can anyone send me all formulas for cacualting ph of every type of mixture in ionic equilibrium
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Calculation of pH of a Buffer Mixture
Calculation of pH of a Buffer Mixture
By Mrs Shilpi Nagpal On September 5, 2017 In Chemistry, Class 11, Ionic Equilibrium Tagged buffer capacity, calculation of pH of acidic buffer mixture, calculation of pH of basic buffer mixture, Henderson- Hasselbalch equation, importance of buffer solution Leave a comment
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For Acidic Buffer mixture( Henderson- Hasselbalch equation)


For Basic Buffer mixture
pOH = pKb + log [salt] / [Base]
pH + pOH =14
pOH = 14 – pH
pKa + pKb = 14
pKb=14 – pKa
14 – pH = 14 – pKa + log [salt) / [base]
pH = pKa – log [salt] / [base]
pH = pKa + log [base] / [salt]
where Ka is the ionization constant of the conjugate acid of the base.
For ex: In the buffer NH4OH + NH4Cl , NH4+ is the conjugate acid of the base, NH3 and Ka represents the ionization constant of the reaction:
NH4+ (aq) + H2O (l) NH3 (aq) + H+ (aq)
pH = pKa + log [NH3] / [NH4+]
pH = pKa + log [Base] / [conjugate acid
Calculation of pH of a Buffer Mixture
By Mrs Shilpi Nagpal On September 5, 2017 In Chemistry, Class 11, Ionic Equilibrium Tagged buffer capacity, calculation of pH of acidic buffer mixture, calculation of pH of basic buffer mixture, Henderson- Hasselbalch equation, importance of buffer solution Leave a comment
WhatsAppFacebookTwitterGoogle+
For Acidic Buffer mixture( Henderson- Hasselbalch equation)


For Basic Buffer mixture
pOH = pKb + log [salt] / [Base]
pH + pOH =14
pOH = 14 – pH
pKa + pKb = 14
pKb=14 – pKa
14 – pH = 14 – pKa + log [salt) / [base]
pH = pKa – log [salt] / [base]
pH = pKa + log [base] / [salt]
where Ka is the ionization constant of the conjugate acid of the base.
For ex: In the buffer NH4OH + NH4Cl , NH4+ is the conjugate acid of the base, NH3 and Ka represents the ionization constant of the reaction:
NH4+ (aq) + H2O (l) NH3 (aq) + H+ (aq)
pH = pKa + log [NH3] / [NH4+]
pH = pKa + log [Base] / [conjugate acid
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