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  2. Calcium carbonate - Wikipedia

    en.wikipedia.org/wiki/Calcium_carbonate

    Calcium carbonate is a chemical compound with the chemical formula Ca CO 3. It is a common substance found in rocks as the minerals calcite and aragonite , most notably in chalk and limestone , eggshells , gastropod shells , shellfish skeletons and pearls .

  3. Neutralization (chemistry) - Wikipedia

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

    For example, hydrochloric acid, HCl, is a strong acid. HCl(aq) → H + (aq) + Cl − (aq) A strong base is one that is fully dissociated in aqueous solution. 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 ...

  4. Calcium bicarbonate - Wikipedia

    en.wikipedia.org/wiki/Calcium_bicarbonate

    As the groundwater enters the cave, the excess carbon dioxide is released from the solution of the bicarbonate, causing the much less soluble calcium carbonate to be deposited. In the reverse process, dissolved carbon dioxide (CO 2) in rainwater (H 2 O) reacts with limestone calcium carbonate (CaCO 3) to form soluble calcium bicarbonate (Ca(HCO ...

  5. Hydrochloric acid - Wikipedia

    en.wikipedia.org/wiki/Hydrochloric_acid

    Hydrochloric acid has been used for dissolving calcium carbonate, e.g. such things as de-scaling kettles and for cleaning mortar off brickwork. When used on brickwork the reaction with the mortar only continues until the acid has all been converted, producing calcium chloride, carbon dioxide, and water: CaCO 3 + 2 HCl → CaCl 2 + CO 2 + H 2 O

  6. Effervescence - Wikipedia

    en.wikipedia.org/wiki/Effervescence

    In the laboratory, a common example of effervescence is seen if hydrochloric acid is added to a block of limestone. If a few pieces of marble or an antacid tablet are put in hydrochloric acid in a test tube fitted with a bung, effervescence of carbon dioxide can be witnessed. CaCO 3 + 2 HCl → CaCl 2 + H 2 O + CO 2 ↑

  7. Calcium lactate - Wikipedia

    en.wikipedia.org/wiki/Calcium_lactate

    Calcium lactate can be prepared by the reaction of lactic acid with calcium carbonate or calcium hydroxide.. Since the 19th century, the salt has been obtained industrially by fermentation of carbohydrates in the presence of calcium mineral sources such as calcium carbonate or calcium hydroxide.

  8. Aragonite - Wikipedia

    en.wikipedia.org/wiki/Aragonite

    Aragonite is the high pressure polymorph of calcium carbonate. As such, it occurs in high pressure metamorphic rocks such as those formed at subduction zones. [13] Aragonite forms naturally in almost all mollusk shells, and as the calcareous endoskeleton of warm- and cold-water corals (Scleractinia). Several serpulids have aragonitic tubes. [14]

  9. Calcium hydrosulfide - Wikipedia

    en.wikipedia.org/wiki/Calcium_hydrosulfide

    It is formed from the reaction of calcium hydroxide or calcium carbonate with hydrogen sulfide: [2] Ca(OH) 2 + 2H 2 S → Ca(HS) 2 + 2H 2 O