The energy of an electrostatic interaction between two charged atoms is dependent on the charges on the atoms, the distance between them, and the dielectric constant of the solvent. for example, the strength of a weak acid (ka, acid dissociation constant) depends on the strength of the electrostatic interaction between a negatively charged carboxylic acid group and a proton. the solvent dielectric constant has a large influence on the pka for weak acids. select the statements that correctly explain the influence of two solvents, water and hexane, on the pka of acetic acid. in water, the association of ch3coo– and h will be favored because charge-charge interactions are stronger in water. nonpolar solvents like hexane will weaken charge-charge interactions resulting in more dissociation of h .the pka will be higher in hexane. hexane cannot affect the pka of acetic acid since hexane cannot donate or accept h .more h will dissociate in water because the dielectric constant is higher.

What volume of a 2.00 m stock solution of naoh is needed to prepare 150. ml of 0.40 m solution?

Compare the equilibrium constants for the systems shown in the table. which favors products the most? which favors products the least? rank these systems in order from most to least in terms of favoring products rather than reactants. d > b > a > c c > a > b > d b > c > d > a a > d > c > b

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced