Explain why buffer potential is maximised at the pH that matches the pka of the weak acid of the buffer. What does this have to do with buffer capacity?
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- Write the chemical equilibrium and expression for the equilibrium constants for the ionization of (a) tartaric acid. (b) malic acid.What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?How the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acid
- The pKa of a weak acid was determined by measuring the pH of a solution containing the weak acid at 0.30 M and its conjugate base at 0.30 M. The measured pH was 8.0. What is the pKa of the weak acid?The primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set at 7.4, what is the ratio of the concentrations of carbonate to bicarbonate. Describe the buffering capacity of this buffer.The degree of dissociation of acids is often expressed in terms of pKa. pka then is Directly measured by titration of the acid with sodium hydroxide Calculated by determining the acid's buffer capacity Directly determined by conductivity measurement The natural log of the acid's dissociation constant The reciprocal log of the dissociation constant
- Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?If a solution of dissolved acid has pH = 2.5 and the pka for the acid chemical is 4.3 and you measure the concentration of the conjugate []-base to be 10mm, what is the concentration of the acid in the solution? pH = pka + logi [HA]Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of H2CO3 (aq) acid are 6.37 and 10.32, respectively.
- The weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)-am inomethane, has pKa = 8.3 at 20 °C and is commonly used to produce a buffer for biochemical applications. At what pH would you expect Tris to act as a buffer in a solution that has equal molar concentrations of Tris and its conjugate acid?Determine the pH of a solution of aspirin (acetylsalicylic acid, HC9H7O4.) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. 652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.Explain how the bicarbonate and phosphate buffer systems resist pH changes.