Which carbonates react with acids

Decide if they want to change the category of any of the statements. Plenary Bring all students into a plenary. Report whether they changed their mind during the lesson. Explain why they changed their ideas. Identify aspects that they are still uncertain about. It is the responsibility of the teacher to carry out an appropriate risk assessment for the demonstration. Commentary The initial demonstration enlivens the introduction of the learning objective. Written feedback should help students to see what further work they need to do.

Download all. Additional information This lesson plan was originally part of the Assessment for Learning website, published in Acknowledgement V. Level years. Use Formative assessment. Category Group work Lesson planning Higher-order thinking and metacognition Acids and bases Reactions and synthesis. AQA Combined science: Synergy 4. AQA Combined science: Trilogy 5. Edexcel Chemistry Topic 3 - Chemical changes Acids 3. The video is a bit clumsy but is chemically accurate.

The calcium carbonate precipitate reacts with more carbon dioxide to form calcium hydrogencarbonate, Ca HCO 3 2. Calcium hydrogencarbonate is soluble in water. This is the same reaction which produces cave systems in limestone rocks. Limestone is a form of calcium carbonate. Carbon dioxide dissolved in rain water gradually dissolves the rock over very long periods of time.

You will find compounds like sodium hydrogencarbonate also called "sodium hydrogen carbonate" separate words or the old name "sodium bicarbonate". I prefer the name "sodium hydrogencarbonate" because it shows that the hydrogen and carbonate are both part of the same HCO 3 - ion. There are very few solid hydrogencarbonates - the only ones you are likely to meet are sodium and potassium hydrogencarbonates. Calcium hydrogencarbonate only exists in solution. If you try to turn it into a solid, it splits up again into calcium carbonate and carbon dioxide and water.

So, for example, if you add dilute hydrochloric acid to solid sodium hydrogencarbonate, it will react giving off colourless carbon dioxide gas and producing colourless sodium chloride solution. Note: To be honest, at this level you might come across calcium hydrogencarbonate being formed in the lime water reaction, and you might come across sodium hydrogencarbonate being used to test for an acid.

The salt produced, potassium sulfate, would be a white solid that produces a lilac flame in a flame test. Since we can de-code our word equation to arrive at what Chris actually did and what was observed, we are confident our word equation is correct. If you come across an even older textbook you will find hydrogencarbonates referred to as bicarbonates. The term bicarbonate is still in general useage you probably have a box of sodium bicarbonate in your kitchen pantry!

Use hydrogencarbonate instead. IUPAC gives the name of the element sulfur with an "f" not a "ph" so the acid is sulfuric acid. The name of a salt derived from sulfuric aicd with an "f" is a sulfate also with an "f" , but in older textbooks you will find that the salts derived from sulphuric acid with a "ph" are called sulphates also with a "ph".

Iron can also form covalent compounds. In this case there is no cation, no positive charge, but we can assign an informal charge based on its oxidation state which is then referred to as its oxidation state or oxidation number. When we do this, we use Roman numerals to indicate the oxidation state of the metal. Do you know this? Do you understand this? Can you apply this? Take the exam now!

Chris boiled off all the liquid at Is your answer plausible? It can be detected by passing the gas through limewater, which will go cloudy. Also, the reaction of metal carbonates with acids is exothermic ie heat energy is given out. This type of reaction can be used to test unknown solutions to see if they are acidic. Simply add a solution of sodium carbonate to the solution and if carbon dioxide gas is given off, the solution is acidic.

This type of reaction can also be used to test unknown solutions for the presence of carbonate CO 3 — ions.