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The polyprotic weak acid phosphoric acid, H3PO4, has 3 ionizable protons with Ka1 = 7.5 x 10-3 M, Ka2 = 6.2 x 10-8 M, and Ka3 = 4.8 x 10-13 M. Which Ka would be the most difficult to determine using the acid-base titration technique discussed in class?

Predict whether the equivalence point for a titration of NH3 with HCl will be above, below, or at pH 7.0.

Which is the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell and what charge is the anode.

If the equilibrium constant for a two-electron redox reaction at 298 K is 1.5 x 10-4, calculate the corresponding E°. Given R = 8.314 J/K-mol and F = 96,488 J/V-mol.

Which of the following is NOT a component of a voltaic cell?

Which of the following graphs would give a straight line for a zero-order reaction?

For the following reaction, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), calculate the emf at 25 °C with a [Zn(NO3)2] = 0.025 M and [Cu(NO3)2] = 0.50 M given the E° = 1.1 V, R = 8.314 J/K-mol, and F = 96,485 J/V-mol.

Which would be correct expression of the solubility product constant, Ksp, for Fe(OH)3?

A buffer is made by adding 0.300 mol CH3COOH and 0.300 mol CH3COONa to enough water to make 1.000 L of solution. The pH of the buffer is 4.74. Calculate the pH of this solution after 15.0 mL of 4.0 M NaOH(aq) solution is added.

If the pH of a solution is 6.27, which of the following statements is true?