aboratory 7 Ionization & Classification of Acids, Bases and Salts NAME: DATE: IN

Question

aboratory 7 Ionization & Classification of Acids, Bases and Salts NAME: DATE: INSTRUCTOR: SECTION: WORKSHOP: CONDUCTIVITY OF SOLUTIONS. Answer the following questions during the lab time. 1. The pH of a solution of 0.1M HNO,? 2. The pH of a solution of 0.00001M KOH 3. The pH and POH of a solution of 0.01M HBr? 4. The pH and POH of a solution of 0.00001M KOH 5. the following substances as strong electrolyte (SE), weak electrolyte (WE) and Classify non-electrolyte (NE) a. Glucose, CH b. Carbon tetrachloride, CCI c. Sodium iodide, Nal d. Hydrochloric acid, HCl e. Vinegar f Iron (III) Chloride, FeCl, g. Ethanol CH,OH h, Nitric Acid, HNO, i. Ammonium Hydroxide, NH40H

Explanation / Answer

Q1.

assume HNO3 is strong acid, since NO3- ionizes completely

so

HNO3 <-> H+ + NO3-

and

pH = -log([H+])

then

[HNO3] = [H+] = 0.1 M

pH = -log(0.1) = 1

Q2.

for KOH, assume this is a base so

KOH --> K+ + OH-

pOH = -log([OH-])

[OH-] = [KOH] = 0.00001 M

pOH = -log(0.00001 ) = 5

then

from the equilibrium of water at T = 25°C

14 = pH + pOH

pH = 14- pOH = 14-5 = 9

pH = 9 for KOH

Q3.

for HBr

[H+] = [HBr] = 0.01 M

pH = -log(H) = -log(0.01) = 2

so

pOH = 14-pH = 14-2 = 12

Q4

for KOH:

[OH-] = [KOH] = 0.00001

pOH = 5

pH = 14-5 = 9

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