Intro to Acids and Bases

Identify the components

100

For the following reaction, identify the acid, base, conjugate acid, and conjugate base.

HNO₃ + H₂O ---> NO₃^- + H₃O⁺

Acid: HNO₃

Base: H₂O

Conj acid: H₃O⁺

Conj base: NO₃^-

200

For the following reaction, identify the acid, base, conjugate acid, and conjugate base.

HCO₃^- + SO₃^2- ---> CO₃^2- + HSO₃^-

Acid: HCO₃^-

Base: SO₃^2-

Conj acid: HSO₃^-

Conj base: CO₃^2-

300

For the following reaction, identify the acid, base, conjugate acid, and conjugate base.

HS^- + H₂PO₄^- ---> H₂S + HPO₄^2-

Acid:  H₂PO₄^-

Base: HS^-

Conj acid: H₂S

Conj base: HPO₄^2-

400

For the following reaction, identify the acid, base, conjugate acid, and conjugate base.

H₃PO₄ + CH₃COO^- ---> H₂PO₄^- + CH₃COOH

Acid: H₃PO₄

Base: CH₃COO^-

Conj acid: CH₃COOH

Conj base: H₂PO₄^-

500

For the following reaction, identify the acid, base, conjugate acid, and conjugate base.

CO₃^2- + HF ---> HCO₃^- + F^-

Acid: HF

Base: CO₃^2-

Conj acid: HCO₃^-

Conj base: F^-

What's the conjugate?

100

What is the conjugate acid of HSO₄^-?

H₂SO₄

200

What is the conjugate base of HSO₄^-?

SO₄^2-

300

What is the conjugate base of OH^-?

O^2-

400

What is the conjugate acid of OH^-?

H₂O

500

What is the conjugate acid of HC₂O₄^-?

H₂C₂O₄

Definitions

100

Define an Arrhenius acid.

Produces H⁺ or H₃O⁺ in solution.

200

Define a Bronsted-Lowry base.

Proton acceptor

300

Define an Arrhenius base.

Produces OH^- in solution.

400

Define a Bronsted-Lowry acid.

Proton donor.

500

What does it mean to be amphoteric?

The substance can act as an acid or as a base.

(ex. water)

Misc.

100

List at least two properties of acids.

-Sour taste

-Can neutralize bases

-Can dissolve many metals

-Change blue litmus paper to red

200

What is the difference between a strong electrolyte and a weak electrolyte?

A strong electrolyte completely dissociates in water, while a weak electrolyte only partially ionizes.

300

List at least two properties of bases.

-Taste bitter

-Feel slippery

-Can neutralize acids

-Change red litmus paper to blue

400

Differentiate between binary acids and oxyacids.

A binary acid has acidic hydrogens attached to a single nonmetal atom, while an oxyacid has acidic hydrogens attached to an oxygen which is attached to another element.

500

What does it mean to be monoprotic vs polyprotic?

Monoprotic acids have only one acidic hydrogen while polyprotic acids have at least two acidic hydrogens.

Strength

100

What determines the strength of a binary acid?

More electronegative nonmetals make more polar bonds with hydrogen, so acid strength increases across a period.

Weaker bonds make stronger acids, so acid strength decreases down a column.

200

What determines oxyacid strength?

As the element bonded to O is more electronegative, acid strength increases (strength decreases down a column).

More oxygen atoms bonded to the element increases polarity and weakens the bond, increasing the strength of the acid/

300

What is the relationship between acid/base strength and dissociation in solution?

Strong acids/bases fully dissociate while weak acids/bases only partially dissociate.

400

Which acid is stronger, HF or HI?

HI is stronger because its bonds are weaker.

500

Which acid is stronger, HClO or HIO?

HClO is stronger because Cl is more electronegative than I.