1.) A 25.3 mL sample of 0.329 M triethylamine, (C2H5)3N, is titrated with 0.344 M nitric...

1.) A 25.3 mL sample of 0.329 M triethylamine, (C₂H₅)₃N, is titrated with 0.344 M nitric acid.

The pH before the addition of any nitric acid =

2.) A 20.8 mL sample of 0.275 M triethylamine, (C₂H₅)₃N, is titrated with 0.304 M hydrochloric acid.

At the equivalence point, the pH =

Expert Solution

queen_honey_blossom answered 2 years ago

A 20.8 mL sample of 0.304 M triethylamine, (C2H5)3N, is titrated with 0.341 M hydroiodic acid....

A 20.8 mL sample of 0.304 M triethylamine, (C2H5)3N, is titrated with 0.341 M hydroiodic acid. (1) Before the addition of any hydroiodic acid, the pH is (2) After adding 7.53 mL of hydroiodic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 26.5 mL of hydroiodic acid, the pH is Please show step by step instructions, many thanks!

A 26.9 mL sample of 0.373 M triethylamine, (C2H5)3N, is titrated with 0.310 M hydroiodic acid....

A 26.9 mL sample of 0.373 M triethylamine, (C2H5)3N, is titrated with 0.310 M hydroiodic acid. The pH before the addition of any hydroiodic acid is . Use the Tables link in the References for any equilibrium constants that are required. A 20.6 mL sample of 0.337 M ammonia, NH3, is titrated with 0.229 M hydrochloric acid. At the equivalence point, the pH is .

Determine the pH during the titration of 34.9 mL of 0.331 M triethylamine ((C2H5)3N , Kb...

Determine the pH during the titration of 34.9 mL of 0.331 M triethylamine ((C2H5)3N , Kb = 5.2×10-4) by 0.331 M HNO3 at the following points. (a) Before the addition of any HNO3. _________ (b) After the addition of 13.6 mL of HNO3 _____ (c) At the titration midpoint ______ (d) At the equivalence point _______ (e) After adding 52.0 mL of HNO3 ________

Determine the pH during the titration of 33.7 mL of 0.345 M triethylamine ((C2H5)3N, Kb =...

Determine the pH during the titration of 33.7 mL of 0.345 M triethylamine ((C2H5)3N, Kb = 5.2×10-4) by 0.345 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI (b) After the addition of 15.0 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 51.9 mL of HI

Calculate the pH of a 0.0290 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb...

Calculate the pH of a 0.0290 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb = 5.20×10-4). pH = ?

A 3.452 M solution of triethylamine ((C2H5)3N, Kb= 4e-4) has a pH of 12.57. What is...

A 3.452 M solution of triethylamine ((C2H5)3N, Kb= 4e-4) has a pH of 12.57. What is the percent ionization of this solution?

1) A 28.6 mL sample of 0.226 M methylamine, CH3NH2, is titrated with 0.221 M nitric...

1) A 28.6 mL sample of 0.226 M methylamine, CH3NH2, is titrated with 0.221 M nitric acid. After adding 11.5 mL of nitric acid, the pH is 2) A 24.0 mL sample of 0.372 M methylamine, CH3NH2, is titrated with 0.381 M hydrochloric acid. After adding 35.9 mL of hydrochloric acid, the pH is

1). A 27.1 mL sample of 0.342 M trimethylamine, (CH3)3N, is titrated with 0.336 M hydrochloric...

1). A 27.1 mL sample of 0.342 M trimethylamine, (CH3)3N, is titrated with 0.336 M hydrochloric acid. The pH before the addition of any hydrochloric acid is _____ 2). A 20.8 mL sample of 0.305 M dimethylamine, (CH3)2NH, is titrated with 0.255 M hydroiodic acid. At the equivalence point, the pH is ______ 3). A 26.2 mL sample of 0.251 M diethylamine, (C2H5)2NH, is titrated with 0.215 M hydrobromic acid. After adding 42.8 mL of hydrobromic acid, the pH is...

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 after 400.0 mL of acid has been added. 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...

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 after 600.0 mL of the acid has been added. 2) A 100.0-mL sample of 0.100 M HCHO2 is titrated with 0.200 M NaOH. Calculate the pH after adding 30.00 mL of the base.

Question