HC2 Chapter 19 Round 2

CONCENTRATION

200

[OH^-] = 1 x 10^-10 mol/L, find [H⁺]

1 x 10^-4 mol/L

400

What is the [H⁺] of a solution with a pH of 3.7?

0.00020 M

600

If the pH is 9, what is the [OH^-]?

1 x 10^-5 M

800

Find the molarity of an HCl solution with a volume of 49.0 mL if it is completely titrated by 68.4 mL of a 0.333 M NaOH solution.

0.465 M

1000

Find the molarity of a barium hydroxide solution if 1950 mL is completely titrated by 261 mL of a 0.505 M nitric acid solution.

0.0338 M

POWER of IONS

200

Standard accepted range of pH values.

0-14

400

[H⁺] = 1 x 10^-13 M, find pOH

1

600

[OH^-] = 1 x 10^-12 M, find pH

2

800

Find the pH for a solution with [OH^-] = 0.000003162 M

8.5

1000

Find the pOH for a solution with a [H⁺] = 1 x 10^-7 M

7

Ka

200

How would a substance with a K_a of 1 x 10^-5 be classified?

WEAK ACID

400

Find the acid dissociation constant of a weak monoprotic acid if a 0.5 M solution gives a [H⁺] of 0.0001 M

2 x 10^-8

600

A weak acid of concentration 0.3 M has a [H⁺] = 0.001 M. Find K_a.

3 x 10^-6

800

A 0.500 M solution of a weak acid has [OH-] = 2.49 x 10^-12 M. Find the dissociation constant for it.

3.26 x 10^-5

1000

Carbonic acid, boric acid, and acetic acid would all have this in common about their K_a.

A LOW VALUE

RANDOM

200

Name all acid/base definers.

ARRHENIUS
BRONSTED-LOWRY
LEWIS

400

What is the conjugate base to hydrogen cyanide?

CN^-

600

Name the two ions typically associated with acids.

HYDROGEN

HYDRONIUM

800

Type of element that typically replaces the hydrogen on an acid in a neutralization.

METAL

1000

Give both names for the vinegar based acid.

ACETIC
ETHANOIC