Chapter 16

H+,OH- (Hydrogen Ion, Hydroxide)
Explanation: Arrhenius acids are compounds that release H+ ions when dissolved in water. Arrhenius bases are compounds that release OH- ions when dissolved in water. Therefore, the two ions central to the Arrhenius definitions of acids and bases are H+ and OH-.

SO3{2-}
Explanation: The conjugate base of HSO3 is SO3-.

H2PO3-
Explanation: The conjugate acid of HPO32- is H2PO3-.

A monoprotic acid is an acid that donates only one proton or hydrogen atom per molecule to an aqueous solution. This is in contrast to acids capable of donating more than one proton or hydrogen, which are called polyprotic acids.
Explanation: Monoprotic acids are acids that donate one proton per molecule during acid-base reactions. In aqueous solution, monoprotic acids dissociate into H+ ions and the conjugate base of the acid. Common examples of monoprotic acids include acetic acid (CH3COOH) and hydrochloric acid (HCl).

Negligible Basicity. Because Perchloric Acid is a strong acid, it's Conjugate Base, ClO4- is Weak, and is negligible because it's not that basic.
Explanation: ClO4- is a weak base.

.001 M of Ba(OH)2.

Hydrochloric Acid (HCl) Hydrobromic Acid (HBr) Hydroiodic Acid (HI) Nitric Acid (HNO3) Perchloric Acid(HClO4) Sulfuric Acid (H2SO4)
Explanation: There are six common strong acids: hydrochloric acid, sulfuric acid, nitric acid, chromic acid, perchloric acid, and hydrofluoric acid. These acids are all highly corrosive and can cause serious damage to living tissue.

Ba(OH)2 >NaOH > N2H4 > HOCl> HCl Ba(OH)2 is a strong base and will dissociate completely at concentrations of 0.01M or less. NaOH is also a strong base, but it will dissociate completely at a concentration of 1.0M not at 0.01M, making Ba(OH)2 the stronger base out of the two strong bases in the list. N2H4 is a weak base, and HOCl and HCl are both acids.
Explanation: The highest pH would be from the Ba(OH)2 followed by the NaOH, N2H4, HOCl, and HCl.

10,56
Explanation: The pH of N2H4 is determined by the Kb of the molecule. The Kb is the equilibrium constant for the dissociation of the molecule into its component ions. The Kb for N2H4 is 1.3*10^-6. This means that at equilibrium, there are 1.3*10^-6 moles of H+ ions for every mole of N2H4. The pH is then determined by the concentration of H+ ions in the solution. The concentration of H+ ions is equal to the Kb divided by the concentration of N2H4. The concentration of N2H4 is 1.3*10^-6 moles/L. Therefore, the concentration of H+ ions is 1.3*10^-6 moles/L. The pH of the solution is then -log(1.3*10^-6). The pH of the solution is 5.89.

4,23
Explanation: The pH of HOCl is 3.5. The reason for this is because the Ka for HOCl is 3.5*10^-8. This means that the concentration of H+ ions in HOCl is 3.5*10^-8 moles/L. Since the pH is defined as the -log[H+], the pH of HOCl is 3.5.

LiNO3,- neutral (salt of a strong acid and a strong base) SrBr2, -neutral (salt of a strong acid and a strong base) NH4ClO4,-acidic (salt of a strong acid and a weak base) KCN, - basic (salt of a weak acid and a strong base) NH4Br = acid NH4CN- basic, LiF = basic
Explanation:The pH of HOCl is 3.5. The reason for this is because the Ka for HOCl is 3.5*10^-8. This means that the concentration of H+ ions in HOCl is 3.5*10^-8 moles/L. Since the pH is defined as the -log[H+], the pH of HOCl is 3.5.

NO3- ions will not affect the pH. It is the weak conjugate base of Strong Acid HNO3. Carbonate ions are obtained from weak acids H2CO3 and HCO3-, so the conjugate base CO3{2-} wil l be strong and accepts protons from water.
Explanation: NO3- ions will affect the pH of a solution because they are acidic. CO3{2-} ions will not affect the pH of a solution because they are neutral.