan melalui dua elektroda, maka daya hantar listrik (G) berbanding lurus dengan luas permukaan elektroda (A) dan berbanding terbalik dengan jarak kedua elektroda (l). Jadi,
G = Rl = k Al
(1)
Di mana k adalah daya hantar jenis dalam satuan ohm -1cm-1 (Sumar, 1994). 2.2
Konduktivitas Termal Zat Cair
Untuk kebanyakan zat cair organik sederhana, konduktivitas termal antara 10 hingga 100 kali harga untuk gas tekanan rendah pada temperatur yang sama. Dalam hal ini ada sedikit ketergantungan terhadap tekanan, dan biasanya menaikkan temperatur berakibat turunnya konduktivitas termal. Karakteristik ini serupa dengan pada
Penentuan Tetapan Kesetimbangan Asam Lemah Lemah secara Konduktometri
1
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
viskositas zat cair, walaupun ketergantungan terhadap temperatur pada yang belakangan ini jelas dan hampir eksponensial, sedangkan dalam hal konduktivitas termal ketergantungan itu lemah dan hampir linier (Robert, 1990). Perhitungan konduktivitas secara langsung dari tahanan sampel dan dimensi sel l dan A tidak dapat diandalkan, karena distribusi arusnya rumit. Dalam prakteknya, sel dikalibrasikan dengan sampel yang diketahui konduktivitasnya k* (yang khas adalah larutan kalium klorida dalam air), dan konstanta sel C ditentukan dari : k* =
C
(2)
R*
Dengan R* merupakan tahanan standar. Dimensi C adalah [panjang] -1. Jika sampel mempunyai tahanan R dalam sel yang sama, maka konduktivitasnya adalah: k=
C R
(3)
Konduktivitas larutan bergantung pada jumlah ion yang ada, dan kita biasa memperkenalkan konduktivitas molar Ʌm, yang didefinisikan sebagai : Ʌm =
k c
(4)
Dengan c merupakan konsentrasi molar elektrolit yang ditambahkan. Konduktivitas molar biasanya dinyatakan dalam S.cm2.mol-1. Konduktivitas biasanya tersedia dalam S.cm -1 dan konsentrasi dalam M, sehingga hubungan praktisnya adalah :
( ⁄)
-1
100 x K/ S.cm-1 S.cm2 .mol Ʌm = c M
(5)
Konduktivitas molar elektrolit, tidak bergantung pada konsentrasi jika k tepat sebanding dengan konsentrasi elektrolit. Walaupun demikian,
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
sebanding dengan konsentrasi elektrolit. Misalnya, konsentrasi ion dalam larutan larutan asam lemah bergantung pada konsentrasi nominal asam itu, tidak mendua-kalikan jumlah ion tersebut. Kedua, karena ion saling berinteraksi dengan kuat, maka konduktivitas larutan tidak tepat sebanding dengan jumlah ion yang ada (Atkins, 1997). 2.3
Elektrolit Lemah
Elektrolit lemah adalah zat yang tidak terionisasi sempurna dalam larutan. Zat ini meliputi asam Bronsted lemah seperti CH 3COOH dan basa Bronsted lemah seperti NH 3. Ketergantungan konduktivitasnya pada konsentrasi dengan jelas, berasal dari pergeseran kesetimbangan (6)
( )
a H3 O+ a(A- ) Ka = a(HA)
(7)
Ke arah produk pada konsentrasi rendah. Konduktivitas bergantung pada jumlah ion dalam larutan, dan karenanya juga pada derajat ionisasi elektrolit α. Derajat ionisasi didefinisikan sehingga untuk asam HA pada konsentrasi nominal c, pada kesetimbangan :
[ ]
H3 O+ = αc
(8)
A = αc
(9)
HA = 1-α c
(10)
Jika kita ki ta mengabaikan mengabai kan koefisien aktivitas, maka konstanta keasaman kirakira kira : α2 c Ka = 1-α
(11)
Oleh karena itu, derajat ionisasi jika konsentrasinya c adalah : Ka α= 2c
1
{ } 4c 1+ Ka
2
-1
(12)
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Jika konduktivitas molar elektrolit terionisasi sempurna hipotetis adalah Ʌ’m, sedangkan fraksi α yang sebenarnya terdapat sebagai ion dalam
larutan sebenarnya, maka konduktivitas molar terukur Ʌm dinyatakan dengan : Ʌm = αɅ'm
Jika
konsentrasi
ion
dalam
larutan
(13) rendah,
maka
kita
dapat
memperkirakan Ʌ’m dengan nilai pembatasnya, dan menuliskan : Ʌm = αɅ°m
(14)
Setelah mengetahui K a, dapat menggunakan persamaan untuk meramalkan ketergantungan konduktivitas molar pada konsentrasi. Cara lain, untuk menggunakan ketergantungan Ʌm pada konsentrasi, dalam pengukuran konduktansi molar pembatas. Dengan mudah memanipulasi ungkapan untuk K a ke dalam bentuk: lαc = 1+ α Ka Kemudian,
dengan
menggunakan
(15)
persamaan,
diperoleh
hukum
pengenceran Ostwald 1 Ʌm
=
1 Ʌ°m
+
Ʌm c
( )
Ka Ʌ°m
2
(16)
Persamaan ini menunjukkan prosedur untuk menentukan konduktivitas molar pembatas larutan, karena persamaan ini menyiratkan bahwa jika 1/Ʌm dialurkan terhadap c, maka perpotongan pada c = 0 merupakan 1/Ʌ°m (Atkins, 1997).
