2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH....

2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH.

2A. Write the net ionic equation for the reaction of phosphoric acid with NaOH to form sodium phosphate and water:

2. What is the pH of the titration medium after the addition of the following volumes of NaOH titrant:

2B. 0.00 mL

: 2C. 12.50 mL:

2D. 15.00 mL:

2E. 25.00 mL:

2F. 37.50 mL:

2G: 50.00 mL

2H.60.00 mL

2I. 62.50 mL:

2J. 75.00 mL:

2K. 85.00 mL

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M NaOH, calculate the...

For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M NaOH, calculate the pH of the reaction mixture after each of the following total volumes of base have been added to the original solution. (Remember to take into account the change in total volume.) Select a graph showing the titration curve for this experiment. (a) 0 mL (b) 10.00 mL (c) 24.90 mL (d) 24.99 mL (e) 25.00 mL (f) 25.01 mL (g) 25.10 mL (h) 26.00...

Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH...

Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. What will the pH of the analyte be if 10.00 mL of NaOH is added?

Consider the titration of 25.00 mL of 0.0200 M MnSO4 with 0.0100 M EDTA at a...

Consider the titration of 25.00 mL of 0.0200 M MnSO4 with 0.0100 M EDTA at a pH of 8.00. Calculate the value of pMn+2 after adding the following EDTA volumes: a. 0.00 mL b. 15.00 mL c. 50.00 mL d. 55.00 mL

titration of 25.00 ml of 0.100M CH3COOH with 0.100 M NaOH (weak acid, strong base) a)...

titration of 25.00 ml of 0.100M CH3COOH with 0.100 M NaOH (weak acid, strong base) a) calculate the initial pH ( kb = 1.8 x10 ^-5) b) why is pH > 7 at the equivalence point? c) calculate the pH at the equivalence point

Consider the titration of 25.00 mL of 0.08313 M KI with 0.05210 M AgNO3. Calculate pAg+...

Consider the titration of 25.00 mL of 0.08313 M KI with 0.05210 M AgNO3. Calculate pAg+ at the following volumes of added AgNO3. (a) 38.46 mL (b) Ve (c) 43.31 mL Ve is the volume at the equivalence point and pAg+=-log[Ag+]

Consider the titration of a 22.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH....

Consider the titration of a 22.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH. Determine each of the following. Part E the pH at the equivalence point Express your answer using two decimal places. Part F the pH after adding 6.00 mL of base beyond the equivalence point Express your answer using two decimal places.

Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH....

Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH. Determine each of the following. a. the volume of added base required to reach the equivalence point b.the pH after adding 6.00 mL of base beyond the equivalence point Express your answer using two decimal places.

Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH....

a. Consider the titration of 25.0 mL of 0.065 M HCN with 0.065 M NaOH. What...

a. Consider the titration of 25.0 mL of 0.065 M HCN with 0.065 M NaOH. What is the pH before any NaOH is added? What is the pH at the halfway point of the titration? What is the pH when 95% of the NaOH required to reach the equivalence point has been added? What is the pH at the equivalence point? pH initial---------------------------------- pH at halfway-------------------------- pH when 95% is added-------------------------- pH at the equivalence point---------------------

Consider the titration of a 24.0 −mL sample of 0.100 M HC2H3O2 with 0.120 M NaOH....

Consider the titration of a 24.0 −mL sample of 0.100 M HC2H3O2 with 0.120 M NaOH. Determine each of the following. Part A the initial pH Express your answer using two decimal places. pH = SubmitMy AnswersGive Up Part B the volume of added base required to reach the equivalence point V = mL SubmitMy AnswersGive Up Part C the pH at 6.00 mL of added base Express your answer using two decimal places. pH = SubmitMy AnswersGive Up Part...

Subjects