The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: A 1.0 * 10^-³ mol sample of M(NO₃)₂ is added to 1.0 L of 15.0 M NH₃ (K_b = 1.8 *10^-⁵). Which of the following would be a dominant species in this solution?

Question

Quizplus · Accepted Answer

The formation constant (K) for the formation of M(NHS1U1B13S1U1B0)S1U1B13S1U1B0S1U1P12+S1S1P0 is higher than that of M(NHS1U1B13S1U1B0)S1U1P12+S1S1P0, which means that the former complex is more stable than the latter. Additionally, the concentration of NHS1U1B13S1U1B0 is very high (15.0 M), which increases the likelihood of forming a complex with a higher number of ligands (S1U1B13S1U1B0 instead of S1U1P1). Therefore, the dominant species in the solution would be M(NHS1U1B13S1U1B0)S1U1B13S1U1B0S1U1P12+S1S1P0.

The Cation M2+ Reacts with NH3 to Form a Series

The Cation M²⁺ Reacts with NH₃ to Form a Series