Chapter 10: Q6P (page 230)

Calculate the pH of $0.300 M$ piperazine. Calculate the concentration of each form of piperazine in this solution.

Short Answer

Expert verified

The pH is $11.60$ .

The concentration of each form of piperazine in this solution:role="math" localid="1654931700149" $[p i p e a z i n e] = 0.296 M [pipeazine - H^{+}] = 3.99 \times 10^{- 3} M [{BH}_{2}^{2 +}] = 2.15 \times 10^{- 9} M$

Step by step solution

Definition of piperazine.

Piperazine is an organic molecule that is made up of a six-membered ring with two nitrogen atoms in opposing places. Piperazine is a saline-tasting tiny alkaline deliquescent crystal.

The pH of 0.300Mpiperazine and the concentration of each form of piperazine in this solution.

Consider the following reaction

$p i p e a z i n e + H_{2} 0 𝆏 p i p e a z i n e - H^{+} + {OH}^{-}$

First calculate the value of by the following: $(K_{w} = 10^{- 14})$

$K_{b 1} = K_{w} / K_{2} = 5.38 \times 10^{- 5}$

Next calculate the value of $x$ :

$K_{b 1} = \frac{x^{2}}{0.3 - x} 5.38 \times 10^{- 5} = \frac{x^{2}}{0.3 - x} x = 3.99 \times 10^{- 3} M x = [{OH}^{-}] SO Calculate pOH = - \log x = - \log (3.99 \times 10^{- 3}) = 2.40 pH = 14 - pOH = 14 - 2.40 = 11.60$

Then calculate the rest of the concentrations

$[p i p e r z i n e] = 0.3 - x = 0.3 - (3.99 \times 10^{- 3}) = 0.296 M [p i p e r z i n e - H^{+}] = x = 3.99 \times 10^{- 3} M [{BH}_{2}^{2 +}] = [p i p e r z i n e - H^{+}] / K_{1} = 2.15 \times 10^{- 9} M$

Unlock Step-by-Step Solutions & Ace Your Exams!

Full Textbook Solutions
Get detailed explanations and key concepts
Unlimited Al creation
Al flashcards, explanations, exams and more...
Ads-free access
To over 500 millions flashcards
Money-back guarantee
We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Calculate the pH of $0.300 M$ piperazine. Calculate the concentration of each form of piperazine in this solution.

Short Answer

Step by step solution

Definition of piperazine.

The pH of 0.300Mpiperazine and the concentration of each form of piperazine in this solution.

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Kinetics

Ionic and Molecular Compounds

Nuclear Chemistry

Chemical Analysis

Chemistry Branches

Study anywhere. Anytime. Across all devices.

Calculate the pH of 0.300Mpiperazine. Calculate the concentration of each form of piperazine in this solution.

Short Answer

Step by step solution

Definition of piperazine.

The pH of 0.300Mpiperazine and the concentration of each form of piperazine in this solution.

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Kinetics

Ionic and Molecular Compounds

Nuclear Chemistry

Chemical Analysis

Chemistry Branches

Study anywhere. Anytime. Across all devices.

Calculate the pH of $0.300 M$ piperazine. Calculate the concentration of each form of piperazine in this solution.