Exp06 –

Titration Curves Application Questions.

No work, no credit, no kidding.

 

1. Weak acid with a strong base: 25mL of 0.2M HCOOH + 0.1M NaOH.         

 

1. Write out the balanced chemical equation representing the reaction corresponding to the acid/base titration:

 

Molarity do we neeed to convert th

2. pH before any NaOH is added: __2.22__________________

 

1. Volume of NaOH at the equivalence point: ________________________

 

1. pH at the equivalence point: ______________________________

 

1. Volume of NaOH at half equivalence point: ________________________

 

1. pH of solution at half-equivalence point: ________________________

 

1. Buffering range of weak acid (“linear” portion of graph): _______________________

Hint: Buffer capacity is +/- 1pH unit from pKa

1. after equivalence point; pH at 100mL 0.1M NaOH added: ____________________

Hint: pOH = -log( )

From all of your above data, sketch the titration curve of the titration of 25mL 0.2M HCOOH with 0.1M NaOH, Label x-axis and y-axis, include data points in your graph that you calculated from above.  Put a point on the graph for above values B, D, F, H. Indicate where the equivalence point and half-equivalence point are.

2. Strong acid with a strong base: 20mL 0.2M HCl + 0.1M NaOH

 

1. Write out the balanced chemical equation representing the reaction corresponding to the acid/base titration:

 

1. pH before any NaOH is added: ____________________

 

1. Volume of NaOH at the equivalence point: ________________________

 

1. pH at the equivalence point: ______________________________

 

1. Volume of NaOH at half equivalence point: ________________________

 

1. pH of solution at half-equivalence point: ________________________

 

1. after equivalence point; pH at 100mL 0.1M NaOH added: ____________________

Hint: pOH = -log( )

 

From all of your above data, sketch the titration curve of the titration of 20 mL 0.2M HCl with 0.1M NaOH, Label x-axis and y-axis, include data points in your graph that you calculated from above.  Put a point on the graph for above values B, D, F, G. Indicate where the equivalence point and half-equivalence point are.

 

3. Weak base with a strong acid: 25mL 0.1M NH₃ with 0.1M HCl

 

1. Write out the balanced chemical equation representing the reaction corresponding to the acid/base titration:

 

 

 

1. pH before any HCl is added: ____________________

 

1. Volume of HCl at the equivalence point: ________________________

 

1. pH at the equivalence point: ______________________________

 

1. Volume of HCl at half equivalence point: ________________________

 

1. pH of solution at half-equivalence point: ________________________

 

1. Buffering range of weak base (“linear” portion of graph): _______________________

Hint: Buffer capacity is +/- 1 pH unit from pKa

 

1. after equivalence point; pH at 100mL 0.1M HCl added: ____________________

Hint: pH = -log( )

From all of your above data, sketch the titration curve of the titration of 25mL 0.1M NH₃ with 0.1M HCl, Label x-axis and y-axis, include data points in your graph that you calculated from above.  Put a point on the graph for above values B, D, F, H. Indicate where the equivalence point and half-equivalence point are.

4. Propose a sketch of a titration curve for the titration of 0.1M H₂SO₄ (a diprotic acid; analyte) with 0.1M NaOH. (titrant). In a few sentences, justify the shape of your curve. Notice there is no volumes given, you do not need to be accurate like the questions above. I am looking for overall shape and justification of your graph.