Amino acids are the key components of proteins. When fully protonated, amino acids have similar chemical reactions as diprotic acids (such as found in H₂CO₃). For example, alanine udergoes the following reactions:

• H₂C₃H₅NO_2⁺(aq)  H⁺_(aq) + HC₃H₅NO_{2 (aq)} K₁ = 4.5 X 10^-3
• HC₃H₅NO_{2 (aq)}  H⁺_(aq) + C₃H₅NO₂^-_(aq) K₂ = 1.3 X 10^-10
• H₂O_(I)  H⁺_(aq) + OH^-_(aq) K_w = 1.0 X 10^-14

Using only the value of the first equilibrium constant value (K₁) from part "A" would a solution that had the following concentrations (H₂C₃H₅NO₂⁺ = 0.000050M; H⁺ = 0.000040M; HC₃H₅NO₂ = 0.000030M) be at equilibrium? What is the value of Q for this system? If it is not at equilibrium, in which direction would it proceed to reach equilibrium?

• 0.000024; Q < K; reaction will proceed to make more products.
• 0.000023; Q > K; reaction will proceed to make more reactants.
• 0.000022; Q < K; reaction will proceed to make more products.
• 0.000020; Q > K; reaction will proceed to make more reactants.
• 0.000019; Q < K; reaction will proceed to make more products.