Inorganic Exam 2

Classify the substances as acidic or basic.

Acidic: Aspirin, soda Basic: Detergent, Oven cleaner, household ammonia

Calculate the standard cell potential (Ecell)∘, for the equation Cr(s)+F2(g)⟶Cr2+(aq)+2F−(aq)

3.78

Classify each reactant and product in the reaction as an acid or base according to the Brønsted theory. H3PO4+C6H5O−↽−−⇀H2PO−4+C6H5OH

Acid: H3PO4, C6H5OH, Base: H2PO4-, C6H5O-

Consider the reaction. Classify each reactant and product as an acid or base according to the Brønsted theory.

Acid: HC-=CH, CH3CH2OH Base: CH3CH2O-, HC-=C-

Using the Brønsted theory, classify the compounds as either an acid or a base.

Acid: HCOOH, HNO3 Base: HCOO-, -CH2COOCH3

Classify each reactant and product in this reaction as an acid or base according to the Brønsted theory. HF+H2O↽−−⇀F−+H3O+

Acid: HF, H3O+ (proton donor) Base: F-, H2O (proton acceptor)

Classify each reactant and product in the reaction as an acid or base according to the Brønsted theory. HNO3+(CH3)3CO−↽−−⇀(CH3)3COH+NO−3

Acid: HNO3, (CH3)3COH Base: (CH3)3CO-, NO3-

Classify each species as a Lewis acid or a Lewis base.

Acid: Mg2+, SO3, AlCl3 Base: H-, H2O

Which of the choices is the Lewis definition of acids and bases?

An acid is any species that can accept a lone pair of electrons, and a base is any species that can donate a lone pair of electrons.

Select the correct definition of solvent system acids and bases.

An acid produces more of a solvent's autodissociated cation, and a base produces more of the solvent's autodissociated anion.

Determine whether the equilibrium for the reaction lies to the left or to the right.

Br3In−As(CH3)3+H3B−NH3 ↽−−⇀ Br3In−NH3+H3B−As(CH3)3 ^ left F3B−As(CH3)3+I3Ga−NH3 ↽−−⇀ F3B−NH3+I3Ga−As(CH3)3 ^ right

Label each reactant and product in this reaction as a Brønsted acid or base.

CH3OH + OH- -> CH3O- + H2O acid. base. base. acid

Label each of the reactants.

CHOCH3 is a Lewis base. BF3 is a Lewis acid.

Identify the Lewis acid and Lewis base in each of the reactions.

Cl- + AlCl3 -> AlCl4- base. acid BF3 + F- -> BF4- acid. base NH3 + H+ -> NH4+ base. acid

Which reactant is the Lewis acid and which is the Lewis base?

FeBr3 is the Lewis Acid

For the given reactions, classify each reactant as a Lewis acid-base, a Brønsted-Lowry acid-base, or both.

H2CO3 + H2O -> H+ + HCO3- B. acid. B. base Ni2+ + 6NH3 -> L. acid. L. base Pt + XeF4 -> L. acid L. base HClO4 + CH3CN -> B. acid. B. base

Identify each reactant and product in this reaction as a Brønsted acid or base.

H2Y- + H2Z- -> H3Y + HZ2- Base. Acid. Acid. Base

The strongest acid that can exist in water is The strongest base that can exist in water is

H3O+ OH-

Identify the pair of species that is not a conjugate acid-base pair.

H3PO4; HPO2−4

Label each reactant and product in this reaction as a Brønsted acid or base.

HCN + NH2- -> CN- + NH3 acid. base. base. acid

Complete the acid-base equation for the dissolution of the compound into liquid HFHF solvent. The relevant p𝐾apKa values are given. Be sure to balance the equations and include the appropriate charges. Phases are optional (liquid, aqueous, etc.).

HF + CH3CH2OH -> CH3CH2OH+ + F-

Identify the Brønsted-Lowry acid and base in each of the reactions.

HF + H2O -> F- + H3O+ acid. Base. base acid H2O + H2CO3 -> H3O+ + HCO3- base acid. acid. base

Indicate which reactant is the Lewis acid and which is the Lewis base.

Hydride is Lewis base. Acetone is Lewis acid.

Use the table of standard reduction potentials to complete the problems below.

Identify a substance which can reduce Br2(l) to Br−(aq) but cannot reduce I2(s) to I−(aq). Ag Identify a substance which can oxidize Cd(s) to Cd2+(aq)but cannot oxidize Pb(s) to Pb2+(aq). Co2+

Use the table of standard reduction potentials to answer the questions.

Identify a substance which can reduce Sn4+(aq) to Sn2+(aq) but cannot reduce Sn2+(aq) to Sn(s). Pb Identify a substance which can oxidize Fe(s) to Fe2+(aq) but cannot oxidize Fe2+(aq) to Fe3+(aq).

Label each reactant according to its role (or roles) in the chemical reaction. Check all that apply.

In Reaction 1, the reactant HO− is a: Bronsted Base The reactant HBr is a: Bronsted acid In Reaction 2, the reactant HO− is a: Lewis base The reactant CH3Br is a: Lewis acid

Classify these factors by how they affect the acidity of a metal cation.

Increases metal cation acidity: increased ion charge, increased electronegativity Decreases metal cation acidity: increased ion size

Classify the hydrides as ionic (saline), covalent (molecular), or metallic.

Ionic (saline) : NaH, SrH2 Covalent (molecular) : Ge2H6, HCl, PH3, GeH4, H2Se Metallic : TiH1.7, HfH2

Arrange the metal ions by their acidity in aqueous solution.

Most Ga3+ In3+ Cd+2 Least

Indicate which reactant is the Lewis acid and which is the Lewis base.

Pyridine is a Lewis base. H+ is Lewis acid.

Consider three generic acids: HX, HY, and HZ. Arrange the acids according to strength.

Strongest HX HY HZ Weakest

Write the IUPAC names of the given compounds. Spelling counts.

SiH4: Silane PH3: Phosphane

Classify each of the hydride compounds as a solid, liquid, or gas at room temperature.

Solid: Liquid: water Gas: Hydrogen Iodide, Hydrogen sulfide, silane, phosphine

Determine which of the acids are Arrhenius acids, Brønsted-Lowry acids, and Lewis acids.

Which acids are Arrhenius acids? HCl, AlCl3 Which acids are Brønsted-Lowry acids? HCl, AlCl3 Which acids are Lewis acids? HCl, BCl3, AlCl3

Classify the species as Arrhenius bases, Brønsted-Lowry bases, or Lewis bases in aqueous solution. It is possible for a base to be of more than one type.

Which species are Arrhenius bases? NH3, NaOH Which species are Brønsted-Lowry bases? NH3, NaOH Which species are Lewis bases? NH3, Br-, NaOH

Consider the acid‑base reaction and classify each of the reactants and products as an acid or base according to the Brønsted theory.

acid: CF3COOH, H3O+ base: H2O, CF3COO-

Using the Brønsted theory, classify the compounds as either an acid or a base.

acid: CH3CH2NH3+ , C6H5OH Base: CH3CH2O-

Using the Brønsted theory, classify the compounds as either an acid or a base.

acid: HBr, (CH3)2C=OH+ base: CH3CH2NH2

In a hydrogen fuel cell, hydrogen gas and oxygen gas are combined to form water. Write the balanced chemical equation describing this reaction using the lowest whole‑number coefficients.

chemical equation: 2H2 + O2 -> 2H2O identify the oxidizing agent: O2 identify the reducing agent: H2 number of electrons transferred: 4