Table 1.

The microscopic rate constants derived from fits to the data.

Solvents	0.05 M NaClc	0.3 M TMAOb	0.8 M TMAOa	0.4 M NaCla	1 M ureaa
Kd(mM)d	0.6 ± 0.1	0.6 ± 0.1	1.3 ± 0.2	4.7 ± 0.2	6.7 ± 0.8
koff/kon(mM)	9.9 ± 1.3	11 ± 3	16 ± 11	69 ± 12	198 ± 78
kclose(ms−1)	31.7 ± 0.9	16.1 ± 1.1	18.6 ± 3.0	21.2 ± 1.1	23.8 ± 3.6
kopen(ms−1)	1.5 ± 0.7	1.6 ± 0.5	2.1 ± 1.8	2.8 ± 0.3	4.1 ± 0.8
kuopen(ms−1)	---	---	2.0 ± 0.1	1.1 ± 0.2	0.7 ± 0.1
kuclose(ms−1)			0.2 ± 0.4	0.1 ± 0.3	0.5 ± 0.1
kd/calc(mM)e	0.5 ± 0.2	0.9 ± 0.4	1.6 ± 2.0	8.2 ± 1.9	20 ± 16

^aEach of these sample solvents contain 0.4 M NaCl and 0.05 M TEA

^bThe sample solvent contains 0.5 M TEA

^cThe sample solvent contains 0.05 M Tris and 0.05 M NaCl

^dK_d is the dissociation constant determined by fluorescence measurements

^e

$K_{d/\mathit{calc}}=\left(k_{\mathit{off}}/k_{on}\right)\left(k_{\mathit{close}}/k_{\mathit{open}}\right)/\left(1+\left(k_{\mathit{close}}^u/k_{\mathit{open}}^u\right)\right)$

$$R^2=\begin{array}{ll}\begin{array}{llll}{K}_d\hfill & k_{\mathit{off}}/k_{on}\hfill & k_{\mathit{close}}\hfill & k_{\mathit{open}}\hfill \end{array}\hfill & \hfill \\ \lfloor \begin{array}{llll}1.00\hfill & 0.89\hfill & 0.00\hfill & 0.93\hfill \\ 0.89\hfill & 1.00\hfill & 0.02\hfill & 0.91\hfill \\ 0.00\hfill & 0.02\hfill & 1.00\hfill & 0.00\hfill \\ 0.93\hfill & 0.91\hfill & 0.00\hfill & 1.00\hfill \end{array}\rfloor \hfill & \begin{array}{l}{K}_d\hfill \\ k_{\mathit{off}}/k_{on}\hfill \\ k_{\mathit{close}}\hfill \\ k_{\mathit{open}}\hfill \end{array}\hfill \end{array}$$