Blog

Which of the following is true for a buffered solution?

A solution is 2.00 x 10-3 M Ba(NO3)2 and 0.0500 M KF.  Given that the Ksp of barium fluoride is 1.5 x 10-6,

Which of the following leads to the formation of a precipitate?

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

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 solutions will be the best buffer at a pH of 9.26? (Ka for HC2H3O2 is 1.8 × 10–5, Kb for NH3 is 1.8 × 10–5).

Assume an indicator works best when the equivalence point of a titration comes in the middle of the indicator range. Which indicator would be best for the following titration?0.100 M HOCl (Ka = 3.5 × 10–8) + 0.100 M NaOH

Which of the following salts shows the lowest solubility in water? (Ksp values: Ag2S = 1.6 × 10–49; Bi2S3 = 1.0 × 10–72; HgS = 1.6 × 10–54; Mg(OH)2 = 8.9 × 10–12; MnS = 2.3 × 10–13)

In the titration of a weak acid, HA, with a sodium hydroxide solution of approximately the same concentration, the stoichiometric point occurs at pH = 9.5. Which of the following weak acid indicators would be best suited to mark the endpoint of this titration?

Which, if any of the following mixtures will result in a precipitate.  You might need to know that the Ksp for AgCN is 2.2 x 10-16 and that for PbI2 is 7.9 x 10-9.I.  a mixture that is 1.2 x 10-6 M AgNO3 and 2.4 x 10-10 M NaCNII.  a mixture that is 2.3 x 10-4 M Pb(ClO4)2 and 4.6 x 10-3 M KI