Last week you solved the membrane potential of a potassium ion selective electrode in a 0.0083 M KNO3 solution with 2.4 X 10-1 M NaBr and 3.6 X 10-4 M NH4Cl assuming [K+] = aK (KKNa = 1 X10-5 & KKNH4 = 2 X 10-3).

Now solve for the membrane potential but use activities instead of equilibrium concentrations- the ionic radii for K+ = 0.300 nm, for Na+=0.400 nm and for NH4+ =0.250 nm. What is the difference in the membrane potential using activities instead of equilibrium concentrations? find
deltaE = E (activities) - E(concentration)

Question

Last week you solved the membrane potential of a potassium ion selective electrode in a 0.0083 M KNO3 solution with 2.4 X 10-1 M NaBr and 3.6 X 10-4 M NH4Cl assuming [K+] = aK (KKNa = 1 X10-5 & KKNH4 = 2 X 10-3).

Now solve for the membrane potential but use activities instead of equilibrium concentrations- the ionic radii for K+ = 0.300 nm, for Na+=0.400 nm and for NH4+ =0.250 nm. What is the difference in the membrane potential using activities instead of equilibrium concentrations? find
deltaE = E (activities) - E(concentration)

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