7-25 mL of 0.25 M HC2H3O2 are titrated with 0.25 M NaOH. a.What is the pH...

7-25 mL of 0.25 M HC2H3O2 are titrated with 0.25 M NaOH. a.What is the pH after 0mL of NaOH have been added? b.What is the pH after 15mL of NaOH have been added? c.What is the pH after 25 mL of NaOH have been added? d.What is the pH after 30mL of NaOH have been added? I need to have the answer as detailed as possible with all tables and work shown

Expert Solution

queen_honey_blossom answered 1 year ago

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH...

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for CH3CO2H = 1.8X10^-5

20.00 mL of 0.11 M HNO3 is titrated with 0.25 M NaOH.  What volume of...

20.00 mL of 0.11 M HNO3 is titrated with 0.25 M NaOH.  What volume of base is required to reach the equivalence point? Calculate pH at each of the following points in the titration. a) 4.40 mL  b) 8.80 mL  c) 12.00 mL

25 ml of 0.105 M HCl is titrated with 0.210 M NaOH a. What is the...

25 ml of 0.105 M HCl is titrated with 0.210 M NaOH a. What is the ph after 5 ml of the base is added? b. what is the ph at the equivalence point? c. What is the ph after 15 ml of the base added? d. how many ml of the base will be required to reach the end point?

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 15.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...

a volume of 25 ml of .1 m c6h5co2h (aq) is titrated with .1 M naoh...

a volume of 25 ml of .1 m c6h5co2h (aq) is titrated with .1 M naoh (aq) what is the ph after the addition of 12.5 ml of naoh (ka of benzoic acid = 6.3E-5

A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence...

A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence point is reached after 21.27 mL of the base were added. Calculate 1) the concentration of the acid in the original solution, 2) the pH of the original HCl solution and the original NaOH solution, 3) the pH after 10.00 mL of NaOH have been added, 4) the pH at the equivalence point, and 5) the pH after 25.00 mL of NaOH have been...

25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. Calculate the pH...

25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. Calculate the pH of the solution after addition of 50 mL of NaOH. Ka(CH3COOH) = 1.8 x 10-5.

QUESTION 8 25 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. At...

QUESTION 8 25 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. At the equilibrium point of titration, sodium acetate is hydrolyzed by water: CH3COO-(aq) + H2O(l) -> CH3COOH(aq) + OH-(aq) Calculate the concentration of hydroxide ions, OH-, and the pH at the equilibrium. Ka(CH3COOH) = 1.8 x 10-5.

7. Consider the titration of 100.0 mL of 0.120 M HNO2 titrated with 0.100 M NaOH....

7. Consider the titration of 100.0 mL of 0.120 M HNO2 titrated with 0.100 M NaOH. Determine the pH after each of the following situations. Show your calculations explicitly. a.) No base has been added. b.) 20.0 mL of NaOH has been added. c.) 45.0 mL of NaOH has been added. d.) 80.0 mL of NaOH has been added. e.) 120.0 mL of NaOH has been added. f.) 140.0 mL of NaOH has been added.

0.1 M NaOH is titrated with 25 mL acetic acid. The equivalence point was reached at...

0.1 M NaOH is titrated with 25 mL acetic acid. The equivalence point was reached at 23.25 mL. a) Based on your experimentally observed equivalence point of 23.25 mL, calculate the original concentration of the acetic acid that came from the stock bottle. b) Based on your experimentally observed half equivalence point of 11.625 mL pH= 4.8, calculate the Ka of acetic acid. c) Based on your answers to 1& 2 calculate the expected pH at the equivalence point

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