Which of the following are Arrhenius acids? (a) H2O, (b) Ca(OH)2, (c) H3PO3, (d) HI

Which of the following are Arrhenius bases? (a) H3AsO4, (b) Ba(OH)2, (c) HClO, (d) KOH.

Classify the following as Arrhenius, Bronsted-Lowry, or Lewis acid-base reactions. A reaction may fit all, two, one, or none of the categories:

$\mathrm { Ag } ^ { + } + 2 \mathrm { NH } _ { 3 } \rightleftharpoons \mathrm { Ag } \left( \mathrm { NH } _ { 3 } \right) _ { 2 } ^ { + }$

HCl

Give the formula of the conjugate base:

HPO42-

Give the formula of the conjugate acid:

O2-

Which of the following are Arrhenius acids? Select all that apply. $\ce{A. H2O B. Ca(OH)2 C. HI D. H3PO4}$

For the following equilibrium system, which of the changes will form more CaCO3? $\mathrm { CO } 2 ( \mathrm { g } ) + \mathrm { Ca } ( \mathrm { OH } ) 2 ( \mathrm { s } ) \rightleftharpoons \mathrm { CaCO } 3 ( \mathrm { s } ) + \mathrm { H } 2 \mathrm { O } ( \mathrm { l } ) \Delta \mathrm { H } ^ { \circ } = - 113 \mathrm { kJ }$ (a) Decrease temperature at constant pressure (no phase change), (b) Increase volume at constant temperature, (c) Increase partial pressure of CO2, (d) Remove one-half of the initial CaCO3

Predict the effect of decreasing the temperature on the amounts of reactants in the following reactions:

$\mathrm { C } 2 \mathrm { H } 2 ( \mathrm { g } ) + \mathrm { H } 2 \mathrm { O } ( \mathrm { g } ) \rightleftharpoons \mathrm { CH } 3 \mathrm { CHO } ( \mathrm { g } ) \Delta \mathrm { H } ^ { \circ } \mathrm { r } \mathrm { xn } = - 151 \mathrm { kJ }$,

Assuming acid strength relates directly to number of O atoms bonded to the central atom. rank H2N2O2 [or (HON)2]; HNO3 (or HONO2); and HNO2 (or HONO) in order of decreasing acid strength.

What do Arrhenius acids have in common? What do Arrhenius bases have in common? Explain neutralization in terms of the Arrhenius acid-base definition. What data led Arrhenius to propose this idea of neutralization?

Classify each substance as a strong acid, strong base, weak acid, or weak base. HCCOH HClO4 HI NH3 NaOH HNO2 CH3COOH (CH3)2NH HNO3 Ca(OH)2 HCl KOH HCN HF CH3NH2 CsOH HBr LiOH Ba(OH)2 H2SO4

Predict the effect of increasing the container volume on the amounts of each reactant in the following reactions:

$\mathrm { CH } 3 \mathrm { OH } ( \mathrm { l } ) \rightleftharpoons \mathrm { CH } 3 \mathrm { OH } ( \mathrm { g }$),

The oxidation of nitrogen monoxide is favored at 457 K: $2 \mathrm { NO } ( g ) + \mathrm { O } _ { 2 } ( g ) \rightleftharpoons 2 \mathrm { NO } _ { 2 } ( g )$ $K _ { \mathrm { p } } = 1.3 \times 10 ^ { 4 }$

Calculate Kc at 457 K.