Question

A 36.6 mL sample of 0.2868 M hydrotelluric acid, H2Te, is titrated with 0.2868 M sodium...


A 36.6 mL sample of 0.2868 M hydrotelluric acid, H2Te, is titrated with 0.2868 M sodium hydroxide.

What is the pH after 18.3 mL, 36.6 mL, 54.9 mL and 73.2 mL of NaOH have been added?

step mL NaOH added

pH
1

18.3
2

36.6
3

54.9
4

73.2


The first and second ionization constants for H2Te are 2.3×10-3 and 1.6×10-11

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Question: A 36.6 mL sample of 0.2868 M hydrotelluric acid, H2Te, is titrated with 0.2868 M sodium hydroxide.

What is the pH after 18.3 mL, 36.6 mL, 54.9 mL and 73.2 mL of NaOH have been added?

Ans: (i) When 18.3ml of NaOH added to 36.6ml hydrotelluric acid pH is 2.63

        (ii) When 36.6ml of NaOH added to 36.6ml hydrotelluric acid pH is 7.897

        (iii) When 54.9ml of NaOH added to 36.6ml hydrotelluric acid pH is 12.76

        (iv) When 73.2ml of NaOH added to 36.6ml hydrotelluric acid pH is 12.98

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 44.6 mL sample of 0.3060 M selenious acid, H2SeO3, is titrated with 0.3060 M sodium...
A 44.6 mL sample of 0.3060 M selenious acid, H2SeO3, is titrated with 0.3060 M sodium hydroxide. What is the pH after 22.3 mL, 44.6 mL, 66.9 mL and 89.2 mL of NaOH have been added? step mL NaOH added pH 1 22.3 2 44.6 3 66.9 4 89.2 The first and second ionization constants for H2SeO3 are 2.4×10-3 and 4.8×10-9
A 32.44 mL sample of 0.202M acetic acid is titrated with 0.185 M sodium hydroxide. Calculate...
A 32.44 mL sample of 0.202M acetic acid is titrated with 0.185 M sodium hydroxide. Calculate the pH of the solution 1. before any NaOH is added 2. after 24.00 mL of NaOH is added 3. at the equivalence point
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 a 26.7 mL sample of a 0.477 M aqueous hypochlorous acid solution is titrated with...
When a 26.7 mL sample of a 0.477 M aqueous hypochlorous acid solution is titrated with a 0.300 M aqueous sodium hydroxide solution, what is the pH after 63.7 mL of sodium hydroxide have been added? pH =
A 21.1 mL sample of a 0.485 M aqueous hypochlorous acid solution is titrated with a...
A 21.1 mL sample of a 0.485 M aqueous hypochlorous acid solution is titrated with a 0.347 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? 12- A 24.0 mL sample of 0.323 M ethylamine, C2H5NH2, is titrated with 0.284 M nitric acid. At the titration midpoint, the pH is :________________.
22.0 mL of 0.122 M diprotic acid (H2A) was titrated with 0.1020 M KOH. The acid...
22.0 mL of 0.122 M diprotic acid (H2A) was titrated with 0.1020 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5and Ka2=3.4×10−10. Find: At what added volume of base does the first equivalence point occur? Find:At what added volume of base does the second equivalence point occur? Find: What is the pH at the first midway point? Find: What is the pH at the second midway point? Find: What is the pH at the first equivalence point?
1) A 16.8 mL sample of a 0.489 M aqueous acetic acid solution is titrated with...
1) A 16.8 mL sample of a 0.489 M aqueous acetic acid solution is titrated with a 0.376 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? pH - ___ 2) What is the pH at the equivalence point in the titration of of a 29.5 mL sample of a 0.460 M aqueous hydroflouric acid solution with a 0.358 M aqueous sodium hydroxide solution? pH - ___
1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....
1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH before the titration begins. 2. A 1.0-L buffer solution contains 0.100 mol HCN and 0.100 mol LiCN. The value of Ka for HCN is 4.9 x 10-10. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa = -log (4.9 x 10-10) = 9.31. Calculate the new pH after the addition...
75.0 ml sample of 0.200 M sodium hydroxide is titrated with .200 M nitric acid. calculate...
75.0 ml sample of 0.200 M sodium hydroxide is titrated with .200 M nitric acid. calculate ph A) after adding 40.00 mL of HNO3 B) at the equivalent point
22.0 mL of 0.128 M diprotic acid (H2A) was titrated with 0.1017 M KOH. The acid...
22.0 mL of 0.128 M diprotic acid (H2A) was titrated with 0.1017 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5and Ka2=3.4×10−10. Part A At what added volume of base does the first equivalence point occur? Part B At what added volume of base does the second equivalence point occur?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT