🗊Презентация Buffer solutions

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BUFFER SOLUTIONS
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BUFFER SOLUTIONS

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Buffer solutions solution which can resist the addition of a strong acid or a strong base or water. Its’ pH changes very slightly. + 1 drop of base [H+] in 1000 000 times + 1 drop of acid [H+] in 5000 times (from 10-7 tо 5 х10-4) In buffer solution from 1.00х10-7 to 1.01х10-7
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Buffer solutions solution which can resist the addition of a strong acid or a strong base or water. Its’ pH changes very slightly. + 1 drop of base [H+] in 1000 000 times + 1 drop of acid [H+] in 5000 times (from 10-7 tо 5 х10-4) In buffer solution from 1.00х10-7 to 1.01х10-7

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Classification
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Classification

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Buffer solutions, слайд №4
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Buffer solutions, слайд №5
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HOW TO PREPARE BUFFER 1. Mixing the components: -for acidic buffer pH = pKa + lg Ns·Vs/Na·Va -for basic buffer pH = 14 – pKв – lg Ns·Vs/Nb·Vb
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HOW TO PREPARE BUFFER 1. Mixing the components: -for acidic buffer pH = pKa + lg Ns·Vs/Na·Va -for basic buffer pH = 14 – pKв – lg Ns·Vs/Nb·Vb

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2. Partial neutralization For acidic buffer nacid = nbase = nsalt СН3СООН + NaOH = CH3COONa + H2O (exsess) pH = pKa + lg Nb·Vb / (Na·Va –Nb·Vb) For basic buffer NH4OH + HCL = NH4Cl + H2O (exsess) pH = 14 – pKв – lg Na·Va / (Nb·Vb - Na· Va)
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2. Partial neutralization For acidic buffer nacid = nbase = nsalt СН3СООН + NaOH = CH3COONa + H2O (exsess) pH = pKa + lg Nb·Vb / (Na·Va –Nb·Vb) For basic buffer NH4OH + HCL = NH4Cl + H2O (exsess) pH = 14 – pKв – lg Na·Va / (Nb·Vb - Na· Va)

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Buffer capacity Ba = nacid / |∆р Н|. Vbuf.sol Вb = nbase/ |∆р Н|. Vbuf.sol n – mole equivalents of a strong acid or a strong base Vbuf.sol - volume of a buffer solution ∆рН – pH change as a result of acid or base addition
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Buffer capacity Ba = nacid / |∆р Н|. Vbuf.sol Вb = nbase/ |∆р Н|. Vbuf.sol n – mole equivalents of a strong acid or a strong base Vbuf.sol - volume of a buffer solution ∆рН – pH change as a result of acid or base addition

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Buffer capacity depends on : pH = pKa + lg nsalt/nacid pH = 14 - pKb - lg nsalt/nbase
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Buffer capacity depends on : pH = pKa + lg nsalt/nacid pH = 14 - pKb - lg nsalt/nbase

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Buffer solutions, слайд №10
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Buffer capacity nsalt > nacid Вa > Вb nsalt < nacid Вa < Вb nsalt = nacid Вa = Вb =Вmax pH = pKa + lg nsalt/nacid
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Buffer capacity nsalt > nacid Вa > Вb nsalt < nacid Вa < Вb nsalt = nacid Вa = Вb =Вmax pH = pKa + lg nsalt/nacid

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Choose the buffer with maximum capacity and рН = 7.36 : Choose the buffer with maximum capacity and рН = 7.36 : 1) acetic рК = 4.75; 2) phosphate рК = 7.21; 3) hydrocarbonate рК = 6.37.
Описание слайда:
Choose the buffer with maximum capacity and рН = 7.36 : Choose the buffer with maximum capacity and рН = 7.36 : 1) acetic рК = 4.75; 2) phosphate рК = 7.21; 3) hydrocarbonate рК = 6.37.

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Buffer systems of a body 1.Mineral Hydrocarbonate Н2СО3 НСО3– Phosphate Н2РО4– НРO42– 2. Protein and aminoacidic.
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Buffer systems of a body 1.Mineral Hydrocarbonate Н2СО3 НСО3– Phosphate Н2РО4– НРO42– 2. Protein and aminoacidic.

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Buffer solutions, слайд №14
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Buffer solutions, слайд №15
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1. A buffer consists of 0,5 moles of equivalent NH3 and 0,5 moles of equivalent NH4Cl. Which buffer component must be added to change pH to 9? Kb(NH3)=1,8*10-5 2. What is the pH of buffer made of 60 ml of 0,10M NH3 with 40 ml of 0,10M NH4Cl. Kb=1,8*10-5. 3. What volume of 0,6M CH3COONa must be added to 600 ml of 0,2M CH3COOH to produce a buffer with pH=4,75? Ka(CH3COOH)=1,75*10-5.
Описание слайда:
1. A buffer consists of 0,5 moles of equivalent NH3 and 0,5 moles of equivalent NH4Cl. Which buffer component must be added to change pH to 9? Kb(NH3)=1,8*10-5 2. What is the pH of buffer made of 60 ml of 0,10M NH3 with 40 ml of 0,10M NH4Cl. Kb=1,8*10-5. 3. What volume of 0,6M CH3COONa must be added to 600 ml of 0,2M CH3COOH to produce a buffer with pH=4,75? Ka(CH3COOH)=1,75*10-5.

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4. What volume of 0,01M NaOH should be added to 100 ml of 0,5M CH3COOH solution to produce a buffer with pH 4,75? pKa(CH3COOH)=4,75 5. A buffer was prepared of 500 ml NaН2РО4 and 500 ml Na2НРO4 . After addition of 1 ml 0.1N HCl the change of buffer pH = 0.03. Calculate buffer capacity Ba. 6. Choose a buffer with Вa > Вb: a). 100 ml 0.2M NaHCO3 + 100ml 0.4M H2CO3 b). 100 ml 0.4M NaHCO3 + 100ml 0.2M H2CO3 c). 100 ml 0.2M NaHCO3 + 100ml 0.2M H2CO3
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4. What volume of 0,01M NaOH should be added to 100 ml of 0,5M CH3COOH solution to produce a buffer with pH 4,75? pKa(CH3COOH)=4,75 5. A buffer was prepared of 500 ml NaН2РО4 and 500 ml Na2НРO4 . After addition of 1 ml 0.1N HCl the change of buffer pH = 0.03. Calculate buffer capacity Ba. 6. Choose a buffer with Вa > Вb: a). 100 ml 0.2M NaHCO3 + 100ml 0.4M H2CO3 b). 100 ml 0.4M NaHCO3 + 100ml 0.2M H2CO3 c). 100 ml 0.2M NaHCO3 + 100ml 0.2M H2CO3

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Buffer solutions, слайд №18
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