Showing posts with label lowry. Show all posts
Showing posts with label lowry. Show all posts

Saturday, October 3, 2020

Brønsted-Lowry Theory of Acids and Bases

 Ammonia, NH3, is a base right?

Well, yes it is sometimes... but it can also be an acid.

Welcome to the wonderful world of Brønsted-Lowry acids and bases.

At AUS-e-TUTE, we've just added a new tutorial, game, tests and exam to help you understand Brønsted-Lowry acids, bases and their conjugates.

If you are not an AUS-e-TUTE Member you can view a tutorial on this subject for free at https://www.ausetute.com.au/bronstedlowry.html

Thursday, September 17, 2015

AlP Rat Poison

Dozens of mysterious sealed silver canisters containing aluminium phosphide have washed up on Australian beaches between 2012 and 2015. The Australian Maritime Safety Authority (AMSA) suspects all the canisters have come from the same ship which dumped or lost its cargo in the Pacific Ocean. Aluminium phosphide is used as a fumigant to poison rats on ships.

When solid aluminium phosphide, AlP, is exposed to water, it releases highly toxic phosphine gas, PH3, which smells like rotting fish. The chemical reaction can be represented by the balanced chemical equation shown below:
AlP(s) + 3H2O(l) → PH3(g) + Al(OH)3(aq)

This is a proton-transfer reaction in which water is acting as Brønsted-Lowry acid by donating a proton to phosphorus. Phosphorus is therefore acting as a Brønsted-Lowry base by accepting a proton from water. Aluminium phosphide will react with acids according to the following chemical
AlP(s) + 3H+(aq) → PH3(g) + Al3+(aq)

These reactions make aluminium phosphide a good choice for ridding a ship of rats.
Firstly, as a solid, AlP can easily be stored as pellets in air-tight, water-tight, containers until it is ready to be used. When required, the pellets can be scattered in the effected area . In the humid air aboard ship, the AlP will start reacting to produce toxic phosphine gas, that is, the area will be fumigated. But it is also possible to entice rats to eat AlP pellets mixed with food, in which case it will act as pesticide, because on entering the acidic stomach of the rat, it will produce the toxic phosphine.

Aluminium phosphide is  a very effective way to get ride of rats, so much so, that is widely used in agriculture to remove rats from grain silos.

References:
"Toxic canisters washing up on Australian beaches pose serious health risk"
 http://www.smh.com.au/environment/toxic-canisters-washing-up-on-australian-beaches-pose-serious-health-risk-20150917-gjp5se.html

"Controlling rabbits with aluminium phosphide tablets"
 http://agriculture.vic.gov.au/agriculture/farm-management/chemical-use/publications/chemical-industry-news/chemical-industry-news-no.-75-summer-autumn-2013

"Phosphine fumigation"
https://www.worksafe.qld.gov.au/injury-prevention-safety/hazardous-chemicals/specific-hazardous-chemicals/phosphine-fumigation

Further Reading
Definition of Acids and Bases
Proton-transfer Reactions
Mass-mole Calculations
Molar Volume of Gases

Suggested Study Questions:

  1. The symbols of some elements are listed below. Name each element.
    • Al
    • P
    • H
    • O
    • K
    • He
    • At
  2. Calculate the amount of aluminium phosphide in moles given the masses of AlP given below:
    • 10 g
    • 10 kg
    • 10 mg
    • 10 μg
  3. Calculate the moles of phosphine gas produced when each mass of AlP below reacts with excess water in a ship's hull:
    • 10 g
    • 10 kg
    • 10 mg
    • 10 μg
  4. Based on your answers to question 3 above, calculate the mass of phosphine produced for each mass of AlP used.
  5. Your ship is sailing towards eastern Australia and has just crossed the Tropic of Capricorn. You have been asked to estimate the volume of phosphine gas that will be produced when you release AlP pellets into the ships hold. Which molar gas volume will you use; 22.71 L or 24.79 L ? Explain your answer.
  6. Rats are currently infesting a small part of your ship, about 150 m3. How much solid AlP would be required to fumigate this area, but not leave any AlP residue left over?
  7. The Cook has already tried to fumigate the pantry and is sure there is a silver canister around that still contains some AlP, it could be in the pile of empty canisters, or, it could be in the pile of full canisters. No-one wants to kill themselves by opening the canisters to find out, so can you suggest a method that could be used on board ship to determine how much AlP is present in each canister.
  8. Explain why the reaction between aluminium phosphide and water is described as a proton-transfer reaction and not as a redox reaction.
  9. Explain why, even though aluminium phosphide and phosphine are toxic, it is considered safe to use these to fumigate silos containing grain which will be eaten by humans.
  10. The silver canisters that have washed up on Australian beaches have no labels, presumably these have come off while they were in the ocean. You have been asked to design new labels for the canisters. The labels must include suitable safety and handling information.

