Consider the following titration curve graphs:   Which plot shows the pH curve expected when NH3 is titrated by HNO3 ?

What is the molar solubility (in M) of iron (II) hydroxide, Fe(OH)2, in water? Hint:  Ksp of Fe(OH)₂ is 1.8 × 10-15

An example of a reaction that experiences a decrease in entropy, ΔS < 0, yet is spontaneous because of the release of a large quantity of heat, ΔH = −151 kJ, is the formation of solid ammonium nitrate from the reaction of gaseous nitric acid with gaseous ammonia.                        HNO3(g)   +   NH3(g)   →  NH4NO3 (s) The change in free energy under standard condition is: ΔG° =  −93. kJ/mol.  Calculate the equilibrium constant, K, for the reaction at T = 298 K.

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.

Which of the following solutions has the lowest H⁺ concentration?  Hint: Consider the common ion effect and how it would change the percent ionization of the weak acid. 

Consider a 1.00 L buffer solution made with 0.200 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.300 mol of NaF.  What is the pH of the solution after the addition of 0.100 mol of HCl. Hint:  Assume no change in volume upon addition of HCl  

Consider the reaction of elemental bromine with elemental chlorine to make a bromochloride compound at 600 K:                                          Br2(g)  +  Cl2(g)   ⇌   2 BrCl(g)       KP = 81.0 A closed vessel at 600 K is charged with 1.20 atm of Br2(g) and 1.20 atm of Cl2(g) initially and allowed to reach equilibrium. What is the partial pressure of the BrCl (in atm) at that equilibrium?

Consider the following aqueous reaction between ammonia (NH3) and formic acid (HCOOH): NH4+ (aq)  + HCOO─ (aq)   ⇌    NH3 (aq)  +  HCOOH (aq)   Identify the stronger acid and predict whether the equilibrium lies to the left or to the right? Hint: The Ka of HCOOH is 1.8 x 10─4 Hint: The Ka of NH4+ is 5.5 x 10─10

Consider the titration of 20 mL of 0.30 M butanoic acid, HC4H7O2, Ka = 1.5 x 10−5.  What is the pH of the solution after adding 10 mL of 0.15 M NaOH?

20.0 mL of a 0.300 M formic acid (HCOOH) solution is titrated with 0.200 M KOH.  What is the pH of the solution after the addition of 10.0 mL of KOH? Hint:  Ka of HCOOH = 1.8 x 10-4