What is the predominant intermolecular force in liquid CH_3CH_2OH? A) ion-dipole

Question

What is the predominant intermolecular force in liquid CH_3CH_2OH? A) ion-dipole attraction B) ionic bonding C) hydrogen-bonding D) London-dispersion forces E) Induced dipole-dipole attraction Define or illustrate the term "common ion effect" in solution equilibria. The effect of a catalyst on an equilibrium is to ______. A) shift the equilibrium to the right B) slow the reverse reaction only C) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture D) increase the rate of the forward reaction only E) increase the equilibrium constant so that products are favored What is the coefficient of the permanganate ion when the following equation is balanced? MnO_4^- + Br^- rightarrow Mn^2+ + Br_2 (acidic solution) A) 4 B) 1 C) 2 D) 5 E) 3 What is the oxidation number of bromine in the BrO_3^- ion? A) +7 B) +5 C) +3 D) -1 E) +1 A Bronsted-Lowry base is defined as a substance that _____. A) increases [H^+] when placed in H_2O B) acts as a proton donor C) acts as a proton acceptor D) increases [OH^-] when placed in H_2O E) decreases [H^+] when placed in H_2O

Explanation / Answer

14). A combination of salts in an aqueous solution will all ionize according to the solubility products, which are equilibrium constants describing a mixture of two phases. If the salts share a common cation or anion, both contribute to the concentration of the ion and need to be included in concentration calculations.

As one salt dissolves, it affects how well the other salt can dissolve, essentially making it less soluble. Le Chatelier's principle states equilibrium will shift to counter a change when more of a reactant is added.

15) The effect of a catalyst on an equilibrium is to.............. OPTION C: increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture

18) A Brønsted-Lowry base is a proton (hydrogen ion) acceptor.

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