Sunday, May 6, 2012

Bath Bombs

Fizzy bath bombs, the scented balls you place in your bath, are an example of a chemical reaction between an acid and a carbonate.
Below is a simple recipe for making your own bath bombs.

EquipmentProcedure
mixing bowl
jar
waxed paper
2 tablespoons citric acid
1/4 cup sodium bicarbonate
1/4 teaspoon fragrant oil (eg lavender oil)
3 tablespoons vegetable oil (eg olive oil)
1. Mix sodium bicarbonate and citric acid together in the mixing bowl.
2. Mix fragrant oil and vegetable oil together in the jar.
3. Slowly add contents of jar to mixing bowl while stirring.
4. Form small balls of mixture and place on waxed paper.
5. Allow balls to dry for 1 or 2 days before storing.
6. Add a ball to your bath water and enjoy!

When you drop your bath bomb into water, the process of dissolving the bath bomb allows the sodium bicarbonate and citric acid to react to produce soluble sodium citrate, water and carbon dioxide gas. The bubbles of carbon dioxide given off during the reaction is why the bath bomb fizzes in the water.

The vegetable oil is not soluble in water, so as the sodium bicarbonate and citric acid react, vegetable oil is released into the water forming a thin layer on your skin which can help "moisturize" it. At the same time, the fragrant oil, which is also insoluble in water, is released, so you can smell the scent.

Further Reading
Definitions and Properties of Acids and Bases
Reaction Calculations: Mass and Moles
Limiting Reagents and Reactants in Excess

Suggested Study Questions
  1. Sodium bicarbonate is also known as sodium hydrogen carbonate, baking soda, bread soda and cooking soda. Write the chemical formula for sodium bicarbonate.
  2. Write a word equation for the reaction between citric acid and sodium bicarbonate.
  3. A balanced chemical equation for the reaction between citric acid and sodium bicarbonate is :
    C5H7O5COOH + NaHCO3 → C5H7O5COO-Na+ + H2O + CO2
    Name each of the following compounds:
    • NaHCO3
    • C5H7O5COOH
    • C5H7O5COO-Na+
    • CO2
    • H2O

  4. Write a chemical equation to show citric acid acting as a Bronsted-Lowry acid.
  5. Sodium bicarbonate is amphiprotic.Write a chemical equation to show sodium bicarbonate
    • accepting a proton
    • donating a proton.
  6. In the reaction between citric acid and sodium bicarbonate, is sodium bicarbonate acting as an acid or a base? Explain your answer. 
  7. For the bicarbonate ion, give the formula for its
    • conjugate base
    • conjugate acid 
  8. The density of citric acid is about 1.5 g/mL. If a tablespoon has a volume of 15 mL, what mass of citric acid was used in preparing the bath bomb? 
  9. Sodium bicarbonate has a density of about 2.2 g/mL and there are 16 tablespoons in 1 cup. What mass of sodium bicarbonate was used to make the bath bomb?
  10. For the reaction between citric acid and sodium bicarbonate given the quantities used in the procedure provided above, which reactant is
    • the limiting reagent
    • the reactant in excess
  11. Calculate the mass of carbon dioxide you would expect to be released during the reaction between citric acid and sodium bicarbonate as described in the above procedure. 
  12. Assuming a temperature of 25oC and a pressure of 100 kPa, what volume of carbon dioxide gas would be released using the data above? 
  13. If the amount of sodium bicarbonate used to make the bath bombs as described above were doubled, what effect would that have on the amount of carbon dioxide produced when the bombs were placed in water?
  14. Write an aim for the experiment described above.