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Calculate the pH of a buffer containing 1.25 M formic acid, HCOOH (Ka = 1.8 × 10-4) and 2.50 M sodium formate, HCOONa.You must show all of your work for credit.

For a certain reaction at 330 K, ∆Hsys = -9.9 kJ and ∆Ssys = 85 J/K, calculate ∆Suniv.

Calculate the pH of a solution with a hydroxide ion concentration of 5.25

For a certain reaction at 330 K, ∆Hsys = 9.9 kJ and ∆Ssys = 85 J/K, calculate ∆Suniv.

Calculate ΔG°rxn for the following reaction at 298 K. 2KCl(s)  → 2K(s) + Cl2(g)  ΔH° = 873 kJ;  ΔS° = 187 J/K Answer: ΔG°rxn  = [a] kJ

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) CO2(s) ⟶ CO2(g)[c] (b) CaCO3(s) ⟶ CaO(s) + CO2(g) [d] (c) 4Fe(s) + 3O2(g) ⟶ 2Fe2O3(s) [e]

Determine the balanced redox reaction represented by the following cell notation. Cu(s) ∣ Cu2+(aq) ∣∣ Zn2+(aq) ∣ Zn(s)

Consider the following equilibrium: CO(g) + H2O(g) ⇌ H2(g) + CO2(g)   Kc = 16 Suppose that 2.00 mol of CO  and 2.00 mol of H2O are placed in 0.500 L flask and allowed to come to equilibrium at high temperature. A) Calculate the equilibrium concentration of CO2(g) [a] mol/L B) Calculate the equilibrium concentration of H2O (g) [b] mol/L C) Calculate the equilibrium concentration of H2(g) [c] mol/L D) Calculate the equilibrium concentration of CO (g) [d] mol/L

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.00 at 25°C.

Select the conjugate base of the following acids: