Ag+ (aq) + 2NH3 (aq) <----> Ag(NH3)2 ^+
Total moles of Ag+ initially present: (3.6x10^-2 moles)
Total moles of NH3 initially present: (6.9x10^-3 moles)
Measured concentration of Ag(NH3)2^+ at equilibrium: (3.4x10^-2 M)
Total solution volume: (100 mL)
a.) calculate the equilibrium concentration of Ag+
b.) calculate the equilibrium concentration of NH3
c.) calculate the value of the equilibrium constant.
please help me with this problem. I have no clue how to do it and my teacher said that there will be a similar one like this on the test tomorrow. thanks for all your help!
Total moles of Ag+ initially present: (3.6x10^-2 moles)
Total moles of NH3 initially present: (6.9x10^-3 moles)
Measured concentration of Ag(NH3)2^+ at equilibrium: (3.4x10^-2 M)
Total solution volume: (100 mL)
a.) calculate the equilibrium concentration of Ag+
b.) calculate the equilibrium concentration of NH3
c.) calculate the value of the equilibrium constant.
please help me with this problem. I have no clue how to do it and my teacher said that there will be a similar one like this on the test tomorrow. thanks for all your help!