Question

A 59 mL sample of hydrobromic acid is titrated with 93 mL of a 3.5 M...

A 59 mL sample of hydrobromic acid is titrated with 93 mL of a 3.5 M solution of strontium hydroxide to reach the equivalence point. What is the concentration of hydrobromic acid?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A 59 mL sample of hydrobromic acid is titrated with 93 mL of a 3.5 M solution of strontium hydroxide to reach the equivalence point. What is the concentration of hydrobromic acid?

We write reaction between HBr and Sr(OH)

Sr(OH)2 + 2 HBr --- > SrBr2 + 2 H2O

Mole ratio between HBr : Sr(OH)2 is 2 : 1

Calculation of moles of strontium hydroxide

Mol strontium hydroxide = Volume in L x molarity

=0.093 L x 3.5 M = 0.3255 mol Sr(OH)2

Mol HBr = 0.3255 mol Sr(OH)2 x 2 mol HBr / 1 mol Sr(OH)2 = 0.651 mol

[HBr]=mol / volume in L

= 0.651 mol / 0.059 L = 11.0 M

Molarity of HBr = 11.0 M

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 solid sample of zinc hydroxide is added to 0.340 L of 0.400 M hydrobromic acid....
A solid sample of zinc hydroxide is added to 0.340 L of 0.400 M hydrobromic acid. The solution that remains is still acidic. It is then titrated with 0.400 M sodium hydroxide solution, and it takes 90.5 mL of the sodium hydroxide solution to reach the equivalence point. What mass of zinc hydroxide was added to the hydrobromic acid solution?
A 21.8 mL sample of 0.223 M trimethylamine, (CH3)3N, is titrated with 0.207 M hydrobromic acid....
A 21.8 mL sample of 0.223 M trimethylamine, (CH3)3N, is titrated with 0.207 M hydrobromic acid. At the equivalence point, the pH is
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH...
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. Calculate the concentration of acetic acid in the 25.0 mL sample. Calculate the pH at the equivalence point (Ka acetic acid = 1.75x10^-5)
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. When a 19.6 mL sample of a 0.498 M aqueous acetic acid solution is titrated...
1. When a 19.6 mL sample of a 0.498 M aqueous acetic acid solution is titrated with a 0.343 M aqueous potassium hydroxide solution, what is the pH after 42.7 mL of potassium hydroxide have been added? pH= 2.What is the pH at the equivalence point in the titration of a 22.2 mL sample of a 0.413 M aqueous acetic acid solution with a 0.500 M aqueous potassium hydroxide solution? pH=
When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what...
When 25 mL of 0.12 M aqueous ammonia is titrated with 0.12 M hydrobromic acid, what is the pH at the equivalence point? For ammonia, NH3, Kb = 1.8 x 10-5.
A 21.0 mL sample of 0.291 M ammonia, NH3, is titrated with 0.210 M hydrobromic acid....
A 21.0 mL sample of 0.291 M ammonia, NH3, is titrated with 0.210 M hydrobromic acid. The pH before the addition of any hydrobromic acid is
A 22.2 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.277 M hydrobromic acid....
A 22.2 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.277 M hydrobromic acid. After adding 10.9 mL of hydrobromic acid, the pH is ______
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated...
In titrating an acid of unknown concentration, a 20.00 mL sample of the acid was titrated using standardized sodium hydroxide. The NaOH had a concentration of 0.1105 M. The titration required 35.45 mL of the base to reach the end-point in the titration. a) How many moles of H+ was in the 20.00 mL sample of acid? b) The solution of acid was prepared by adding 9.605 grams of the acid to 1.000 liter of water. What was the molecular...
A 28.5 mL sample of 0.253 M diethylamine, (C2H5)2NH, is titrated with 0.247 M hydrobromic acid....
A 28.5 mL sample of 0.253 M diethylamine, (C2H5)2NH, is titrated with 0.247 M hydrobromic acid. After adding 13.0 mL of hydrobromic acid, the pH is_____
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT