Why sio2 does not react with water

Silicon dioxide reacts with sodium hydroxide solution, but only if it is hot and concentrated. This is also an example of the acidic silicon dioxide reacting with a base. Silicon dioxide has a water solubility of 0. Under normal conditions, silicon does not react with most acids but is dissolved by hydrofluoric acid.

Silicon is attacked by bases such as aqueous sodium hydroxide to give silicates. Silicon dioxide acts as a Lux—Flood acid, being able to react with bases under certain conditions. Bicarbonate is naturally produced by the reaction of carbon dioxide CO2 with water.

H2O to produce carbonic acid H2CO3 , which dissociates to a bicarbonate ion and a. Silicon is applied as an aid in steel, chemical and electron industries, where it is processed under high temperatures. Steel and other alloys are eventually processed to for example engine blocks or cylinder heads.

Industrially significant silicon compounds are rubber- or resin-like compounds, which are generally water resistant and also withstand oxidation processes and chemical weathering. These are applied as lubricants under high temperatures, as a sealing kit for windows, roofs and pipes, in rubber hoses and in plastic parts for car engines. Silicon oils are applied in cosmetics, and for textile impregnation. In microchips this element is a semi conductor, as it is in transistors and other electronic parts.

Solar panels consist of n-semi conductors of silicon and arsenic and p-semi conductors of silicon and boron. It occurs in elementary form in optic lenses and prisms for infrared light. Silicon carbide is nearly as hard as diamond and is applied as an abrasive. Quartz crystals that exist naturally and are produced chemically have the characteristic of vibrating in very exact frequencies, when they come in contact with electricity.

This may be applied in watches, radios and televisions. Alkali silicones are added to cleansing agents, glue and bleaching agents for textiles. Zeolites are silicones that are applied as foam regulators in detergents. These directly influence water quality. Other silicon compounds may be applied as absorbents. Silicon dioxide is a dietary requirement for various organisms. The mechanism of intake is currently unclear. Diatoms and sea sponges apply silicon for skeleton strengthening.

Small hairs on nettles also consist of silicon. Chickens and rats require silicon for bone development. It is very likely that silicon is a dietary requirement for humans, as the skin and connective tissue contains significant amounts of this element. Silicon is also essential for plant growth.

Gurtman, J. Kirsch, and C. Hastings, J. Stull and H. Prophets, eds. Cowperthwaite and W. Z, Vol. I , Vols. II-IV Bundy, J. If you really want to be certain, check past papers and mark schemes. I found one question about the reaction between sodium oxide and phosphoric V acid where the mark scheme accepted any of the possible equations - which is what I would expect.

I know I haven't given you that particular set of equations, but they aren't difficult to work out as long as you understand the principle, and I can't possibly give every single acid-base equation. This already long page would go on for ever, and everybody would give up in despair well before the end! That's why you are trying to understand chemistry rather than learn it parrot-fashion.

Please don't waste time learning equations - or at least, not until you know and understand all the rest of the chemistry that you need to know and understand! Any one equation stands a very small chance of coming up in an exam, even if it is on your particular syllabus. Life is too short to waste time learning equations. Know how to work them out if you need to. We are going to be looking at sulphur dioxide, SO 2 , and sulphur trioxide, SO 3. Sulphur dioxide is fairly soluble in water, reacting with it to give a solution known as sulphurous acid, and traditionally given the formula H 2 SO 3.

However, the main species in the solution is simply hydrated sulphur dioxide - SO 2 , xH 2 O. It is debatable whether any H 2 SO 3 as such exists at all in the solution. Sulphurous acid is also a weak acid with a pK a of around 1. A reasonably concentrated solution of sulphurous acid will again have a pH of about 1.

Note: There is some variability in the pK a value quoted for sulphurous acid by various sources - ranging from 1. I have no way of knowing which of these is right. The ionisation of the "sulphurous acid" involves ionisation of the hydrated complex, and you shouldn't need to worry about this at this level. Sulphur dioxide will also react directly with bases such as sodium hydroxide solution. If sulphur dioxide is bubbled through sodium hydroxide solution, sodium sulphite solution is formed first followed by sodium hydrogensulphite solution when the sulphur dioxide is in excess.

Note: Sodium sulphite is also called sodium sulphate IV. Sodium hydrogensulphite is also sodium hydrogensulphate IV or sodium bisulphite. Notice that the equations for these reactions are different from the phosphorus examples. In this case, we are reacting the oxide directly with the sodium hydroxide, because that's the way we are most likely to do it. Another important reaction of sulphur dioxide is with the base calcium oxide to form calcium sulphite calcium sulphate IV.

This is at the heart of one of the methods of removing sulphur dioxide from flue gases in power stations. Sulphur trioxide reacts violently with water to produce a fog of concentrated sulphuric acid droplets. Note: If you know about the Contact Process for the manufacture of sulphuric acid, you will know that the sulphur trioxide is always converted into sulphuric acid by a round-about process to avoid the problem of the sulphuric acid fog.

You will find details of the Contact Process elsewhere on this site if you are interested, but it isn't relevant to the current topic. The acid reacts with water to give a hydroxonium ion a hydrogen ion in solution, if you like and a hydrogensulphate ion.

The second hydrogen is more difficult to remove. In fact the hydrogensulphate ion is a relatively weak acid - similar in strength to the acids we have already discussed on this page. This time you get an equilibrium:.

Sulphuric acid, of course, has all the reactions of a strong acid that you are familiar with from introductory chemistry courses. For example, the normal reaction with sodium hydroxide solution is to form sodium sulphate solution - in which both of the acidic hydrogens react with hydroxide ions.

In principle, you can also get sodium hydrogensulphate solution by using half as much sodium hydroxide and just reacting with one of the two acidic hydrogens in the acid.

In practice, I personally have never ever done it - I can't at the moment see much point! Sulphur trioxide itself will also react directly with bases to form sulphates. For example, it will react with calcium oxide to form calcium sulphate. This is just like the reaction with sulphur dioxide described above.

Chlorine VII oxide is also known as dichlorine heptoxide, and chlorine I oxide as dichlorine monoxide. It continues the trend of the highest oxides of the Period 3 elements towards being stronger acids. The pH of typical solutions will, like sulphuric acid, be around 0. You probably won't need this for the purposes of UK A level or its equivalents , but it is useful if you understand the reason that chloric VII acid is a stronger acid than chloric I acid see below.

You can apply the same reasoning to other acids on this page as well. When the chlorate VII ion perchlorate ion forms by loss of a hydrogen ion when it reacts with water, for example , the charge can be delocalised over every oxygen atom in the ion.

That makes it very stable, and means that chloric VII acid is very strong.