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26 Nov 2019

Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after 100.0 mL of HNO3 have been added.I know the pH is 1.301029996I don't know how many significant figures to go to. Please give the answer in the correct number of sig figs. (Hint: I have tried 1, 1.3, and 1.30. None of them are correct.)

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Elin Hessel
Elin HesselLv2
22 Mar 2019

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Related questions

Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the 20.0 mL of HNO3 have been added.

Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 x 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 has been added.

a. 0.0 mL

b. 20.0 mL

c. 25.0 mL

d. 40.0 mL

e. 50.0 mL

f. 100.0 mL

1) What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 90.0 mL of 0.0509 M NaOH and 60.0 mL of 0.0400 M Ba(OH)2?

2) What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 78.0 mL of 0.604 M HCl and 69.0 mL of 0.823 M NaOH?

3) Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0 mL of 2.54-M HCl to 470. mL of each of the following solutions.

Change is defined as final minus initial, so if the pH drops upon mixing the change is negative.

a) water

pH before mixing =
pH after mixing=
pH change =

b) 0.178 M C2H3O21-

pH before mixing =
pH after mixing=
pH change =

c) 0.178 M HC2H3O2

pH before mixing =
pH after mixing=
pH change =

d) a buffer solution that is 0.178 M in each C2H3O21- and HC2H3O2

pH before mixing =
pH after mixing=
pH change =

4) Calculate the change in pH to 0.01 pH units caused by adding 10. mL of 2.60-M NaOH is added to 550. mL of each of the following solutions.

a) water

pH before mixing =
pH after mixing=
pH change =

b) 0.176 M NH41+

pH before mixing =
pH after mixing=
pH change =

c) 0.176 M NH3

pH before mixing =
pH after mixing=
pH change =

d) a buffer solution that is 0.176 M in each NH41+ and NH3

pH before mixing =
pH after mixing=
pH change =

5)

Consider the titration of 30.0 mL of 0.189-M of KX with 0.172-M HCl. The pKa of HX = 8.59. Give all pH values to 0.01 pH units.

a) What is the pH of the original solution before addition of any acid?

pH =

b) How many mL of acid are required to reach the equivalence point?

VA = mL

c) What is the pH at the equivalence point?

pH =

d) What is the pH of the solution after the addition of 11.2 mL of acid?

pH =

e) What is the pH of the solution after the addition of 39.6 mL of acid?

pH =

6)

A 4.543-g sample of a solid, weak, monoprotic acid is used to make 100.0 mL of solution. 15.0 mL of this solution was titrated with 0.07921-M NaOH. The pH after the addition of 28.38 mL of base was 5.60, and the equivalence point was reached with the addition of 48.60 mL of base.

a) How many millimoles of acid are in the original solid sample? Hint: Don't forget the dilution.

mmol acid

b) What is the molar mass of the acid?

g/mol

c) What is the pKa of the acid?

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A lot of these are similar problems, so if someone could let me know how to do them then I could probably figure the rest of them out. I was out of class the day we went over this and am completely lost.

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