23) b is a weak base. which equilibrium corresponds to the equilibrium constant ka for hb+? a) hb+ (aq) + h2o (l) ⇌ b (aq) + h3o+(aq)b) hb+ (aq) + h3o+(aq) ⇌ h2b2+ (aq) + h2o (l)c) b (aq) + h2o(l) ⇌ hb+ (aq) + oh-(aq)d) hb+ (aq) + oh-(aq) ⇌ b (aq) + h2o (l)e) b (aq) + h3o+(aq) ⇌ hb+ (aq) + h2o (l)

The correct option is: A) HB⁺ (aq) + H₂O (l) ⇌ B (aq) + H₃O⁺ (aq)

Explanation:

The acid dissociation constant (Kₐ) is the equilibrium constant of a given dissociation reaction of an acid. It is also called the acidity constant as it represents the acidic strength of a given species.

The dissociation of a given acid (HA) gives the conjugate base (A⁻) and the hydrogen ion (H⁺).

HA + H₂O ⇌ A⁻ + H₃O⁺

The acid dissociation constant:

Whereas, the dissociation of the conjugate base (BH⁺) of a given weak base (B), gives the base (B) and the hydrogen ion (H⁺).

BH⁺ + H₂O ⇌ B + H₃O⁺

The acid dissociation constant:

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.