Blog

Consider the titration of 50.0 mL of 0.10 M HClO4 with KOH.   What is the pH after 20.0 mL of 0.50 M KOH has been added?

Copper metal, Cu (s), is produced by running a current through a solution of Cu2+ in an electrolytic cell. How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for 2.00 h? Hint:  F = 96,500 C/mol e− Hint:  1 A = 1 C/s

The diagrams here represent solutions at various stages in the titration of a weak base B (such as NH3) with HCl. Which image best represents the solution beyond the equivalence point?             

Given the two following reduction half reactions: Fe3+(aq) +  e- →  Fe2+(aq)                  Eo = +0.770 V Pb2+(aq) +   2 e- →   Pb (s)                  Eo = −0.13 V Calculate ΔGº (in kJ) for a Fe2+/Pb voltaic cell. Hint:  Remember that a voltaic cell runs on a spontaneous redox reaction.  Hint: Make sure to determine the total moles of electrons transferred for the cell.

At 25°C, the pH of a solution is 7.23.  What is the hydroxide ion concentration, [OH−], of this solution?  

Which of the following has the smallest standard molar entropy, S° (298.15 K)?  

Which of the following combinations, when mixed in equal concentrations in water, would result in a buffer solution?  

If a reaction has a  ΔG = 0, this indicates that:

A 0.085 M solution of acetic acid (CH3COOH)  has a pH of 2.55. What is the percent ionization of this solution?

Consider the reaction of elemental bromine with elemental chlorine to make a bromochloride compound at 600 K:                                        2 BrCl(g)   ⇌   Br2(g)  +  Cl2(g)         KP = 81.0 A closed vessel at 600 K is charged with 3.00 atm of BrCl initially and allowed to reach equilibrium. What is the partial pressure of the Br2 (in atm) at that equilibrium?