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Bisulfate

is HSO4- anion, which is weakly acidic in nature (capable of protolysis,

proton donation) while the

acetate anion (CH3COO-) is basic only.

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What is the colour of pH paper of CH3COONa?

The color of pH paper when testing a solution of sodium acetate (CH3COONa) typically ranges from green to blue, indicating a pH above 7, as sodium acetate is a salt formed from a weak acid (acetic acid) and a strong base (sodium hydroxide). This means that in aqueous solution, it tends to be slightly basic. The exact color may vary depending on the concentration of the solution and the specific pH paper used.


Would the pH of a sodium hydroxide solution be above or below 7?

NaOH is a base so it will produce a pH above 7.


What will happen is a single crystal is introduced into a super-saturated solution?

We often find that there is a limit to the quantity of solute which will dissolve in a given quantity of solvent. This is especially true when solids dissolve in liquids. For example, if 36 g KCl crystals is shaken with 100 g H2O at 25°C only 35.5 g of the solid dissolves. If we raise the temperature somewhat, all the KCl will dissolve, but on cooling to 25°C again, the extra 0.5 g KC1 will precipitate, leaving exactly 35.5 g of the salt dissolved. We describe this phenomenon by saying that at 25°C the solubility of KCl in H2O is 35.5 g KC1 per 100 g H2O. A solution of this composition is also described as a saturated solution since it can accommodate no more KCl. Under some circumstances it is possible to prepare a solution which behaves anomalously and contains more solute than a saturated solution. Such a solution is said to be supersaturated. A good example of supersaturation is provided by Na2S2O3, sodium thiosulfate, whose solubility at 25°C is 50 g Na2S2O3 per 100 g H2O. If 70 g Na2S2O3 crystals is dissolved in 100 g hot H2O and the solution cooled to room temperature, the extra 20 g Na2S2O3 usually does not precipitate. The resulting solution is supersaturated; consequently it is also unstable. It can be "seeded" by adding a crystal of Na2S2O3, whereupon the excess salt suddenly crystallizes and heat is given off. After the crystals have settled and the temperature has returned to 25°C, the solution above the crystals is a saturated solution-it contains 50 g Na2S2O3. Another example of crystallizing salt out of a supersaturated solution can be seen in the following video. In this case, a supersaturated solution of sodium acetate is poured over a crystals of sodium acetate. These crystals provide the lattice structure "seed" which causes the sodium acetate ions in solution to crystallize out. The video begins with a few crystals of sodium acetate placed on the lab bench. A supersaturated solution of sodium acetate is poured over the crystals providing a seed or crystallization. The salt begins to crystallize, forming a large sodium acetate structure from the precipitation of the ions out of solution. When the sodium acetate crystallizes, the oppositely charged ions are brought closer together by the crystal structure. Since formation of a crystal lattice lowers potential energy by placing like charges close together, the system releases the excess energy in the crystallization process. Thus, the structure ends up being warm to the touch from this excess energy.


Is magnesium sulphate melting point above 50 degrees Celsius?

Yes: FAR above.


Why do you prepare lassaigne extract?

