ACID/BASE CHEMISTRY TRIVIA + QUIZZES
Interesting Questions, Facts, and Information
Acids and Bases
Which acid is formed when milk is fermented to form yoghurt? | Acids, Bases and You! |
Aqua regia is a very powerful acid and its name in Latin means 'Royal Water'. Why was it given this name? | Acids, Bases and You! |
This acid is used in almost all car batteries and is also known as 'Oil of Vitriol'. Which acid is it? | Acids, Bases and You! |
A very well known gas is highly basic when dissolved in water but mildly basic in vapour form. It is used for making explosives such as TNT and fertilizers such as Urea. Which gas is it? | Acids, Bases and You! |
The chemical name for Vitamin C is __________ acid? | Acids, Bases and You! |
The 'fizz' in soft drinks is produced by adding which acid? | Acids, Bases and You! |
If you're suffering from acidity in your stomach then you should take antacids. 'Antacids' could contain which two bases? | Acids, Bases and You! |
If a base will dissolve in water, by what name is it better known? | Acids and Bases |
What are the products when silver reacts with dilute sulphuric acid? | Acids and Bases |
Aluminium will react with Hydrochloric acid. What are the products of this reaction? | Acids and Bases |
What are the products, if a reaction occurs between nitric acid and sodium hydroxide? | Acids and Bases |
If I react magnesium with hydrochloric acid, what gas is produced? | Acids and Bases |
What colour would hydrochloric acid (pH 1) turn universal indicator? | Acids and Bases |
Why is universal indicator a better indicator to use than litmus indicator? | Acids and Bases |
What colour is methyl orange in alkali conditions? | Acids and Bases |
What is a buffer solution? | High School Acids & Bases |
What is Kw? | High School Acids & Bases |
What is an equivalence point? | High School Acids & Bases |
What is the range of pH for a acid? | High School Acids & Bases |
What does a strong base do in solution? | High School Acids & Bases |
What is an amphiprotic substance? | High School Acids & Bases |
What is the pH of water at 25 degrees c? | High School Acids & Bases |
What is an Arrhenius Acid? | High School Acids & Bases |
ACID-BASE CHEMISTRY
For thousands of years people have known that vinegar, lemon juice and many other foods taste sour. However, it was not until a few hundred years ago that it was discovered why these things taste sour - because they are all acids. The term acid, in fact, comes from the Latin term acere, which means "sour". While there are many slightly different definitions of acids and bases, in this lesson we will introduce the fundamentals of acid/base chemistry.
In the seventeenth century, the Irish writer and amateur chemist Robert Boylefirst labeled substances as either acid or bases (he called bases alkalies) according to the following characteristics:
Acids taste sour, are corrosive to metals, change litmus (a dye extracted from lichens) red, and become less acidic when mixed with bases.
Bases feel slippery, change litmus blue, and become less basic when mixed with acids.
While Boyle and others tried to explain why acids and basesbehave the way they do, the first reasonable definition of acids and bases would not be proposed until 200 years later.
Acids are substances which produce hydrogen ions in solution.
Bases are substances which produce hydroxide ions in solution.
Neutralisation happens because hydrogen ions and hydroxide ions react to produce water.
Limitations of the theory
Hydrochloric acid is neutralised by both sodium hydroxide solution and ammonia solution. In both cases, you get a colourless solution which you can crystallise to get a white salt - either sodium chloride or ammonium chloride.
These are clearly very similar reactions. The full equations are:
In the sodium hydroxide case, hydrogen ions from the acid are reacting with hydroxide ions from the sodium hydroxide - in line with the Arrhenius theory.
However, in the ammonia case, there don't appear to be any hydroxide ions!
You can get around this by saying that the ammonia reacts with the water it is dissolved in to produce ammonium ions and hydroxide ions:
This is a reversible reaction, and in a typical dilute ammonia solution, about 99% of the ammonia remains as ammonia molecules. Nevertheless, there are hydroxide ions there, and we can squeeze this into the Arrhenius theory.
However, this same reaction also happens between ammonia gas and hydrogen chloride gas.
In this case, there aren't any hydrogen ions or hydroxide ions in solution - because there isn't any solution. The Arrhenius theory wouldn't count this as an acid-base reaction, despite the fact that it is producing the same product as when the two substances were in solution. That's silly!
An acid is a proton (hydrogen ion) donor.
A base is a proton (hydrogen ion) acceptor.
The Relationship Between Arrhenius and Bronsted-Lowry
The Bronsted-Lowry theory doesn't go against the Arrhenius theory in any way - it just adds to it. Hydroxide ions are still bases because they accept hydrogen ions from acids and form water. An acid produces hydrogen ions in solution because it reacts with the water molecules by giving a proton to them. When hydrogen chloride gas dissolves in water to produce hydrochloric acid, the hydrogen chloride molecule gives a proton (a hydrogen ion) to a water molecule. A co-ordinate (dative covalent) bond is formed between one of the lone pairs on the oxygen and the hydrogen from the HCl. Hydroxonium ions, H3O+, are produced. | |
When an acid in solution reacts with a base, what is actually functioning as the acid is the hydroxonium ion. For example, a proton is transferred from a hydroxonium ion to a hydroxide ion to make water. Showing the electrons, but leaving out the inner ones: It is important to realise that whenever you talk about hydrogen ions in solution, H+(aq), what you are actually talking about are hydroxonium ions. |
- Neutralization reaction occurs, when equal quantities of acids and bases occurs. For example: H+ ions react with OH- ions, to make the H2O molecule.
Conjugate acid - base pairs
have chemical formula that differ by one H+ (they differ by both one H atom and by a +1 charge). They typically appear in a chemical equation for an acid-base reaction, where one is a reactant and the other is a product. Stronger acids have weaker conjugate bases, while stronger bases have weaker conjugate acids. The strongest acids have conjugate bases that are so weak as to be non-basic. The strongest bases have conjugate acids that are so weak as to be non-acidic.