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Misc. Acid misc. Base misc. Acid base definition

s

TitrationpH/pOH

Acids produce ____ ions in water

A 100

Hydronium; H3O+

A 100

Kw= ___x___=___

A 200

[H+]; [OH-]; 1.00x10-14

A 200

Organic acids have a _____ backbone and a ______ group

A 300

Carbon; carboxyl (COOH)

A 300

What are dyes with pH-sensitive colors used for in

Chemistry?

A 400

Acid/base indicators

A 400

Give two examples of compounds that could be

produced by a neutralization reaction

A 500

H2O; NaCl; NH4Cl; KCl; KNO3; Ba(NO3)2; must have an ionic

compound (salt) and water

A 500

Acids make (blue) litmus paper turn this color

B 100

Red

B 100

Strong acids react with ____ to produce _____ and _____

B 200

Bases; salt; water

B 200

Give an example of an oxyacid

B 300

H2SO4; H3PO4; HNO3

B 300

Which acid is produced in your stomach?

B 400

Hydrochloric acid (HCl)

B 400

List 4 strong acid names with their formulas

B 500

Hydrochloric acid HCl, hydrobromic acid HBr, hydroiodic acid HI, nitric acid HNO3, sulfuric

acid H2SO4; perchloric acid HClO4

B 500

Bases either contain or react with water to form which ion

C 100

OH-

C 100

A strong base _______ completely and conducts

_______ in water

C 200

Dissociates; electricity

C 200

Where on the periodic table can you find metals that will form strong bases (with hydroxide)? Are

all those bases strong?

C 300

Group 1; yes

C 300

DAILY DOUBLE

C 400

DAILY DOUBLE

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Write a chemical equation that shows how ammonia

reacts with water

C 400

NH3 + H2O => NH4+ + OH-

C 400

Calculate the hydroxide ion concentration in a solution

with a hydrogen ion concentration of 1.00x10-4

C 500

1.00x10-10

C 500

Arrhenius acids and bases form ___ in water

D 100

Ions

D 100

Arrhenius bases would increase the concentration of

which ion in aqueous solutions?

D 200

Hydroxide

D 200

Bronsted-Lowry acids and bases donate or accept _____

D 300

Protons

D 300

Tell whether these acids would form weak or strong conjugate bases: acetic acid, hydrochloric acid, sulfurous

acid

D 400

Strong, weak, strong

D 400

A Lewis acid ____ electron pairs, while a Lewis base

____ electron pairs

D 500

Accepts; donates

D 500

What quantities must be known before beginning a titration?

E 100

Concentration of either the acid or the base and the

volume of the substance with the unknown concentration

E 100

What quantity or quantities are measured during a

titration?

E 200

Volume of base (or acid if that’s the substance in the

buret)

E 200

A 750 mL sample of 1 M HCl is titrated with 0.5 M NaOH.

What volume of NaOH is required to reach the endpoint

of the titration?

E 300

1.5 L

E 300

If 15 mL of a 5 M NaOH solution is needed to titrate 20 mL of HCl, what is the

molarity of the HCl?

E 400

3.75 M

E 400

Calculate the volume of 2.0 M Ba(OH)2 that is required to titrate 10 mL of 0.05 M nitric

acid.

E 500

0.125 mLNitric acid reacts with barium hydroxide as

expressed in the following reaction: 2HNO3 + Ba(OH)2 => Ba(NO3)2 + 2H2O

The reaction products are barium nitrate and water. The barium nitrate is a salt, and in the

classic acid-base reaction, the products are a salt and water.

E 500

Acids have pH under __; neutral solutions have a pH of __; basic solutions have a pH

over __

F 100

7

F 100

pH=?; fill in the formula

F 200

-log[H+]

F 200

pH + pOH= ___

F 300

14

F 300

A solution with a high pH has a ___ pOH

F 400

Low

F 400

What is the hydronium ion concentration of a solution

whose pH is 2.3?

F 500

5.0x10-3

F 500

The Final Jeopardy Category is:

Acid/base definitions

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What is the main assumption that the Arrhenius theory makes?

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Acids and bases must produce ions in solution because they

conduct electricity

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