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
III. PROSEDUR PERCOBAAN 3.1
Alat dan Bahan
3.1.1 Alat dan Fungsinya
No
Alat
Fungsinya
1
Gelas Piala
untuk wadah larutan
2
Labu Ukur
untuk tempat mengencerkan larutan
3
Labu Semprot
untuk wadah akuades
4
Konduktometer
untuk alat untuk mengukur hantaran listrik
5
Gelas Ukur
untuk wadah mengukur larutan
6
Sel Hantaran
untuk sel penghantar
3.1.2 Bahan dan Fungsinya
No
Bahan
Fungsinya
1
Larutan asam asetat
sebagai sampel uji
2
Akuades
sebagai pelarut
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
3.2
Cara Kerja
Pada praktikum kali ini, digunakan larutan asam asetat sebagai larutan sampel. Larutan asam asetat dibuat dengan berbagai konsentrasi yaitu 1 ; 0,5 ; 0,25 ; 0,125 ; 0,0625 dan 0,03125 N dengan cara pengenceran bertingkat dari larutan induk asam asetat 100% dengan menggunakan labu ukur 100 mL. Larutan asam asetat yang telah dibuat diukur hantaran dan suhu menggunakan konduktometer yang sebelumnya telah dikalibrasi dengang menggunakan akuades. Hasil pengamatan dicatat dan ditentukan nilai Ka dari larutan asam asetat dengan menggunakan grafik.
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
3.3
Skema Kerja
Larutan asam asetat - dibuat dengan konsentrasi 1 ; 0,5 ; 0,25 ; 0,125 ; 0,0625 dan 0,03125 N - ditentukan nilai hantaran dan suhu dengan menggunakan konduktometer yang telah dikalibrasi - dicatat data pengukuran dengan konduktometer konduktometer - dibuat grafik dan ditentukan Ka Hasil
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
3.4
Skema Alat
1
2 3
4
Keterangan : 1. Konduktometer 2. Sel hantaran 3. Gelas piala 4. Larutan elektrolit
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
IV. DATA DAN PERHITUNGAN 4.1
Data
Hantaran aquades = 0,57 x 10-6 Suhu aquades
= 31,3°C
No. Konsentrasi asam asetat (N)
Hantaran (s)
Suhu ( ºC)
1
0,03125
1,96 x 10-6
32,5
2
0,0625
1,91 x 10-6
32,4
3
0,125
1,87 x 10-6
32,7
4
0,25
1,78 x 10-6
32,4
5
0,5
1,38 x 10-6
32,0
6
1
0,82 x 10-6
32,1
4.2
Perhitungan
1.
Pengenceran larutan asam asetat Larutan asam asetat 100%
N= =
ρ × % ×1000 Mr 1,059 g/mol × % ×1000 60 g/mol
= 17,65 N Larutan asam asetat 1N
V1 x N1 = V2 x N2 V1 x 17,65 N = 100 mL x 1 N
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Larutan asam asetat 0,25 N
V1 x N1 = V2 x N2 V1 x 0,5 N = 100 mL x 0,25 N V1 = 50 mL Larutan asam asetat 0,125 N
V1 x N1 = V2 x N2 V1 x 0,25 N = 100 mL x 0,125 N V1 = 50 mL Larutan asam asetat 0,0625 N
V1 x N1 = V2 x N2 V1 x 0,125 N = 100 mL x 0,0625 N V1 = 50 mL Larutan asam asetat 0,03125 N
V1 x N1 = V2 x N2 V1 x 0,0625 N = 100 mL x 0,03125 N V1 = 50 mL 2.
