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TEORI ASAM BASA

TEORI ASAM BASA. KIMIA DASAR 2012. ASAM BASA. ASAM BASA. ASAM BASA. ASAM BASA. ASAM BASA. ASAM BASA. ASAM BASA. KEKUATAN ASAM BASA. ASAM KUAT. ASAM LEMAH. REACTION OF ZINK WITH STRONG VS WEAK ACID. ACIDS Berasa asam Merubah lakmus React with active metals – Fe, Zn

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TEORI ASAM BASA

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  1. TEORI ASAM BASA KIMIA DASAR 2012

  2. ASAM BASA

  3. ASAM BASA

  4. ASAM BASA

  5. ASAM BASA

  6. ASAM BASA

  7. ASAM BASA

  8. ASAM BASA

  9. KEKUATAN ASAM BASA

  10. ASAM KUAT ASAM LEMAH REACTION OF ZINK WITH STRONG VS WEAK ACID

  11. ACIDS Berasa asam Merubah lakmus React with active metals – Fe, Zn React with bases Sifat umum • BASES • Berasa pahit • Merubah lakmus • Feel soapy or slippery (react with fats to make soap) • React with acids blue to red red to blue

  12. Teori ASAM BASA Svante August ARRHENIUS (Swedish) 1859 - 1927 Johannes Nicolaus BRØNSTED (Danish) 1879 - 1947 Thomas Martin LOWRY (English) 1874 - 1936 Gilbert Newton LEWIS (American) 1875 - 1946

  13. DEFINISI 1. TEORI ARRHENIUS : “ ASAMMERUPAKAN SENYAWA YANG DAPAT MENGHASILKAN ION HIDROGEN H+ BILA DILARUTKAN KEDALAM AIR”. Ion hidrogen (proton) dalam molekul air tidak dapat berdiri sendiri dan bergabung dengan cara mengganti sepasang elektron sunyi oksigen dari mol ekul air dan disebut ion HIDRONIUM Setiap molekul HCl hanya dapat menghasilkan 1 ion H+ disebut valensi asam. Asam semacam ini disebut juga asam monoprotik. Kalau menghasilkan 2 ion H+ disebut asam diprotik DAN lebih dari 2 disebut poliprotik

  14. DEFINISI 1. Arrhenius

  15. DEFINISI 1. Arrhenius “BASA MERUPAKAN SENYAWA YANG DAPAT MEMBERIKAN ION HIDROKSIDA (OH-) BILA DILARUTKAN DALAM AIR” Untuk menunjukkan sifat basanya larutan NH3 sering ditulis NH4OH

  16. DEFINISI 1. Arrhenius

  17. 2. TEORI BRØNSTED-LOWRY An acid is aproton donor, any species that donates an H+ ion. An acid must contain H in its formula; HNO3 and H2PO4- are two examples, all Arrhenius acids are Brønsted-Lowry acids. A base is a proton acceptor, any species that accepts an H+ ion. A base must contain a lone pair of electrons to bind the H+ ion; a few examples are NH3, CO32-, F -, as well as OH -. Brønsted-Lowry bases are not Arrhenius bases, but all Arrhenius bases contain the Brønsted-Lowry base OH-. Therefore in the Brønsted-Lowry perspective, onespecies donatesa protonand another species accepts it: an acid-base reaction is a proton transfer process. Acids donate a proton to water Bases accept a proton from water

  18. Molecular model: Two water (h2o) molecules react to form H3O+ and OH- OH- H2O H3O+ H2O Molecular model: The reaction of an acid HA with water to form H3O+ and a conjugate base. Acid (HA) Base (H2O) Conjugate Conjugate acid (H3O+) base (A-)

  19. 2. TEORI BRØNSTED-LOWRY

  20. 2. TEORI BRØNSTED-LOWRY

  21. 2. TEORI BRØNSTED-LOWRY

  22. Conjugate Pair Acid + Base Base + Acid Conjugate Pair The Conjugate Pairs in Some Acid-Base Reactions Reaction 1 HF + H2O F– + H3O+ Reaction 2 HCOOH + CN– HCOO– + HCN Reaction 3 NH4+ + CO32– NH3 + HCO3– Reaction 4 H2PO4– + OH– HPO42– + H2O Reaction 5 H2SO4 + N2H5+ HSO4– + N2H62+ Reaction 6 HPO42– + SO32– PO43– + HSO3–

  23. 2. TEORI BRØNSTED-LOWRY Conjugate pairs CH3COOHCH3COO- HCl Cl- NH4+NH3 HNO3NO3- How does a conjugate pair differ? H+transfer

  24. 2. TEORI BRØNSTED-LOWRY SENYAWA AMFOTER

  25. Lewis acid - a substance that accepts an electron pair 3. TEORI LEWIS Lewis base - a substance that donates an electron pair

  26. 3. TEORI LEWIS Formation ofhydronium ionis also an excellent example. • Electron pair of the new O-H bond originates on the Lewis base.

  27. 3. TEORI LEWIS

  28. 3. TEORI LEWIS

  29. 3. TEORI LEWIS

  30. RANGKUMAN • ASAM – produce H+ • BASA - produce OH- • ASAM – donate H+ • BASA – accept H+ • ASAM – accept e- pair • BASA – donate e- pair Arrehenius Unt. senyawa yg hanya larut dalam air Brønsted-Lowry Mencakup senyawa yg tak larut dalam air Lewis Digunakan dalam kimia organik, wider range of substances

  31. CONTOH

  32. KEKUATAN ASAM BASA

  33. KEKUATAN ASAM BASA

  34. ASAM DAN REAKSI IONISASINYA

  35. BASA DAN REAKSI IONISASINYA

  36. CONTOH SENYAWA AMFOTER

  37. ASAM DAN REAKSI IONISASINYA

  38. ASAM DAN REAKSI IONISASINYA

  39. TETAPAN KESETIMBANGAN

  40. TETAPAN KESETIMBANGAN

  41. TETAPAN KESETIMBANGAN

  42. TETAPAN KESETIMBANGAN

  43. TETAPAN KESETIMBANGAN

  44. TETAPAN KESETIMBANGAN Ka HCN = 17 x 10-10, Ka HOCl = 3 x 10-8, Ka CH3COOH = 76 x 10-5

  45. TETAPAN KESETIMBANGAN

  46. DERAJAT IONISASI

  47. DERAJAT IONISASI

  48. DERAJAT IONISASI

  49. DERAJAT IONISASI

  50. DERAJAT IONISASI • Jika diketahui Ka asam asetat adalah 1,76 x 10-5: • Berapakah derajat ionisasi ( ) asam asetat pada konsentrasi 0,1 M dan 0,01 M • Berapakah konsentrasi ion H+ pada kedua konsentrasi tersebut dengan memperhatikan derajat ionisasinya ( )?

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