lassaigne extractA small piece of sodium is heated gently in an ignition tube till the sodium melts. About 50 to 60 mg of the organic compound is added to this and the tube heated strongly for 2-3 minutes to fuse the material inside it. After cooling, the tube is carefully broken in a china dish containing about 20 to 30 mL of distilled water. The fused material along with the pieces of ignition tube is crushed with the help of a glass rod and the contents of the china dish are boiled for a few minutes. The sodium salts formed in the above reactions (i.e. NaCN, Na2S, NaX or NaSCN) dissolve. Excess of sodium reacts with water to give sodium hydroxide. This alkaline solution is called Lassaigne's extract or sodium extract. The solution is then filtered to remove the insoluble materials and the filtrate is used for making the tests for nitrogen, sulphur and halogens.ReactionsAn organic compound containing C, H, N, S and halogens when fused with sodium metal gives the following reactions.(NaSCN) is formed during fusion, which in the presence of excess sodium forms sodium cyanide and sodium sulphide.Detection of nitrogenA small quantity of the sodium extract is taken in a test tube. It is made alkaline by adding 2-3 drops of sodium hydroxide (NaOH) solution. 1 mL of freshly prepared solution of ferrous sulphate is added to this solution. The mixture of the two solutions is boiled and then acidified with dilute sulphuric acid. The appearance of prussian blue or green colouration of the precipitate confirms the presence of nitrogen in the given organic compound. The carbon and nitrogen present in the organic compound on fusion with sodium metal give sodium cyanide (NaCN) soluble in water. So, the sodium extract contains sodium cyanide which, on reaction with ferrous sulphate, gives sodium ferrocyanide. Some of the ferrous salt is oxidised to the ferric salt on heating and this reacts with sodium ferrocyanide to form ferric ferrocyanide.Note: When nitrogen and sulphur both are present in any organic compound, sodium thiocyanate is formed during fusion. When extracted with water sodium thiocyanate goes into the sodium extract and gives 'blood red coloration' with ferric ions due to the formation of ferric thiocyanate.Detection of sulphurThe presence of sulphur in any organic compound is detected by using sodium extract as follows:Lead acetate testA small portion of sodium extract is acidified with acetic acid and lead acetate solution is added to it. A black precipitate of lead sulphide indicates the presence of sulphur.Sodium nitroprusside testTo a small quantity of sodium extract taken in a test tube, 2 to 3 drops of sodium nitroprusside are added to the solution. A violet color indicates the presence of sulphur. This color fades away slowly on standing.by: zoren roicres apostol. copy and pastesource:http://www.tutorvista.com.

Related Questions

What is the colour of pH paper of CH3COONa?

The color of pH paper when testing a solution of sodium acetate (CH3COONa) typically ranges from green to blue, indicating a pH above 7, as sodium acetate is a salt formed from a weak acid (acetic acid) and a strong base (sodium hydroxide). This means that in aqueous solution, it tends to be slightly basic. The exact color may vary depending on the concentration of the solution and the specific pH paper used.


What is the pH level of sodium acetate and distilled water?

Sodium acetate is a basic salt, so when dissolved in water it will slightly increase the pH above 7. Distilled water has a neutral pH of 7.


Mixing acetone and sodium hydroxide?

oxidation-reductionWhat type of a reaction occurs when a sodium hydroxide solution is mixed with an acetic acid solution?The answer above is wrong. The correct answer is acid-base neutralization


Would the pH of a sodium hydroxide solution be above or below 7?

NaOH is a base so it will produce a pH above 7.


What is meant by Sodium acetate is a basic salt?

Sodium acetate is called a basic salt because a solution of it in initially pure water has a pH value well above the neutral value of 7. This occurs because acetate ions when dissolved in water must come to an equilibrium in the ionic reaction C2H3O2-1 + H2O <-> C2H4O2 + OH-1 and sodium ions when dissolved in water must come to an equilibrium in the ionic reaction Na+1 + H2O <-> NaOH + H+1. Additionally, water itself must maintain an equilibrium in the ionic reaction H2O <-> H+1 + OH-1. The values of these three equilibrium constants are such that the net result is a higher concentration of hydroxide ions than of hydrogen ions in a solution of sodium acetate. These relative concentrations of hydroxide and hydrogen ions is the defining characteristic of a basic (or alkaline) aqueous solution: Such a relative concentration of hydroxide and of hydrogen ions, although not all the other characteristics of a sodium acetate solution, could be achieved by dissolving an appropriate amount of the base sodium hydroxide in initially pure water.


What is the reaction for Sodium acetate plus H2O?

The reaction between sodium acetate and water is a dissolution process where sodium acetate dissociates into its ions (sodium and acetate) when placed in water. The equation for this process is: CH3COONa + H2O → CH3COO- + Na+ + H2O


How can you test a solution for the barium ions?

