Please Circle A2 on your Free Response Sheet You titrate 40.0 mL of 0.39 M unknown Acid with 0.37 M NaOH.  The pH at half-equivalence was 4.05.  Use the graph paper provided to draw the titration curve for this unknown acid.    Make sure your graph is properly labeled and contains the following (show your work for each calculation): initial pH mL to half equivalence and pH at half-equivalence mL to equivalence and pH at equivalence pH 10 mL after equivalence

Which of the following is the equilibrium constant expression for the dissociation of the weak acid HOCl?

Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2 × 10–10). Which of the following statements is true?

Which of the following aqueous solutions will have the highest pH? For NH3, Kb = 1.8 × 10–5; for C2H3O2–, Kb = 5.6 × 10–10.

The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of these statements (to a close approximation) is true?

For the stepwise dissociation of aqueous H3PO4, which of the following is not a conjugate acid–base pair?

Which of the following mixtures would be classified as a buffer solution?

Given the following Ksp values, which statement about solubility in mol/L in water is correct?   Ksp   Ksp PbCrO4 2.0 × 10–16 Pb(OH)2 1.2 × 10–15 Zn(OH)2 4.5 × 10–17 MnS 2.3 × 10–13

Consider the following indicators and their pH ranges: Methyl orange 3.2-4.4 Methyl red 4.8-6.0 Bromothymol blue 6.0-7.6 Phenolphthalein 8.2-10.0 Alizarin yellow 10.1-12.0 Assume an indicator works best when the equivalence point of a titration comes in the middle of the indicator range. For which of the following titrations would methyl red be the best indicator?

Consider the reaction HNO2(aq) + H2O(l)