Chemistry - Acids and Bases Flashcards
When an acid reacts with a metal, it produces a salt and hydrogen gas (H₂). This is typically seen with reactive metals like magnesium or zinc. An acid and a base react to form a salt and water in a process called neutralization. This reaction helps balance pH levels and is common in chemistry and everyday life (e.g., indigestion remedies).
what is produced when an acid reacts with metal
Key Terms
what is produced when an acid reacts with metal
Salt + H2
what is produced when an acid reacts with a base
Salt and water
what is produced when an acid reacts with a carbonate
salt + water + CO2
What is the general word equation for a metal reacting with an acid
metal + acid= salt + hydrogen
What does the speed of a rection depend on?
How high up in the reactivity series it is
What is the Lab test for Hydrogen
A burning wooden splint goes pop if it is put into a test tube of hydrogen.
The flame ignites the hydrogen, which burns explosively to make a lo...
Related Flashcard Decks
| Term | Definition |
|---|---|
what is produced when an acid reacts with metal | Salt + H2 |
what is produced when an acid reacts with a base | Salt and water |
what is produced when an acid reacts with a carbonate | salt + water + CO2 |
What is the general word equation for a metal reacting with an acid | metal + acid= salt + hydrogen |
What does the speed of a rection depend on? | How high up in the reactivity series it is |
What is the Lab test for Hydrogen | A burning wooden splint goes pop if it is put into a test tube of hydrogen. |
What is the Arrhenius definition of an acid | An acid is a substance that dissociates in water to produce H+ ions |
What is the Arrhenius definition of a monobasic acid and give an example | Each molecule dissociates in solution to produce one H+ ion |
What is the Arrhenius definition of a dibasic acid and give an example | Each molecule dissociates in solution to produce two H+ ions |
What is the Arrhenius definition of a tribasic acid, and give an example | Each molecule dissociates in solution to produce three H+ ions |
What does the H+ ion react with water to form | Hydronium ion |
What is the general formula for the dissociation of acids in water | H(acid) +H2O = H3O+(Acid)- |
What is a Arrhenius Base | A base is a substance that dissociates in water to produce OH- ions |
What is the Arrhenius definition of a monobasic base and give an example | Each molecule dissociates to produce one OH- ion in solution |
What is the Arrhenius definition of a dibasic base and give an example | Each molecule dissociates to produce two OH- ion in solution |
What is the Arrhenius definition of a tribasic base and give an example | Each molecule dissociates to produce three OH- ion in solution |
What is a Arrhenius strong acid | A strong acid dissociates fully in aqueous solution to produce H+ ions |
What is a Arrhenius strong base | Dissociates fully in aqueous solution to produce OH- ions |
What is a Arrhenius weak acid | A weak acid dissociates only slightly in aqueous solution to produce H+ ions |
What is a Arrhenius weak base |
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Limitations of Arrhenius theory | Limited to diluted aqueous solutions |
What is the Brønsted-Lowry definition of an acid | An acid is a proton donor |
What is the Brønsted-Lowry definition of a base | A base is a proton acceptor |
What is the Brønsted-Lowry definition of a stronger acid | A good proton donor |
What is the Brønsted-Lowry definition of a weaker acid | Poor proton donor |
What is the Brønsted-Lowry definition of a stronger base | A good proton acceptor |
What is the Brønsted-Lowry definition of a weaker base | A poor proton acceptor |
What does Amphoteric discribe, name an example | A substance which can act as either an acid or a base. Eg water |
Advantages of the Brønsted-Lowry Theory over Arrhenius theory | Not limited to aqueous solutions. Explains how substances can be amphoteric. Defines a larger range of substances as acids or bases. Takes into account the existence of hydronium ions |
Name examples of a strong acid | HCl, sulfuric acid (H2SO4) |
Name examples of a strong Base | sodium hydroxide ( NaOH) |
Name examples of a weak acid | ethanoic acid ( CH3COOH) |
Name examples of a weak base | Sodium Carbonate (Na2CO3) |
What is a conjugate (acid/base) pair | A conjugate (acid/base) pair is two substances that differ from each other by a H+ (a single proton) |
The stonger an acid the —— its conjugate base | Weaker |
The stonger an base the —— its conjugate acid | Weaker |
What is a conjugate acid | the substance formed when a base accepts a proton |
if asked to give the conjugate acid, you are given the… | Base. Make it accept a proton to get the conjugate acid |
What is a conjugate base | substance formed when an acid donates a proton |
if asked to give the conjugate base, you are given the… | Acid. Remove a proton from it to get the conjugate base |
Neutralisation | The reaction between an acid and a base to form salt and water |
What is a salt | A substance formed when the hydrogen ion from an acid is replaced by a metal or ammonium ion |
Use of neutralisation reactions in Medcine | Relief from excess HCL can be obtained by taking an antacid ( alkali tablets) |
Use of neutralisation reactions in Agriculture | Lime (CaO) is spread on fields to neutralises the acid in the soil increasing crop yield |
Use of neutralisation reactions in Envirmental protection | Lime is added to lakes in places which suffer from acid rainfall to neutralise the acid in lakes |
Use of neutralisation reactions in miscellaneous | Toothpaste is slightly basic to neutralise the plaque (acidic) in your mouth vinegar is an acid that neutralises the alkali sting of wasps |
What does it mean to dissociate | A molecule breaks down into its individual +and - ions |
What is an alkali | A base that dissolves in water |
What is the conjugate base of OH-? | O 2- |