Penentuan hantaran (L) Larutan asam asetat 1N
L = L asam asetat – L aquades = 0,82 x 10-6 – 0,57 x 10-6 = 0,25 x 10-6 s Larutan asam asetat 0,5 N
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Larutan asam asetat 0,125 N
L = L asam asetat – L aquades = 1,87 x 10-6 – 0,57 x 10-6 = 1,3 x 10-6 s Larutan asam asetat 0,0625 N
L = L asam asetat – L aquades = 1,91 x 10-6 – 0,57 x 10-6 = 1,34 x 10-6 s Larutan asam asetat 0,03125 N
L = L asam asetat – L aquades = 1,96 x 10-6 – 0,57 x 10-6 = 1,39 x 10-6 s 3.
Penentuan nilai K
1
= 0,099 / cm
Larutan asam asetat 1N
K=Lx
1λ
= 0,25 x 10-6 s x 0,099 /cm = 2,475 x 10-8 s/cm Larutan asam asetat 0,5 N
K=Lx
1λ
= 0,81 x 10-6 s x 0,099 /cm = 8,019 x 10-8 s/cm
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Larutan asam asetat 0,125 N
K=Lx
1λ
= 1,3 x 10-6 s x 0,099 /cm = 12,87 x 10-8 s/cm Larutan asam asetat 0,0625 N
K=Lx
1λ
= 1,34 x 10-6 s x 0,099 /cm = 13,266 x 10-8 s/cm Larutan asam asetat 0,03125 N
K=Lx
1λ
= 1,39 x 10-6 s x 0,099 /cm = 13,761 x 10-8 s/cm 4.
Penentuan hantaran ekuivalen Ʌ=
1000 x k c
Larutan asam asetat 1 N
1000 x 2,475x10 -8
⁄
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Larutan asam asetat 0,0625 N
⁄
1000 x 13,266x10 -8 s cm Ʌ = 0,0625 N = 212,256 x 10-5 s/cm N Larutan asam asetat 0,03125 N
⁄ 03125
1000 x 13,761x10 -8 s cm Ʌ = 0, N = 440,352 x 10-5 s/cm N 5.
Persamaan Regresi X = Hantaran ekivalen Ʌ (s/cm.N) Y = 1/Ʌ X
Y
XY
X2
2,475 x 10-5
40404
0,999999
6,1256 x 1010
16,033 x 10-5
6237
0,999978
2,5705 x 108
47,916 x 10-5
2086
0,999528
2,2959 x 107
102,96 x 10-5
971
0,999742
1,0600 x 106
212,256 x 10-5
471
0,999726
4,5052 x 106
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
4.3 Grafik
Pengaruh Hantaran Ekivalen Ʌ terhadap 1/ Ʌ 50000 40000 30000 Ʌ
/ 1
20000
y = -4518889x + 14590 R² = 0,2272
10000 0 -10000
0
0.001
0.002
0.003
Hantaran Ekivalen ( Ʌ)
0.004
0.005
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
V. PENGAMATAN DAN PEMBAHASAN 5.1
Pengamatan Setiap Langkah Kerja
No
Cara Kerja dan Reaksi
Foto
1.
Sel hantaran dicuci dengan
Nilai
akuades dan diukur nilai
muncul
hantarannya
konduktometer
dengan
konduktometer. Dicuci dan diukur
lagi
Pengamatan
Analisis
hantaran
yang Nilai hantaran yang berkisar pada pada 0,57 x 10-6 dikarenakan oleh zat berkisar yang diukur adalah sama yaitu
pada angka 0,57 x 10-6
akuades
hantarannya
sampai nilainya tetap
2.
Dibuat larutan CH3COOH
Tidak
dengan variasi konsentrasi 1
perubahan, karena larutan sebenarnya mengalami perubahan,
; 0,5 ; 0,25 ; 0,125 ; 0,0625 dan
CH3COOH tidak berwarna
0,03125
N
dengan
pengenceran bertingkat
Penentuan Tetapan Kesetimbangan Asam Asam Lemah secara Konduktometri
terlihat
adanya Konsentrasi
dengan
larutan
pengenceran
konsentrasi
larutan
CH3COOH
bertingkat, CH3COOH
semakin encer
15
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
3.
