) SHOW ALL YOUR WORK 2) use the periodic table provided for +he class 3) Don't forget Sig. fig. & unit ACID-BASE TITRATION * NAME: DATA TABLES STANDARDIZATION OF THE 0.100 M NaOH SOLUTION WITH POTASSIUM HYDROGEN PHTHALATE (KHP), KHC8H4O4 PART 2 Write a balanced equation for the reaction between KHC8H404 and NaOH: NOOH t KH Co HuOy 7 NakGo Hy OytH20 ACID DATA, KHP (KHC8H404) TRIAL NUMBER: # 1 # 2 #3 # 4 Mass of KHP used 0.220 0.246 0.237 g g BASE DATA (NaOH) A burette can be read two places after the decimal; XX.XX ±0.01 mL! Normally burette readings contain four significant figures! Final NaOH 10.96 23.29 35.00 mL burette reading mL mL mL Initial NaOH 0.00 mL -10.96 23.29 mL mL eth burette reading mL Volume of 11.71 12.33 m 0.977 10.96 mL mL mL NaOH used Molarity of NaOH solution 0.009 M 0.099 M M M Average Molarity of the NaOH solution 0.392 Use this molarity in all future stoichiometric calculations involving NaOH. If you look at PART 2 (Standardization of the 0.100 M NaOH solution with potassium hydrogen phthalate, KHC8H4O4, Theoretical Part, Letter a) * Show NaoH molarity calculation for each trial on the last page of the manual * The NaOH solution was made to have a molarity of 0.100 M. What is the percentage error? If there is a % error, it is a reflection of the stockroom's work and not of your making. % Error 士
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![1) SHOW
2) use the periodic table provided for the class
3) Don't forget sig. fig. & unit
ALL YOUR WORK
SHOW
use 1
Don'4
CID-BA
OST LA
ACID-BASE
TITRATION
H NAME:
DATA TABLES
849
STANDARDIZATION OF THE 0.100 M NaOH SOLUTION WITH
POTASSIUM HYDROGEN PHTHALATE (KHP), KHC8H404
ns or
PART 2
ne ma
Write a balanced equation for the reaction between KHC8H4O4 and NaOH:
NaOH + KH CaHuDy
7 NäkGo HyOy +H20
HO
ACID DATA, КНР (КНС;НДО4)
TRIAL NUMBER:
# 1
#2
#3
#4
0.220g
0.246
0.237
Mass of KHP used
g
A burette can be read two places after the decimal; XX.XX ±0.01 mL!
Normally burette readings contain four significant figures!
BASE DATA
(NaOH)
Final NaOH
2.
he
10.96
23.29
35.00 mL
burette reading
_mL
mL
mL
Initial NaOH
0.00
- 10.96
- 23.29
ch
burette reading
mL
mL
mL
CEES
mL
Volume of
10.96mL 12.33 mL
11.71
mL
mL
NaOH used
Molarity of
NaOH solution
0.099 M
0.977M 0.099 m
M
Average Molarity of the NaOH solution 0.392
Use this molarity in all future stoichiometric calculations involving NaOH. If you look at
PART 2 (Standardization of the 0.100 M NaOH solution with potassium hydrogen phthalate, KHC8H4O4,
Theoretical Part, Letter a)
* Show NaOH molarity calculation for each trial on the
last page of the manual *
The NaOH solution was made to have a molarity of 0.100 M. What is the percentage
error? If there is a % error, it is a reflection of the stockroom's work and not of your
making.
% Error
士
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