Dissociation Constants of acids and bases lab report

Calculate and fill out the data tables with the information provided:

CH3COOH
Molarity of CH3COOH (M) 0.1020
Volume of CH3COOH (mL) 10.0
pH (First Reading) Not given
pH (Second Reading) Not given
Average pH 2.77
CH3COOH initially present (moles)
Concentration of H+ @ Equilibrium (M)
H+ present @ Equilibrium (moles)
CH3COO- present @ Equilibrium (moles)
Concentration of CH3COO- @ Equilibrium (M)
CH3COOH present @ Equilibrium (moles)
Concentration CH3COOH @ Equilibrium (M)
Ka
CH3COOH + NaOH
Molarity of NaOH (M) 0.0920
Volume of NaOH (mL) 4.0
pH (First Reading) Not given
pH (Second Reading) Not given
Average pH 4.28
CH3COOH initially present (moles)
CH3COOinitially present (moles)
NaOH present @ Equilibrium (moles)
Concentration NaOH @ Equilibrium (M)
CH3COOH present @ Equilibrium (moles)
Concentration CH3COOH @ Equilibrium (M)
CH3COO- present @ Equilibrium (moles)
Concentration of CH3COO- @ Equilibrium (M)
Concentration of H+ @ Equilibrium (M)
Ka
Average Ka
% Error of Ka

Table 2. Raw, Processed, and Theoretical Data for the Determination of the Dissociation Constant of Phosphoric Acid

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  Mass of Sample

 

Volume H2O

 

Concentration Solution

 

Experimental pH

 

Theoretical pH

 

  (g) (mL) (M)    
NaH2PO4

 

0.609 30.0 4.42
Na2HPO●7H2O

 

0.608 30.0 8.45
Na3PO●12H2O

 

0.224 10.0 11.96 12

Complete the calculations with the information from the data table and show work:

– Acetic Acid

■ Hydrogen ion concentration

■ Ka

■ % Error

– Acetic Acid + NaOH

■ Equilibrium molarity of CH3COOH and CH3COO-

■ Hydrogen ion concentration

■ Ka

– Phosphate Salts

■ Concentration of H2PO4 – and HPO4 2- and PO4 3- solutions

■ Theoretical pH for H2PO4 – and HPO4 2-

■ % Error for pH of H2PO4 – and HPO4 2- and PO4 3-

Answer the discussion questions and be specific:

■ Give a thorough interpretation of your results

■ Based on the today’s experiment describe a process to identify an unknown, weak acid. How would you determine the number of acidic groups present? What calculations should be done?

■ List possible sources of errors in both Parts A and B. State how each error would effect the calculated Ka (part A) and pH (part B) values.

Write a conclusion:

■ Restate the purpose of the experiment

■ How did you attempt to meet the purpose?

■ Was the purpose met?

■ Restate the anticipated outcome. Was the actual outcome close to the anticipated outcome?

■ Why or why not? What errors did you specifically experience in this experiment? – Distance-learning format of the class is not an error

■ What are some future improvements to this experiment? – “Updating the lab manual”, “clear/better instructions on how to perform calculations”, “instructor not explaining the lab procedure”, “do not make the class a distance-learning course”, etc. are NOT future improvements

LAB MANUAL (pg. 213-221)

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