CHEM 101-017 Chapter 4: Reactions in Aqueous Solution

Define solution.

Any homogenous mixture that is physically and chemically the same throughout the whole system/reaction.

How many components does a solution have?

Two

What are the components of a solution?

The solvent and solute.

Define the characteristics of a solvent.

They’re present in large amounts; the solvent is usually water in the case of aqueous solutions.

Define the characteristics of a solute.

It’s the substance that is dissolved in the solvent and usually present in small amounts.

What formula is used to the find the molarity or concentration of a substance?

Moles of solute/Liter of solution

What formula is used to dilute concentrated solutions and what does each variable mean?

M1 x V1 = M2 x V2

M1 = initial molarity

V1 = initial volume

M2 = final molarity

V2 = final volume

Give me three types of chemical reactions that we’ll focus on this chapter.

1.) Precipitation Reactions

2.) Acid-Base Neutralization Reactions

3.) Oxidation-Reduction (Redox) Reactions

Define precipitation reactions.

Process in which soluble reactants yield an insoluble solid product that falls out of the reaction.

Define acid-base neutralization reactions.

Process in which an acid reacts with a base to yield water and an ionic compound (salt).

Define oxidation-reduction (redox) reactions.

Process in which one or more electrons are transferred between reactants AND includes oxygen on the reactant side of the balanced equation.

Ionic solids and some polar compounds, such as ____ acids and ____ bases, tend to have the _____ solubility and form ions when dissolved in water.

1.) strong

2.) strong

3.) highest

What is an electrolyte?

Defined as any aqueous solution that conducts electricity in water and substances that dissolve in water produce conducting solutions of ions.

What is a nonelectrolyte?

Substances which do not produce ions in aqueous solutions.

What are some characteristics of weak electrolytes?

They consist of weak acids and weak bases. They partially dissolve in water, resulting in low conductivity.

Is this an example of a strong electrolyte, weak electrolyte, or nonelectrolyte?

Weak electrolyte.

Is this an example of a strong electrolyte, weak electrolyte, or nonelectrolyte?

Strong electrolyte.

Is this an example of a strong electrolyte, weak electrolyte, or nonelectrolyte?

Nonelectrolyte.

What are characteristics of strong electrolytes?

They consist of strong acids and strong bases. They completely dissolve in water, resulting in high conductivity.

What are examples of acid halides and are they characterized as a strong or weak acid? Are they examples of weak or strong electrolytes?

• HF (hydrofluoric acid) - weak acid

• HCl (hydrochloric acid) - strong acid

• HBr (hydrobromic acid) - strong acid

• HI (hydroiodic acid) - strong acid

All of these substances are strong electrolytes, except for HF.

What are examples of Acid oxy halides and are they characterized as a strong or weak acid? Are they examples of weak or strong electrolytes?

• HOF (hypofluorous acid) - weak acid

• HOCl (hypochlorous acid) - weak acid

• HOBr (hypobromous acid) - weak acid

• HOI (hypoiodous acid) - weak acid

All of these substances are weak electrolytes.

What are examples of oxyacids and are they characterized as a strong or weak acid? Are they examples of weak or strong electrolytes?

• HNO3 (nitric acid) - strong acid

• H2SO4 (sulfuric acid) - strong acid

• HClO4 (perchloric acid) - strong acid

• HIO4 (periodic acid) - strong acid

• H2CO3 (carbonic acid) - weak acid

• H3PO4 (phosphoric acid) - weak acid

• HNO2 (nitrous acid) - weak acid

• HCN (hydrocyanic acid) - weak acid

HNO3, H2SO4, HClO4, and HIO4 are strong electrolytes. H2CO3, H3PO4, HNO2, and HCN are weak electrolytes.

What are two types of organic acids, are they strong or weak acids/bases, and do they have strong or weak electrolytes?

• HCOOH (fermic acid) - weak acid

• CH3COOH (acetic acid or vinegar) - weak acid

These substances are weak electrolytes.

What are four examples of non-electrolytes that are soluble in water?

• C2H6O (ethanol)

• C2H6O2 (ethylene glycol)

• C6H12O6 (glucose)

• C12H22O11 (sucrose)

What types of compounds are characterized as a strong electrolyte/strong base?

Group 1 A and Group 2 A elements paired to an OH- ion.

What are examples of strong electrolytes, particularly strong bases?

• NaOH (sodium hydroxide)

• KOH (potassium hydroxide)

• Ba(OH)2 (barium hydroxide)

• Ca(OH)2 (calcium hydroxide)

• And many more

Any element paired to a _____ atom is a weak base!!!!

nitrogen

Strong electrolytes are soluble ____ solids, ____ acids, and ____ bases.

1.) Ionic

2.) Strong

3.) Strong

Is ammonia (NH3) a weak electrolyte and is it a weak acid or base?

NH3 is a weak electrolyte and a weak base.

Waters, soluble alcohols, sugars, and any polar covalent compounds that is not an acid or base are either strong electrolytes, weak electrolytes, or nonelectrolytes?

Nonelectrolyte

Are group one elements (Li+, Na+, K+, Rb+, Cs+) and NH4+ soluble?

Yes, they’re soluble with no exception.

Are NO3-, ClO4-, and C2H3O2- soluble or insoluble in water?

These ions are soluble in water without any exceptions.

Are the halides (F-, Cl-, Br-, I-) soluble? What are its exceptions?

Yes, these ions are soluble except for Ag+, Hg2 +2, and Pb+2.

Is SO4-2 soluble? What are its exceptions?

Yes, sulfate is soluble except for Sr+2, Ba+2, Hg2 +2, and Pb+2.

Is CO3 -2 soluble? What are its exceptions?

No, carbonate is insoluble except for group one elements, ammonium, Ca+2, Ba+2, and Sr+2.

Is S-2 soluble? What are its exceptions?

No, sulfide is insoluble except for group one elements, ammonium, Ca+2, Ba+2, and Sr+2.

Is OH- soluble? What are its exceptions?

No, hydroxide is insoluble except for group one elements, ammonium, Ca+2, Ba+2, and Sr+2.

Is PO4-3 soluble? What are its exceptions?

No, phosphate is insoluble except for group one elements and ammonium.