Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). On planet X, a toy rocket, rising vertically with a velocity of 110 m/sec. Drag them down through the rows that correspond to the pre-equivalence phase (but no farther). Label all primary, secondary, and tertiary carbons. In each curve, label the halfway points to equivalence. Draw the titration curve for anserine. Since the concentrations of the acid and conjugate base are equal, pH = pKa + log (1). pKa is expressed as a common logarithm (base 10) and not as a natural logarithm (base e). Formula to calculate Ka from pKa. Suppose the pKa is 7. Calculate the Ka. Therefore, the Ka is 10^ -7. This means that this is a strong acid.
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