Acidify the given solution with a few drops of concentrated HNO3 followed by the addition of 4 mol dm-3 sulphuric acid or ammonium sulphate. A white precipitate implies that there are Barium (II) ions present in the solution. The objective of the test give above is to recognize the Barium(II) ions as the white precipitate of barium sulphate which is not soluble in most of the solvents. Adding a sulphate solution at first might cause distractions as other cations such as strontium also make white precipitates with sulphate ions. Those other precipitates dissolve in dilute nitric acid.


How do you activate hot ice?

Normal H2O(water) ice can't be hot. If the temperature get's above 0 C it will become liquid. Only under extremely high pressure ice will remain in it's solid state at higher temperature. But you can make hot ice by dissolving a special powder called sodiumacetate(can be bought easilly and cheap online) in water. And then touch it with your finger. But then its not 'real' ice, the official name is sodium acetate trihydrate. If you go to YouTube and search for 'sodium acetate', you'll get the coolest videos.


What will happen is a single crystal is introduced into a super-saturated solution?

We often find that there is a limit to the quantity of solute which will dissolve in a given quantity of solvent. This is especially true when solids dissolve in liquids. For example, if 36 g KCl crystals is shaken with 100 g H2O at 25°C only 35.5 g of the solid dissolves. If we raise the temperature somewhat, all the KCl will dissolve, but on cooling to 25°C again, the extra 0.5 g KC1 will precipitate, leaving exactly 35.5 g of the salt dissolved. We describe this phenomenon by saying that at 25°C the solubility of KCl in H2O is 35.5 g KC1 per 100 g H2O. A solution of this composition is also described as a saturated solution since it can accommodate no more KCl. Under some circumstances it is possible to prepare a solution which behaves anomalously and contains more solute than a saturated solution. Such a solution is said to be supersaturated. A good example of supersaturation is provided by Na2S2O3, sodium thiosulfate, whose solubility at 25°C is 50 g Na2S2O3 per 100 g H2O. If 70 g Na2S2O3 crystals is dissolved in 100 g hot H2O and the solution cooled to room temperature, the extra 20 g Na2S2O3 usually does not precipitate. The resulting solution is supersaturated; consequently it is also unstable. It can be "seeded" by adding a crystal of Na2S2O3, whereupon the excess salt suddenly crystallizes and heat is given off. After the crystals have settled and the temperature has returned to 25°C, the solution above the crystals is a saturated solution-it contains 50 g Na2S2O3. Another example of crystallizing salt out of a supersaturated solution can be seen in the following video. In this case, a supersaturated solution of sodium acetate is poured over a crystals of sodium acetate. These crystals provide the lattice structure "seed" which causes the sodium acetate ions in solution to crystallize out. The video begins with a few crystals of sodium acetate placed on the lab bench. A supersaturated solution of sodium acetate is poured over the crystals providing a seed or crystallization. The salt begins to crystallize, forming a large sodium acetate structure from the precipitation of the ions out of solution. When the sodium acetate crystallizes, the oppositely charged ions are brought closer together by the crystal structure. Since formation of a crystal lattice lowers potential energy by placing like charges close together, the system releases the excess energy in the crystallization process. Thus, the structure ends up being warm to the touch from this excess energy.


What is a solution that contains more hydroxide than hydrogen?

A solution with more hydroxide ions than hydrogen ions is basic in nature. It has a pH above 7, indicating it is alkaline. Examples include solutions of sodium hydroxide or potassium hydroxide.


Are there forms in which sodium chloride conducts electricity?

In order to conduct electricity, sodium chloride has to separate into its ionic forms (sodium ions and chloride ions). It does this in a water (aqueous) solution and also when in molten form, which is when heated above 801 °C.


Is magnesium sulphate melting point above 50 degrees Celsius?

Yes: FAR above.