Acids and Bases Review Worksheet Answers PDF

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Acids and Bases Review Worksheet Answers...

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Acids & Bases Review 1. Name the following compounds as acids and circle which are weak acids: a) HNO3

b) H2SO4

c) HF

nitric acid

sulfuric acid

d) H2CO3

hydrofluoric acid

e) HC2H3O2

carbonic acid

2. Write the formulas for the following bases: a) calcium hydroxide b) aluminum hydroxide Ca(OH)2 Al(OH)3

f) H3PO4

acetic acid

phosphoric acid

c) ammonium hydroxide d) lithium hydroxide NH4OH LiOH

3. Complete the following table:

Definition

Acids

Bases

A substance that increases the concentration of H+ (or H3O+) when added to water.

A substance that increases the concentration of OH— when added to water.

or

or

A substance that acts as a proton (H+) donor.

A substance that acts as a proton (H+) acceptor.

H+

OH—

less than 7

greater than 7

sour

bitter

blue turns red

red turns blue

yes

no

Electrolyte in aqueous solution? pH Taste Litmus turns Which reacts with metals to form H2 gas?

Conjugate acid-base pairs: 4. Identify the acid, the base, the conjugate acid and the conjugate base in the reactions:

NH3 (g) + H2O (l)  NH4+(aq) + OH-(aq) base acid conj. acid conj. base HCO3~ (aq) + H2O (l) acid base



CO32~ (aq) + H3O+ (aq) conj. base conj. acid

5. An acid will form the conjugate _base_and a base will form the conjugate _acid__.

Neutralization: 6. Classify the following acids as monoprotic, diprotic or triprotic: a) H2SO4 diprotic

b) H3PO4 triprotic

c) HCl monoprotic

d) HC2H3O2 or CH3COOH (same thing) monoprotic

7. What is the concentration of an unknown NaOH solution if it took an average of 15.4 mL of 0.100 M HCl solution to neutralize 10.0 mL of the NaOH solution? balanced chemical reaction: HCl + NaOH à NaCl + H2O 7&8

moles&of&HCl&used = c×V = 0.100&M&×&15.4&mL× 7999&:8 = 1.54×10;< &moles moles&of&NaOH = moles&of&HCl× conc. of&NaOH =

:@AHI&BCDE J&BCDE&KIHL

=

7&:@A&BCDE 7&:@A&EFA

7.MN×79OP = 9.97999&8

= 1.54×10;< &moles 0.154&M

pH/pOH calculations: 8. A solution has a [H3O+] of 1×10;Q M, what is its pH?____Is this an acid, base or neutral? pH = − log H< OU = − log 1×10;Q = 7 9. What is the pH of a solution if the [H+] = 7.2×10;X M?_____ Is this an acid or base? pH = − log H< OU = − log 7.2×10;X = 8.1 10. If the pH of a solution is 0.8, what is its hydronium ion concentration? ___________ H< OU = 10;ZE = 10;9.[ = 0.2&M 11. What is the pH of a 1.0 M HCl solution? ______ Would this turn litmus paper red or blue? HCl à H+ + Cl— (strong acids fully ionize in water) pH = − log H< OU = − log 1.0 = 0 12. What is the pH of a solution if the [OH—] = 2.0×10;M M? __________ pH = − log OH ; = − log 2.0×10;M = 4.7 pH + pOH = 14 pOH = 14 − pH = 14 − 4.7 = 9.3 13. If the [H+] of a solution is 2.5×10;N M, what is the concentration of the hydroxide ion?_____ Is this solution an acid or a base? K ` = [H U ][OH; ] = 1.0×10;7N 7.9×79 Ocd

[OH ; ] = e.M×79 Od = 4.0×10;77

Ionization of acids and bases: 14. Write the expression for the acid dissociation constant of the strong acid HBr HBr à H+ + Br—

KC =

Ef [ghO ] [Egh]

15. A 0.10 M solution of formic acid, HCOOH, has an equilibrium [H+] = 4.2×10;< M. What is the Ka of formic acid? The equilibrium is shown below: HCOOH (aq) 

H+ (aq)

+

HCOO-(aq)

initial

0.10 M

0

0

change

−x

+x

+x

0+x

0+x

= 4.2×10;< M

= 4.2×10;< M

0.10 − x equilibrium

=0.10 − 4.2×10;< = 0.096 M

KC =

H U HCOO; HCOOH

&&&&&&&=

4.2×10;< 0.096

e

&&&&&&&&&= &1.8×10;N &&&&& note: can use [HCOOH]≈0.10 M at equilibrium...