Nai h2so4

The structural properties of these electrolyte films were examined by X-ray diffraction XRD studies. The proton conductivity and impedance of the electrolyte were studied with changing sulfuric acid concentration from nai h2so4 to 5.

This page describes and explains the redox reactions involving halide ions and concentrated sulphuric acid. It uses these reactions to discuss the trend in reducing ability of the ions as you go from fluoride to chloride to bromide to iodide. There are two different types of reaction which might go on when concentrated sulphuric acid is added to a solid ionic halide like sodium fluoride, chloride, bromide or iodide. The concentrated sulphuric acid can act both as an acid and as an oxidising agent. The concentrated sulphuric acid gives a hydrogen ion to the halide ion to produce a hydrogen halide.

Nai h2so4

Started by JJoseph Board Chemistry. Started by taregg Board Chemistry. Science News Features. Interviews Answers to Science Questions. Pages: [ 1 ] Go Down. What is the reaction between sulphuric acid and sodium iodide? Hi this is Eunice, Sean's sister, My AS level Chemistry is next week and im stuck, help me out please Jan, Module 2 3e describe two observations that you would make when concentrated sulphuric acid is added to solid sodium iodide. Write an equation for a reaction that occurs in which iodide ions are oxidised by the sulphuric acid. They say that when you die, your life flashes in front of you. Make it worth watching! Jeeze, that's an intense test question!!! Since H2SO4 is a diprotic acid so it will react twice. After thinking about it for a minute, I don't think you need all of that redox balancing with that one extra equation you can just add and subtract equations to reach the one at the bottom.

Iodide ions reduce the sulphuric acid to a mixture of products including hydrogen sulphide. By contrast, nai h2so4, for the energetic reasons you will find discussed, iodine is relatively reluctant to form its negative ion in solution.

Direct link to this balanced equation:. A chemical equation represents a chemical reaction. It shows the reactants substances that start a reaction and products substances formed by the reaction. However, this equation isn't balanced because the number of atoms for each element is not the same on both sides of the equation. A balanced equation obeys the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction.

Direct link to this balanced equation:. A chemical equation represents a chemical reaction. It shows the reactants substances that start a reaction and products substances formed by the reaction. However, this equation isn't balanced because the number of atoms for each element is not the same on both sides of the equation. A balanced equation obeys the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction. This is the most straightforward method. It involves looking at the equation and adjusting the coefficients to get the same number of each type of atom on both sides of the equation. Process: Start with the most complex molecule or the one with the most elements, and adjust the coefficients of the reactants and products until the equation is balanced. This method uses algebraic equations to find the correct coefficients.

Nai h2so4

H 2 SO 4 is categorized as a strong acid. Sodium iodide is formed by the reaction of sodium metal and iodine. These two components react to generate fumes of hydrogen iodide and the color of the resultant solution is red. Let us discuss the product formed when H 2 SO 4 reacts with NaI, the type of reaction, the net ionic equation and many other related topics in this article. Sulphuric acid reacts with sodium iodide to give sodium sulphate, hydrogen sulphide, iodine and water. We need a burette, conical flask, burette holder, volumetric flask, and beakers for this titration. The phenolphthalein or methyl orange indicator can be used because it is a strong acid versus weak base reaction, and its endpoint is pink to colorless. The burette was filled with standardized H 2 SO 4 and NaI was taken in a conical flask along with the respective indicator. H 2 SO 4 is added dropwise to the conical flask and the flask was shaking constantly. After a certain time when the endpoint arrived, indicator changes its color and the reaction was done.

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We need to supply the energy to remove the electron from the chloride ion. Chemical forum. Fluorine is a very powerful oxidising agent because it very readily forms its negative ion in solution. The total enthalpy change will be the sum of the enthalpy changes for the halide ion half-reaction and the sulphuric acid half-reaction. There will also be red colours where the iodine comes into contact with the solid iodide. Bromide ions reduce the sulphuric acid to sulphur dioxide. Limiting reagent can be computed for a balanced equation by entering the number of moles or weight for all reagents. Because this is a gas, it immediately escapes from the system. It sounds convincing, but it only tells part of the story. The table shows that this isn't anything to do with the amount of energy needed to remove an electron from a fluoride ion. O is balanced: 4 atoms in reagents and 4 atoms in products.

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Now, both sides have 4 H atoms and 2 O atoms. It is actually easier to remove an electron from a fluoride ion than from a chloride ion. UK A' level students should search their syllabuses, past exam papers, mark schemes and any other support material available from their Exam Board. With bromide ions The bromide ions are strong enough reducing agents to reduce the concentrated sulphuric acid. The iodide ions are oxidised to iodine. There are two different types of reaction which might go on when concentrated sulphuric acid is added to a solid ionic halide like sodium fluoride, chloride, bromide or iodide. O is balanced: 4 atoms in reagents and 4 atoms in products. This only works and even then, not very well! Correspondence to E. The fluoride and chloride ions aren't strong enough reducing agents to reduce the sulphuric acid.