Kinetics of Complex Formation between DNA and Cationically Charged Cylindrical Brush Polymers Observed by Stopped Flow Light Scattering

2009 ◽  
Vol 30 (17) ◽  
pp. 1470-1476 ◽  
Author(s):  
Frauke Kuehn ◽  
Karl Fischer ◽  
Manfred Schmidt
Keyword(s):  
Light Scattering ◽  
Complex Formation ◽  
Stopped Flow ◽  
Kinetics Of ◽  
Brush Polymers

Early stage kinetics of polyelectrolyte complex coacervation monitored through stopped-flow light scattering

Soft Matter ◽  
2016 ◽  
Vol 12 (44) ◽  
pp. 9030-9038 ◽  
Author(s):  
Xiaoqing Liu ◽  
Marie Haddou ◽  
Isabelle Grillo ◽  
Zohra Mana ◽  
Jean-Paul Chapel ◽  
...  
Keyword(s):  
Light Scattering ◽  
Polyelectrolyte Complex ◽  
Early Stage ◽  
Stopped Flow ◽  
Complex Coacervation ◽  
Kinetics Of

pH-Induced Deswelling Kinetics of Sterically Stabilized Poly(2-vinylpyridine) Microgels Probed by Stopped-Flow Light Scattering

Langmuir ◽  
2008 ◽  
Vol 24 (17) ◽  
pp. 9334-9340 ◽  
Author(s):  
Jun Yin ◽  
Damien Dupin ◽  
Junfang Li ◽  
Steven P. Armes ◽  
Shiyong Liu
Keyword(s):  
Light Scattering ◽  
Stopped Flow ◽  
Kinetics Of

Kinetics of ribosome dissociation and subunit association studied in a light-scattering stopped-flow apparatus

Biochemistry ◽  
1976 ◽  
Vol 15 (26) ◽  
pp. 5743-5753 ◽  
Author(s):  
Helmut Goerisch ◽  
Dixie J. Goss ◽  
Lawrence J. Parkhurst
Keyword(s):  
Light Scattering ◽  
Stopped Flow ◽  
Flow Apparatus ◽  
Kinetics Of

Metal-ion oxidations in solution. Part XVIII. Characterization, rates, and mechanism of formation of the intermediates in the oxidation of thiols by chromium(VI)

1977 ◽  
Vol 55 (18) ◽  
pp. 3328-3334 ◽  
Author(s):  
Alexander McAuley ◽  
M. Adegboyega Olatunji
Keyword(s):  
Complex Formation ◽  
Thermodynamic Parameters ◽  
Rate Constants ◽  
Metal Ion ◽  
Formation Mechanisms ◽  
Stopped Flow ◽  
Mechanism Of Formation ◽  
Chromium Vi ◽  
Kinetics Of ◽  
Absorbance Data

The stopped-flow technique has been used to study the reactions of [HCrO4−] and penicillamine, glutathione and β-mercaptoethylamine (RSH) in perchlorate media, [H+] = 0.02−0.100 M, I = 1.00 M over the temperature range 10–30 °C. The transient orange species formed as intermediates are 1:1 chromate esters,[Formula: see text]with λmax ∼ 420–430 nm and K1 ∼ 700 (DL-penicillamine) to 1440 M−1 (glutathione) at T = 25 °C. Thermodynamic parameters for complex formation have been derived from initial absorbance data and the evidence for sulphur bonding is discussed. Kinetics of the reactions conform to the rate law[Formula: see text]Activation enthalpies lie in the range 6–10 kcal/mol but ΔS≠ values vary considerably possibly reflecting solvation effects. The rate constants kfH+ are several orders of magnitude lower than those found for this parameter in other reactions of this type. The complex formation mechanisms are discussed and the possibility of some associative character in the present reactions is considered.

Kinetics of the Cu(II) – Nitrilotriacetic Acid Reaction

1974 ◽  
Vol 52 (24) ◽  
pp. 4106-4108 ◽  
Author(s):  
James Maguire
Keyword(s):  
Complex Formation ◽  
Nitrilotriacetic Acid ◽  
Stopped Flow ◽  
Kinetic Behavior ◽  
First Order ◽  
Acid Reaction ◽  
Decreasing Ph ◽  
Ph Range ◽  
Rate Limiting ◽  
Kinetics Of

The kinetics of the reaction between Cu(II) and nitrilotriacetic acid (NTA) to form the 1:1 complex have been studied by the stopped-flow technique over the pH range 2–6. The reaction is kinetically first order in both [Cu(II)] and [NTA]total; the rate constant has a minimum value of 1.1 × 105 l mol−1 s−1 in the pH range 3.5–5 and increases with either increasing or decreasing pH. An explanation for the observed kinetic behavior may be that in the case of the monoprotonated species HNTA2− there is a rate-limiting transfer of a proton from nitrogen before complex formation takes place, and that this transfer is facilitated with increasing acidity.

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