Diukur
nilai
hantaran
Semakin besar konsentrasi Hasil pengamatan sesuai dengan
larutan CH3COOH 1 ; 0,5 ;
larutan
0,25 ; 0,125 ; 0,0625 dan
semakin
0,03125
hantaran larutannya
N
menggunakan
CH3COOH, teori, di mana konsentrasi larutan kecil
nilai elektrolit akan berbanding terbalik dengan daya hantaran listrik
konduktometer
Penentuan Tetapan Kesetimbangan Asam Asam Lemah secara Konduktometri
16
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
5.2 Pembahasan
Pada praktikum kali ini yaitu penentuan tetapan asam lemah secara konduktometri yang bertujuan untuk menentukan nilai Ka asam lemah dan mempelajari daya hantar listrik larutan elektrolit kuat dan elektrolit lemah. Pada percobaan penentuan tetapan kesetimbangan asam lemah secara konduktometri ini, pengukuran derajat disosiasi dilakukan berdasarkan pengukuran konduktivitas elektrolit yang biasa disebut metoda konduktivitas. Dari konduktometer bisa diketahui besarnya konduktivitas atau hantaran dari suatu larutan yang akan digunakan. Larutan yang akan ditentukan hantarannya ialah asam asetat. Untuk mendapatkan variasi konsentrasi dari asam asetat dilakukan pengenceran
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
VI. KESIMPULAN DAN SARAN 6.1
Kesimpulan
Dari percobaan yang telah dilakukan dapat disimpulkan bahwa tetapan kesetimbangan asam lemah dapat ditentukan secara konduktometri. Nilai Ka asam lemah yang diperoleh dari percobaan adalah 2,475 x 10 -6. Larutan asam lemah akan terionisasi sebagian jika dilarutkan dalam air dan reaksinya bersifat reversible
6.2 Saran
Untuk mendapatkan hasil yang lebih sesuai dengan yang diinginkan maka disarankan agar :
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
DAFTAR PUSTAKA Atkins, P. W.: Kimia Fisika, Edisi Keempat, Jilid 2; 2 ; Erlangga; Jakarta, 1997. Hendayana, Sumar, Ph.D; Kadarohman, Drs. Asep; Sumarna, Drs. AA; Supriatna, Drs. Asep: Kimia Analitik Instrumen, Edisi Kesatu; Kesatu ; IKIP Semarang Press; Semarang, 1994. Reid, Robert C.; Prausnitz, John M.; Sherwood, Thomas K.: Sifat Gas dan Zat Cair, Edisi Ketiga; Ketiga; PT Gramedia Pustaka Utama; Jakarta, 1991.
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Lampiran 1. Tugas Sebelum Praktikum
1. Jelaskan tentang hantaran jenis dan hantaran ekivalen apa satuannya? Hantaran jenis adalah perbandingan daerah elektroda dengan jarak elektroda atau daya hantar 1 cm 3. Satuannya : ohm/cm Hantaran ekuivalen adalah hantaran larutan asam atau daya hantar larutan elektrolit sebanyak 1 g equivalen diantara 2 elektroda dengan jarak 1 cm. Satuannya : mho/cm2. 2.
Apa gunanya mengukur hantaran larutan KCl 0,1 N ? Gunanya untuk mengukur hantaran larutan KCl 0,1 N adalah untuk menentukan hantaran jenis larutan lain dimana nilai-nilai hantaran jenis dianggap konstan.
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
6.
Turunkan persamaan penentuan Ka untuk elektrolit 1-2 dengan pengukuran hantaran ! Penentuan Ka untuk elektrolit 1-2 dengan pengukuran hantaran, penurunan persamaan : AB
A+ + B-
C(1-α) C(1-α) K= α=
( A)( B) ( AB)
c
o
=
( c ) 2 C (1 )
αc
αc
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Lampiran 2. Analisis Artikel Ilmiah Judul
Penentuan konstanta disosiasi untuk bahan aktif dari ekstrak herbal menggunakan metode kesetimbangan fase cair Tujuan
Untuk menentukan konstanta disosiasi untuk bahan aktif dari ekstrak
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
tabel 5 menunjukkan bahwa fase berair yang mengandung pelarut organik menghasilkan nilai pka yang meningkat. Sedangkan pada tabel 7 menunjukkan bahwa nilai pKa yang diperoleh secara praktikum mendekati nilai Pka secara teori. Hubungan dengan Praktikum
Jurnal ini berisi tentang penentuan konstanta disosiasi bahan aktif dari
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Lampiran 3. Simbol yang Digunakan
No.
Simbol
Keterangan
1.
α
derajat ionisasi
2.
Ʌc
hantaran ekivalen larutan pada konsentrasi tertentu
3.
Ʌ
hantaran ekivalen larutan pada pengenceran tak
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Praktikum Kimia Fisika II Tahun Akademik 2017/2018
Lampiran 4. Struktur Senyawa Utama
No. 1.
Senyawa Asam Asetat CH3COOH
Struktur