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Why do we need distilled water in preparation of sodium hydroxide solution sodium carbonate and oxalic acid solutions?
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Why do you need distilled water in preparation of Naoh solution sodium carbonate and oxalic acid solution?
Distilled water is the closest one can get with conventional methods to pure water, which would be ideal to create solutions. Tap water is typically not used because it contains minerals and other foreign materials that can affect the solution itself, and alter results.
Does sodium hydrogen carbonate have a lower pH than sodium hydroxide?
It depends on the concentrations of these substances. However, sodium hydroxide is a very strong base and therefore is capable of producing solutions with high pH values. On the other hand, sodium hydrogen carbonate is weakly acidic, and is therefore capable of producing solutions that are somewhat less than neutral. (Carbonic acid is itself a weak acid.)
How do you distinguish sodium hydroxide and sodium acetate?
To test presence of Sodium ions, do a flame test: color observed: golden yellow. To test presence of carbonate or hydrogen carbonate ions: Take some of the sodium hydrogen carbonate in a dry test tube. Heat the test tube and bubble the gas through limewater. Limewater turns milky. Carbonate or hydrogen carbonate ions present. To distinguish between carbonate and hydrogen carbonate: Add indicator solution. If colour of solution turns green, pH is 7-8, hydrogen carbonate ions are present. If colour of solution turns blue, pH is 12-13, carbonate ions are present. -Iberuz
Why does sodium hydroxide and phenolphthalein mixture turn clear when carbon dioxide is added?
Carbon dioxide dissolves in the aqueous solution to produce carbonic acid. The carbonic acid dissociates to produce the carbonate ion and two protons. The protons reacts with the hydroxide provided by the already dissociated sodium hydroxide to produce water. The sodium carbonate is fairly soluble and stays in solution. Since the hydroxide ion is depleted, the phenolphthalein reverts from pink to clear as it does in solutions with a pH less than 8.3.
An aqueous solution that contains extra hydroxide ions is?
Basic solutions are solutions that have more than a 1E-7 concentration of hydroxide ion. Thus, solutions with "extra" hydroxide ions are basic. On the other hand, solutions with extra hydrogen (hydronium) ions are acidic.
Why do you need distilled water in preparation of Naoh solution sodium carbonate and oxalic acid solution?
Distilled water is the closest one can get with conventional methods to pure water, which would be ideal to create solutions. Tap water is typically not used because it contains minerals and other foreign materials that can affect the solution itself, and alter results.
Why should base solutions be carbonate free?
Base solutions should be carbonate free because of carbonate interference. They can cause impurities and changes to the concentration in the solutions.
Does sodium hydrogen carbonate have a lower pH than sodium hydroxide?
It depends on the concentrations of these substances. However, sodium hydroxide is a very strong base and therefore is capable of producing solutions with high pH values. On the other hand, sodium hydrogen carbonate is weakly acidic, and is therefore capable of producing solutions that are somewhat less than neutral. (Carbonic acid is itself a weak acid.)
How do you distinguish sodium hydroxide and sodium acetate?
To test presence of Sodium ions, do a flame test: color observed: golden yellow. To test presence of carbonate or hydrogen carbonate ions: Take some of the sodium hydrogen carbonate in a dry test tube. Heat the test tube and bubble the gas through limewater. Limewater turns milky. Carbonate or hydrogen carbonate ions present. To distinguish between carbonate and hydrogen carbonate: Add indicator solution. If colour of solution turns green, pH is 7-8, hydrogen carbonate ions are present. If colour of solution turns blue, pH is 12-13, carbonate ions are present. -Iberuz
What is sodium chloride commonly used in?
Some important applications of sodium chloride- seasoning for foods- preservative for foods- preparation of sodium, chlorine, sodium hydroxide, hydrogen- roads deicing- soaps fabrication- salts baths- isotonic solutions - sodium is indispensable for lifeetc.Some important applications of sodium chloride- seasoning for foods- preservative for foods- preparation of sodium, chlorine, sodium hydroxide, hydrogen- roads deicing- soaps fabrication- salts baths- isotonic solutions- sodium is indispensable for lifeetc.
An aqueous solution that contains extra hydroxide ions is?
Basic solutions are solutions that have more than a 1E-7 concentration of hydroxide ion. Thus, solutions with "extra" hydroxide ions are basic. On the other hand, solutions with extra hydrogen (hydronium) ions are acidic.
Why does sodium hydroxide and phenolphthalein mixture turn clear when carbon dioxide is added?
Carbon dioxide dissolves in the aqueous solution to produce carbonic acid. The carbonic acid dissociates to produce the carbonate ion and two protons. The protons reacts with the hydroxide provided by the already dissociated sodium hydroxide to produce water. The sodium carbonate is fairly soluble and stays in solution. Since the hydroxide ion is depleted, the phenolphthalein reverts from pink to clear as it does in solutions with a pH less than 8.3.
What products can you get from salt?
Some important applications of sodium chloride - preparation of sodium, chlorine, sodium hydroxide, hydrogen- soaps fabrication- salts baths- isotonic solutions and other applications in medicine
How salt is and was used?
Sodium chloride applications - seasoning for foods - preservative for foods - preparation of sodium, chlorine, sodium hydroxide, hydrogen - roads deicing - soaps fabrication - salts baths - isotonic solutions etc.
What is a substance that produces hydroxide ions in aqueous solutions?
Acid
Solutions of aluminum acetate and lithium hydroxide are mixed?
2
What do you get when aqueous solutions of sodium carbonate and zinc chloride are combined?
Sodium chloride solution with zinc carbonate precipitate.
