We're being asked to determine the governing equilibrium for the given solution.
CH3NH3Cl is a salt and will break up into its ions in the solution:
CH3NH3Cl(aq) → CH3NH3+(aq) + Cl-(aq)
CH3NH3+(aq) → positively charged amine → weak acid
Cl-(aq) → ion from a strong acid (HCl) → neutral ion and will not contribute to pH
1.00 g CH3NH3Cl (MW = 67.52 g/mol) and 1.00 g Ba(OH) 2∙8H2O (a strong base, MW = 315.47 g/mol) are added to 80 mL of water and dissolved. The resulting solution is diluted to 100 mL with water at 25°C.
Write the governing equilibrium.
A. CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH-(aq)
B. CH3NH3Cl(aq) ⇌ CH3NH3+(aq) + Cl-(aq)
C. Ba(OH)2(aq) ⇌ Ba2+(aq) + OH-(aq)
D. 2 CH3NH3Cl(aq) + Ba(OH)2(aq) ⇌ 2 CH3NH2(aq) + BaCl2 + 2 H2O(l)
E. CH3NH3+(aq) + OH-(aq) ⇌ CH3NH2(aq) + H2O(l)
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