(3) Calculate the ionic strength of the following, assuming complete dissociation of salts: (a) 0.54 mM...
(4) A cyanide ion-selective electrode obeys the equation, E-K-0.05916log(CN). The potential was - 0.230 V when the electrode was immersed in 1.00 mM NaCN. (a) Evaluate the constant in the equation (b) Using the result from part (a), find (CN) if E=-0.280 V. (c) Without using the constant from part (a), find (CN) if E= -0.280 V.
A cyanide ion-selective electrode obeys the equation given below.E = constant − 0.05916 log [CN− ] The potential was −0.237 V when the electrode was immersed in 1.21 mM NaCN. (Assume that the Nernst potential is 0.05916 V.) (a) Evaluate the constant in the above equation. c = _____?_____V (b) Using the result from part (a), find [CN− ] if E = −0.318 V. −0.318 = c − 0.05916 log(x) x = ___?___ mM (c) Without using the constant from...
Assuming complete dissociation of the salts, calculate the ionic strength of a solution of 0.3 mM AlCl3.