Exam 7: Chemical Equilibrium

Calculate the total nickel concentration for a solution prepared by dissolving Ni(OH)₂ (s)in a 0.10 M OH⁻ solution.K_sp = 6 × 10⁻¹⁶,₁ = 1.26 × 10⁴,₂ = 1 × 10⁹,and ₃ = 1 × 10¹²_.

The pH of a solution is 9.65.The solution is________________________________________and the hydroxide concentration is____________________ than the hydronium concentration.

Calculate the pH for a 0.293 M OH⁻ solution.

The molar solubility of a saturated iron(II)carbonate solution derived from the K_sp value is 5.6 x 10⁻⁶ M.The molar solubility is greater than 5.6 x 10⁻⁶ M when accounting for additional reactions.Which of the reactions below will not increase the solubility of iron(II)carbonate?

What is the pH for a 5 x 10⁻⁵ M OH⁻ solution?

A student attempts to separate Cl⁻ and I⁻ from a solution that is 0.05 M Cl⁻ and 0.10 M I⁻ with Pb(NO₃)₂.As Pb(NO₃)₂ is added,which anion will precipitate first and what will the concentration of the anion be when the second anion begins to precipitate? K_sp = 1.7 x 10⁻⁵ for PbCl₂ and K_sp = 9.8 x 10⁻⁹ for PbI₂.

Which statements below are TRUE for enthalpy and entropy? I Enthalpy is the heat flow,q,under constant applied pressure. II Standard conditions for entropy and enthalpy changes are 1 M concentration,1 bar pressure and 298.15 K. III The entropy change for a system is the amount of energy,at a given temperature,that is dispersed into motion of the molecules in the system. IV When the value of H is negative,heat is released.When the value of S is negative,entropy is increased.

For a triprotic acid,which of the following is NOT true?

When the direction for a reaction is reversed the new value of K is:

For a reaction with a H^o = +50 kJ and a S^o = +100.0 J/K,G^o is____________________ and the equilibrium constant is____________________ .

For the reaction HCN (aq)+ H₂O (l) CN^- (aq)+ H₃O⁺ (aq),all of the following will shift the equilibrium toward the products,except: I adding HCN. II adding H₂O. III removing CN⁻. IV removing H₃O⁺.

Calculate the molar solubility for calcium fluoride in a 0.10 M NaF solution.K_sp = 3.2 × 10⁻¹¹ for CaF₂.

A reaction has a = −167.5 kJ/mol and = 57.3 J/mol K.Calculate the equilibrium constant for the reaction.

All of the following are strong acids,except:

Which of the classes of acids and bases and strength have been incorrectly matched?

Which of the following is INCORRECT for Brønsted-Lowry acids and bases?

In which solution is solubility of silver chloride the largest?

Silver ion is being considered as a reagent for separating IO₃⁻ from CO₃²⁻ in a solution that is 0.060 M in K₂CO₃ and 0.070 M in NaIO₃.Which anion will precipitate first and what will its concentration be when the second anion begins to precipitate? Can the two ions be separated with 99.99% efficiency? K_sp = 3.1 x 10⁻⁸ for AgIO₃ K_sp = 8.1 x 10⁻¹² for Ag₂CO₃

For the reaction aA (aq)+ bB (s) cC (l)+ dD (g),all of the statements below are TRUE,except:

Nickel forms three complexes with hydroxide,NiOH⁺ (aq),Ni(OH)₂ (aq)and Ni(OH (aq).Which statement(s)regarding the impact of complex formation on the solubility of nickel hydroxide are FALSE? I Hydroxide behaves as a Lewis acid when forming a complex with nickel. II The total nickel concentration is [Ni²⁺]_tot = [Ni²⁺] + [NiOH⁺] + [Ni(OH)₂] + [Ni(OH]. III As [OH^-] increases,the solubility of Ni(OH)₂ initially decreases but then increases. IV