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  2. Ammonia solution - Wikipedia

    en.wikipedia.org/wiki/Ammonia_solution

    Because aqueous ammonia is a gas dissolved in water, as the water evaporates from a surface, the gas evaporates also, leaving the surface streak-free. Its most common uses are to clean glass [10], porcelain, and stainless steel. It is good at removing grease and is found in products for cleaning ovens and for soaking items to loosen baked-on grime.

  3. Ammonia fountain - Wikipedia

    en.wikipedia.org/wiki/Ammonia_fountain

    The experiment consists of introducing water through an inlet to a container filled with ammonia gas. [1] Ammonia dissolves into the water and the pressure in the container drops. As a result, more water is forced into the container from another inlet creating a fountain effect.

  4. Ammonia - Wikipedia

    en.wikipedia.org/wiki/Ammonia

    Ammonia readily dissolves in water. In an aqueous solution, it can be expelled by boiling. The aqueous solution of ammonia is basic, and may be described as aqueous ammonia or ammonium hydroxide. [30] The maximum concentration of ammonia in water (a saturated solution) has a specific gravity of 0.880 and is often known as '.880 ammonia'. [31]

  5. Solubility chart - Wikipedia

    en.wikipedia.org/wiki/Solubility_chart

    The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.

  6. Solvated electron - Wikipedia

    en.wikipedia.org/wiki/Solvated_electron

    Solvated electrons are involved in the reaction of alkali metals with water, even though the solvated electron has only a fleeting existence. [10] Below pH = 9.6 the hydrated electron reacts with the hydronium ion giving atomic hydrogen, which in turn can react with the hydrated electron giving hydroxide ion and usual molecular hydrogen H 2. [11]

  7. Neutralization (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Neutralization_(chemistry)

    The pH at the end-point is greater than 7 and increases with increasing concentration of the acid, T A, as seen in the figure. In a titration of a weak acid with a strong base the pH rises more steeply as the end-point is approached. At the end-point, the slope of the curve of pH with respect to amount of titrant is a maximum.

  8. This Family Drives 350 Miles For What Could Be A Common ...

    projects.huffingtonpost.com/projects/dying-to-be...

    The first stop is his mother’s modular home in Hermosa, just south of the city, where he will change cars. In the distance, the lights of Rapid City are mostly dark or blinking like strings of busted Christmas tree lights. The road is covered in snow, and Fischer can’t see a thing. He fingers his patchy beard and talks at double speed.

  9. Hydrolysis - Wikipedia

    en.wikipedia.org/wiki/Hydrolysis

    Hydrolysis (/ h aɪ ˈ d r ɒ l ɪ s ɪ s /; from Ancient Greek hydro- 'water' and lysis 'to unbind') is any chemical reaction in which a molecule of water breaks one or more chemical bonds. The term is used broadly for substitution, elimination, and solvation reactions in which water is the nucleophile. [1]