7A

strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO4, HClO3

HNO3

strong electrolyte

Steps for Metathesis reactions

1) Use the chemical formulas of the reactants to determine which ions are present. 2) Write formulas for the products: cation from one reactant, anion from the other. Use charges to write proper subscripts. 3) Check your solubility rules. If either product is insoluble, a precipitate forms. 4) Balance the equation.

If you have an aqueous solution that contains 1.5 moles of HCl, how many moles of ions are in the solution?

3 moles

Solution

A homogeneous mixture of two or more substances

Predict the identity of the precipitate that forms when aqueous solutions of BaCl2 and K2SO4 are mixed.

BaSO4

Which solute will cause the light bulb in the previous slide to glow most brightly, CH3OH, NaOH, or HC2H3O2? Why?

CH3OH is not an electrolyte NaOH is a strong electrolyte (this one) HC2H3O2 is a weak electrolyte

What compound precipitates when aqueous solutions of Fe2(SO4)3 and LiOH are mixed?

Fe(OH)3

Metathesis Reactions

It appears as though the ions in the reactant compounds exchange, or transpose, ions Ex. AgNO3(aq) + KCl(aq) ⎯→ AgCl(s) + KNO3(aq)

strong bases

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

C2H5OH

nonelectrolyte

What are the 3 ways to write a metathesis reaction

Molecular equation Complete ionic equation Net ionic equation

Gas Forming reactions

Substances other than hydroxide containing compounds can react with the hydrogen cations (H+) in acids to form insoluble compounds in the gaseous state.

If you were to draw diagrams representing aqueous solutions of (a) NiSO4, (b) Ca(NO3)2, (c) Na3PO4, (d) Al2(SO4)3, how many anions would you show if each diagram contained six cations?

a) 6 b) 12 c) 12 d) 9

dissociate

When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them.

precipitate

When two solutions containing soluble salts are mixed, sometimes an insoluble salt will be produced. A salt "falls" out of solution

Diprotic acids

Yield two H+ per molecule of acid (H2SO4)

Electrolyte

a substance that dissociates into ions when dissolved in water

What dissolved species are present in a solution of KCN? CCl4? NaClO4?

a) KCN -> K+ + CN- b) CCl4 -> individual CCl4 c) NaClO4 -> Na+ + ClO4-

NH3

accepts an H+ ion from water molecule and thereby produces an OH- ion Ammonia is a weak electrolyte because only about 1% of the NH3 forms NH4+ and OH-

organic acids

acidic hydrogen is the one that is attached to the oxygen in the -COOH functional group, aka carboxyl group. weak and do not ionize completely

complete (total) ionic equation

all strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions. Ex. Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq) ⎯→ AgCl(s) + K+(aq) + NO3−(aq)

Solutes

are dissolved in the substance

strong electrolyte

dissociates completely when dissolved in water (ionic compounds, strong acids/bases)

carbonates/bicarbonates with acids

form CO2 (g), H2O (l), and an ionic salt Ex. Molecular: CaCO3(s) + 2 HCl(aq) ⎯→CaCl2(aq) + CO2(g) + H2O(l) Net:CaCO3(s) + 2H+(aq) ⎯→ Ca2+ + CO2(g) + H2O(l)

Ammonia with bases

form NH3(g), H2O (l), and an ionic salt. ex. Molecular Equation: NH4Cl + NaOH → NaCl + NH3 (g) + H2O(l) Net Ionic Equation: NH4+ (aq) + OH- (aq) → NH3 (g) + H2O(l)

Sulfites/bisulfite with acid

form SO2 (g), H2O (l), and an ionic salt Ex. Molecular Equation: Na2SO3 (aq) + 2 HCl(aq) → 2 NaCl (aq) + SO2(g) + H2O(l) Net Ionic Equation: SO32- (aq) + 2 H+ (aq) → SO2 (g) + H2O(l)

Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of silver nitrate and potassium phosphate are mixed. Which ions remain in solution, unreacted, after solutions potassium carbonate and magnesium sulfate are mixed? Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: K+, Pb2+, Ba2+?

idk man

Organic acid example: CH3COOH

leaving CH3COO- (acetate ion) and H+

nonelectrolyte

may dissolve in water, but it does not dissociate into ions when added to water (instead it breaks into individual molecules or atoms)

COOH

means its an acid

Will a precipitate form when solutions of Ba(NO3)2 and KOH are mixed?

no

Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of calcium chloride and sodium carbonate are mixed.

notes

weak electrolyte

only dissociates partially when dissolved in water (weak acids and bases).

Solvent

present in the greatest abundance (does the dissolving)

bases Bronsted Lowry

proton acceptor

Acid (Bronsted-Lowry)

proton donor

Metal suflide with acid

salt and H2S ex. Molecular: Na2S(aq) + 2 HCl(aq) → 2 NaCl(aq) + H2S(g) Net: 2 H+ (aq) + S2- (aq) → H2S(g)

Net Ionic equation

show only the soluble, strong electrolytes (represented by ions) and omit the spectator ions, which go through the reaction unchanged ex. Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq) ⎯→ AgCl(s) + K+(aq) + NO3−(aq) Ag+(aq) + Cl−(aq) ⎯→ AgCl(s)

CaCl2

strong electrolyte

Acid (Arrhenius)

substances that increase the concentration of H+ when dissolved in water

Bases (Arrhenius)

substances that increase the concentration of OH- when dissolved in water

Although H2SO4 is a strong electrolyte, (ASK WHYYYYY)

sulfuric acid contain a mixture of H+, HSO4-, and SO42

acid-base reaction (aka neutralization reaction)

the acid donates a proton (H+) to the base

aq

the ions are dissacioted

spectator ions

the ions crossed out

When the base is a metal hydroxide

water and a salt (an ionic compound) are produced in an acid base reaction

Aqueous solution

when water is the solvent

Monoprotic acids

yield one H+ per molecule of acid (ex. HNO3, HCl)