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What is the significance of the Henderson-Hasselbalch equation in acid-base chemistry, and how does it relate to the pH of a solution?
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- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. a. Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. b. Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)Write the expression for the solubility product constant for Pb(OH)2.Write the expression for the solubility-product constant of the ionic compound: SrSO4
- Can HCl, a strong acid, be added to pure water and there be no significant change in pH?In terms of pH indicators, please fully explain what must occur in a solution to observe a colour change?Derive the Henderson- Hasselbalch equation for the dissociation of a weak base, B, in terms of pOH and pKb.
- The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?Explain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context of a titration.Describe buffer solutions in terms of acid-base equilibria. Give an example. How can you overwhelm buffer capacity?
