Calculate the hydroxide ion concentration in an aqueous solution with a pH of 3.00 at 25°C.

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) Pb2+(aq) + S2-(aq) ⟶ PbS(s) [a] (b) NaNO3(s) ⟶ Na+(aq) + NO3-(aq) [b] (c) CO2(s) ⟶ CO2(g)[c]

Calculate the cell potential of a voltaic cell, which consists of a Sn/Sn2+ half-cell and a Cu/Cu2+ half-cell. Sn2+ + 2 e⁻  →  Sn Eo = -0.14 V Cu2+ + 2 e⁻  →  Cu Eo = +0.34 V

Are the following solutions acidic, basic, or neutral? a) Ba(NO3)2(aq) [a] b) NaClO2(aq) [b] c) NH4ClO4(aq) [c]

At 298 K , ∆H = -198.4 kJ and ∆S = -187.9 J/K for the reaction shown below. 2SO2(g)  +  O2(g) ⟶ 2SO3(g) (a) Use the data to decide if this reaction is spontaneous at 298 K. [a] (b) What is the temperature below which the reaction is spontaneous? [b]

A 0.300 M solution of a weak base, B, has a pH of 9.75. Calculate the value of Kb for the base. Hint: Write the reaction between the base B and water (B + H2O → BH+ + OH-), and use on ICE Table. You must show all of your work for credit.

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) Pb2+(aq) + S2-(aq) ⟶ PbS(s) [a] (b) CO2(s) ⟶ CO2(g)[c] (c) 4Fe(s) + 3O2(g) ⟶ 2Fe2O3(s) [e]

Use the following values to calculate ∆S for the sublimation of 1 mole of I2. I2(s) ⟶I2(g) Substance (state) So (J/mol.K) I2(s) 116.1 I2(g) 260.7

Calculate the cell potential of a voltaic cell, which consists of a Sn/Sn2+ half-cell and a Fe/Fe2+ half-cell. Sn2+ + 2 e⁻  →  Sn Eo = -0.14 V Fe2+ + 2 e⁻  →  Fe Eo = -0.44 V

What is the cell potential at 25oC for the concentration cell described by: Cu(s) | Cu2+(aq, 0.10 M) || Cu2+(aq, 0.80 M) | Cu(s) You must show all of your work for credit!