Which one of the following aqua-ion would you expect to have the lowest pka? a. [Rh(OH2)6]³+ O b. [Co(OH2)G]3+ O c. [Ir(OH2)6]3+

Silver and ammonia may react to form Ag(NH3)2+ complex (​K​f = 1.66 x 10​7). A 500 mL of 0.20mol Ag+ and 500 mL of 0.80 mol NH3 are mixed together.a. Write the complexation reaction.b. Write the formation constant expression.c. What is the concentration of the complex at equilibrium?d. What is the concentration of the metal at equilibrium?

1a) Using the ionic model, determine the valence electron count of the transition metal in complex A shown below; convince yourself that complex A is already a catalyst. (i-Pr)2P- -Ir -P(i-Pr)2 A

How many unpaired electrons are in the following complex ions? a) Ru(NH3)62+ (low spin case) _____ unpaired electron(s) b) Ni(H2O)63+ (low spin case) ______ unpaired electron(s) c) V(en)32+ ________ unpaired electron(s)

[Cd(CN)4] complex K₁=6.03 × 10¹8 at 25 °C. x Suppose equal volumes of 0.0086M Cd (NO3), solution and 0.18M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Cd²+ ion. For the aqueous Round your answer to 2 significant digits.

2. Which aquo ion would you expect to have the lowest pKa (i.e., be most acidic)? Explain your choice. MAZ a) [Ir(OH₂)6]³+ b) [Rh(OH2)6]³+ c) [Co(OH₂)6]³+ d) [Co(OH₂)6]²+ AL OH₂ H₂O.OH₂ H₂0 OH₂ OH₂ n+

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31 For the aqueous [Ni(CN)4] complex K₁=2.00 × 10³¹ at 25 °C. .2+ Suppose equal volumes of 0.0052M Ni (NO3), solution and 1.0M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. Round your answer to 2 significant digits. M x10 × Ś

In the right conditions, a zinc–bacteriochlorin complex can be synthesized according to the reaction below. The complex-formation reaction shown is a Lewis acid–base reaction. Which substance is the acid, and which is the base? Why?

Please show solution and explain   [Co(H2O)6]2+ + 4Cl1- ⇋ [CoCl4]2- + 6H2O