Question

A sample of 180.0 mL of 1.65M HNO3 is titrated with 0.90M KOH. Fill in the...

A sample of 180.0 mL of 1.65M HNO3 is titrated with 0.90M KOH. Fill in the following table for each different point (a, b, c, etc….) during the titration. Also graph the titration curve with pH on the y­axis and Vbase on the x­axis (Make sure all work is attached for credit)

Point |Vbase (mL)| molbase added| mol acid remain| molbase remain| [OH ­ ]| [H3O + ]| pH|

a            0.00

b           75.00

c           200.25

d           275.50

e            Veq=

f            400

Homework Answers

Answer #1

The equivalence point EP is at V:

V x 0.90 mol/L = 0.180 L x 1.65 mol/L    

V= 0.33 L = 330 mL KOH

For the Excel Table

Initial acid quantity is

0.180 L x 1.65 mol/L = 0.297 mol

Base, mol is    Vb/1000 x 0.9 M

Acid remain, mol     0.297-Base

Base remain, mol     Base – 0.297

point

Vb, mL

base, mol

acid remain,mol

base remain, mol

pH

pOH

[H+]

[HO-]

a

0

0

0.297

0

0.53

13.47

0.297

3.37E-14

b

75

0.068

0.230

0

0.64

13.36

0.230

4.36E-14

c

200.25

0.180

0.117

0

0.93

13.07

0.117

8.56E-14

d

275.5

0.248

0.049

0

1.31

12.69

0.049

2.04E-13

e EP

330

0.297

0

0

7

7

1.00E-07

1.00E-07

f

400

0.36

0

0.063

12.80

1.20

1.59E-13

0.063

Do a graph by hand using pH versus Vb columns.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A sample of 447.9 mg of hydroxylamine (NH2OH) is dissolved in 55.5 mL of DI H2O....
A sample of 447.9 mg of hydroxylamine (NH2OH) is dissolved in 55.5 mL of DI H2O. This sample is to be titrated with 0.315 M HClO4 . Fill in the following table for each different point (a, b, c, etc….) during the titration. (Make sure all work is attached for credit). Also graph the titration curve with pH on the y­axis and Vbase on the x­axis. Point |Vbase (mL)| molbase added| mol acid remain| molbase remain| [OH ­ ]| [H3O...
A 15.00 mL of 0.250 M HNO3 (aq) is titrated with 30.0 mL of 0.175 M...
A 15.00 mL of 0.250 M HNO3 (aq) is titrated with 30.0 mL of 0.175 M KOH (aq). d.) After neutralization, how many moles of excess reactant remain? e.) What is the pH for this titration mixture?
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the...
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addition of the following volumes of acid. a) 0.0 mL b) 15.0 mL c) At the equivalence point d) 40.0 mL
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid...
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the first equivalence point occur? 20.8 mL of 0.146 M diprotic acid (H2A) was titrated with 0.14 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the second equivalence point occur? Consider the titration of...
When 25.00 mL of HNO3 are titrated with Sr(OH)2, 58.4mL of a .218M solution are required....
When 25.00 mL of HNO3 are titrated with Sr(OH)2, 58.4mL of a .218M solution are required. a. What is the pH of HNO3 before titration? b. What is the pH at the equivalence point? Please write out formulas and explain where you got the numbers.
For all of the following questions 20.00 mL of 0.192 M HBr is titrated with 0.200...
For all of the following questions 20.00 mL of 0.192 M HBr is titrated with 0.200 M KOH. Region 1: Initial pH: Before any titrant is added to our starting material What is the concentration of H+ at this point in the titration? M What is the pH based on this H+ ion concentration? Region 2: Before the Equivalence Point 10.13 mL of the 0.200 M KOH has been added to the starting material. Complete the BCA table below at...
Two 25.0 ml samples, on 0.100 mol/L HCl and the other 0.100mol/L HF, were titrated with...
Two 25.0 ml samples, on 0.100 mol/L HCl and the other 0.100mol/L HF, were titrated with 0.200 mol/L KOH. a) What is the volume of added base at the equivalence point for each titration? b) Predict whether the pH at the equivalence point for each titration will be acidic, basic or neutral? Explain your selection. c) Predict which titration curve will have the lower initial pH and explain your selection.
a 30.0 ml sample of 0.75 M hypociouous acid, hocl, is titrated with 1.25 M KOH....
a 30.0 ml sample of 0.75 M hypociouous acid, hocl, is titrated with 1.25 M KOH. what is the ph of the solution after 7.0 ml of KOH is added
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka...
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka for HCLO is 3.5 x 10-8. Calculate..... a. the pH when no base has been added b. the pH when 30.0 mL of the base has been added c. the pH at the equivalence point d. the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka...
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka for HCLO is 3.5 x 10-8. Calculate the pH when no base has been added, the pH when 30.0 mL of the base has been added ,. the pH at the equivalence point and the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT