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When a reaction equation is not balanced, the coefficients show inequality. Here is an example with the separation of natural gas from hydrochloric acid using magnesium. Mg + HCl → MgCl 2 + H 2 (unbalanced) Here is the element-reaction-product table:
In chemistry, equivalent weight (also known as gram equivalent [1] or equivalent mass) is the mass of one equivalent, that is the mass of a given substance which will combine with or displace a fixed quantity of another substance.
A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and chemical formulas.The reactant entities are given on the left-hand side and the product entities are on the right-hand side with a plus sign between the entities in both the reactants and the products, and an arrow that points towards the products to show the direction of the reaction. [1]
For example, sodium hydroxide, NaOH, is a strong base. NaOH(aq) → Na + (aq) + OH − (aq) Therefore, when a strong acid reacts with a strong base the neutralization reaction can be written as H + + OH − → H 2 O. For example, in the reaction between hydrochloric acid and sodium hydroxide the sodium and chloride ions, Na + and Cl − take ...
Phosphorous acid (or phosphonic acid) is the compound described by the formula H 3 PO 3.This acid is diprotic (readily ionizes two protons), not triprotic as might be suggested by this formula.
The Brønsted–Lowry theory (also called proton theory of acids and bases [1]) is an acid–base reaction theory which was first developed by Johannes Nicolaus Brønsted and Thomas Martin Lowry independently in 1923.
Ammonium phosphomolybdate can be made by heating ammonium orthomolybdate combined with phosphoric acid and nitric acid, yielding ammonium nitrate, water, and a yellow precipitate of ammonium phosphomolybdate is obtained.
Amphoteric is derived from the Greek word amphoteroi (ἀμφότεροι) meaning "both".Related words in acid-base chemistry are amphichromatic and amphichroic, both describing substances such as acid-base indicators which give one colour on reaction with an acid and another colour on reaction with a base.