Acid and Complete Neutralization Ml
EXPERIMENT 19: Properties and Reactions of Acids-Bases
REPORT FORM
Instructor ________________________ Date ____________________________ Partner’s Name: ___________________ Results and Observations Name ___________________________
I. & II. Conductivity and pH of Acid/Base Solutions:
Solution
Strong or Weak Conductivity
Strong or Weak Acid/Base
pH
0.1 M HCl (aq) 0.1 M HC2H3O2 (aq) 0.1 M NaOH (aq) 0.1 M NH3 (aq) Question 1. Both acids above have the same concentration, 0.1 M, but they exhibit different pH value. Explain.
Question 2. Both bases above have the same concentration, 0.1 M, but pH of NH3(aq) is lower than that of
NaOH. Explain.
7
III.
a) Observation of HCl/NaOH product. b) Identity of the product: c) Write the reaction occurred between HCl and NaOH. __________________________________________________________________________
IV.
Monitoring Neutralization Reactions by Use of Different Indicators:
Color Of Acid Solution After Adding Phenolthalein # Of Drops Of Base Added For Complete Neutralization mL of Base Added The Color of Solution At the Point of Complete Neutralization
20 Drops of 1.0 M Acid
HCl HC2H3O2
20 Drops of 1.0 M Acid
Color of Acid Solution After Adding Universal Indicator
# Of Drops Of Base Added For Complete Neutralization
mL of Base Added
The Color of Solution At the Point of Complete Neutralization
HCl HC2H3O2
V. Heat of Neutralization: Acid Initial T, oC Highest T , oC after adding NaOH Is reaction exo- or endothermic?
HCl HC2H3O2
8
EXPERIMENT 19: Properties and Reactions of Acids-Bases
Name ___________________________ Pre- laboratory Questions and Exercises
Due before lab begins. Answer in space provided. 1. Define neutralization.
2. Give two examples of balanced chemical equations for neutralization reaction. (other than HCl and NaOH)
3. Provide definitions for the following terms; a) Bronsted-Lowry acid and base
b) Acidic, basic, and neutral
REPORT FORM
Instructor ________________________ Date ____________________________ Partner’s Name: ___________________ Results and Observations Name ___________________________
I. & II. Conductivity and pH of Acid/Base Solutions:
Solution
Strong or Weak Conductivity
Strong or Weak Acid/Base
pH
0.1 M HCl (aq) 0.1 M HC2H3O2 (aq) 0.1 M NaOH (aq) 0.1 M NH3 (aq) Question 1. Both acids above have the same concentration, 0.1 M, but they exhibit different pH value. Explain.
Question 2. Both bases above have the same concentration, 0.1 M, but pH of NH3(aq) is lower than that of
NaOH. Explain.
7
III.
a) Observation of HCl/NaOH product. b) Identity of the product: c) Write the reaction occurred between HCl and NaOH. __________________________________________________________________________
IV.
Monitoring Neutralization Reactions by Use of Different Indicators:
Color Of Acid Solution After Adding Phenolthalein # Of Drops Of Base Added For Complete Neutralization mL of Base Added The Color of Solution At the Point of Complete Neutralization
20 Drops of 1.0 M Acid
HCl HC2H3O2
20 Drops of 1.0 M Acid
Color of Acid Solution After Adding Universal Indicator
# Of Drops Of Base Added For Complete Neutralization
mL of Base Added
The Color of Solution At the Point of Complete Neutralization
HCl HC2H3O2
V. Heat of Neutralization: Acid Initial T, oC Highest T , oC after adding NaOH Is reaction exo- or endothermic?
HCl HC2H3O2
8
EXPERIMENT 19: Properties and Reactions of Acids-Bases
Name ___________________________ Pre- laboratory Questions and Exercises
Due before lab begins. Answer in space provided. 1. Define neutralization.
2. Give two examples of balanced chemical equations for neutralization reaction. (other than HCl and NaOH)
3. Provide definitions for the following terms; a) Bronsted-Lowry acid and base
b) Acidic, basic, and neutral