In the formation of a transition metal complex, the central metal atom or ion acts as:

The following scenes (1, 2, and 3) represent solutions of calcium (gray) and iodate (black and red) ions that are above solid calcium iodate Ca(IO3)2. (The solid, other ions, and water are not shown)   a. Which scene best represents the solution in equilibrium with the solid in water? [A] b. In which, if any, other scene(s) will additional solid form? [B] c. Once the equilibrium has established in all scenes if applicable, how will addition Ca(NO3)2 (aq) affect the mass of solid present in any scene? [C]

Give the systematic name for [Ni(en)2(H2O)2]Cl2 (where en = ethylenediamine)

I hereby swear that I accept and will comply to all aspects of the UF honor code including the assertion: “I have neither given nor received any unauthorized aid in the execution of this exam” I am also currently shredding my scratch paper.

A popular buffer solution consists of carbonate (CO32–) and hydrogen carbonate (HCO3–) conjugate acid-base pair.  Which, if any, of the following such buffers can neutralize the greatest amount of added sodium hydroxide, while remaining within its buffer range?

  Determine whether a 0.1M solution formed from each of the following salts would be acid, basic, or neutral. NaNO3 [1] NH4Cl [2] KNO2 [3] NH4HCO3 [4] NaHS [5]  

  Determine whether a 0.1M solution formed from each of the following salts would be acid, basic, or neutral. KCl [1] NaCN [2] CH3NH3I [3] NH4ClO [4] NaHCO3 [5]  

What is the pH of a 0.025 M CH3COONa solution? Express using 2 decimal places.

Consider the following curve for the titration of a weak monoprotic acid (HA) with a strong base and answer each of the following questions: If the question asks for a volume, express your answer in increments of 5 mL (ex: 0, 5, 10, etc.). For all other questions, express your as a whole numbers (1, 2, 3, etc). A. What is the pH at the equivalence point? [A] B. What is the volume of added base at the equivalence point? [B] mL C. At what volume of added base is the pH calculated by working an equilibrium problem based on the initial concentration and Ka of the weak acid? [C] mL D. At what volume of added base does pH=pKa? [D] mL E. What is the pKa of the acid? [E]

A solution contains 0.002 M CO32− and 0.002 M OH−. Choose an answer that fulfills the two following questions when Co(NO3)2 is added slowly to the solution above. Ksp(CoCO3) = 1.0×10−13 and Ksp(Co(OH)2) = 1.0×10−15 Which salt will precipitate first AND what concentration of Co(NO3)2 added will cause its precipitation?