Effect of water viscosity (increased due to NaCl concentration) on dissolution rate of CO2 We did an experiment involving different $\ce{NaCl}$ concentration(ranging, 1-4%) on 100 mL of water. Our aim of the experiment was to find the dissolution rate of $\ce{CO2}$in the brine solvent. We did some research and found that $\ce{NaCl}$ increases the viscosity of the solvent, which in-turn decreases the dissolution rate. We want to explain how the entire process works, in a microscopic level.

Answers with good source would be good.
By dissolving NaCl you increase the ionic strength of the solution, i.e. there is more electrostatic attraction between the layers of water increasing the viscosity. Carbon dioxide is non-polar, so by increasing the polarity of the solvent, the carbon dioxide tend to form less interactions with the solvent.