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Hydrogen carbonate calcium

Inside newiy formed caverns, calcium carbonate precipitates from water dripping from the ceilings of the chambers. This happens when water that is saturated with carbon dioxide and calcium hydrogen carbonate comes into contact with air. Some of the dissolved CO2 escapes into the gas phase. This shifts the two equilibria to the left, and solid calcium carbonate precipitates ... [Pg.1192]

Write formulas for each of the following compounds (a) calcium hydrogen carbonate, (b) disodium hydrogen phosphate, (c) sodium dihydrogen phosphate, and (d) calcium dihydrogen phosphate. [Pg.111]

Calcium hydrogen carbonate plus heat yields calcium carbonate plus carbon dioxide plus water... [Pg.124]

This compound is calcium bicarbonate or calcium hydrogen carbonate. The S042" ion is the sulfate ion. The cation is Fe2+, iron(II). [Pg.42]

E 170 Calcium carbonates (i) Calcium carbonate (ii) Calcium hydrogen carbonate... [Pg.33]

Temporary hardness, caused by hydrogen carbonate (or bicarbonate) ions, can be removed through boiling. For example, calcium hydrogen carbonate, often present in temporary hard water, is boiled in a teapot to remove its hardness. In this, process, a scale, composed of insoluble calcium carbonate, forms on the inside of the kettle. ... [Pg.99]

Carbonates. Carbonic acid H CO, is present to the extent of (1.27 i of the total CO present in ihe solution that is formed by dissolving CO in H 0 ai room temperature. The CO may be expelled fully upon boiling. The solution reads with alkalis to form carbonates, e.g. sodium carbonate, sodium hydrogen carbonate, calcium carbonate, calcium hydrogen carbonate. The acid ionization constant usually cited for carbonic... [Pg.285]

Limestone is mostly made up of the mineral calcite, or calcium carbonate (CaC03). As the calcium carbonate rock dissolves in the slightly acidic water, spaces and even caves develop underground. If carbonic acid dissolves all the way through the rock and into a cave below the Earth s surface, the resulting solution contains calcium hydrogen carbonate (calcium bicarbonate). [Pg.66]

Since liquid impurities may produce exudates in explosive compositions, to avoid this the crude product should be purified. For a preliminary washing, a dilute (2%) solution of sodium carbonate may be used. Picric acid reacts with the carbonate which then goes into solutions as sodium picrate. Instead of sodium carbonate milk of lime or calcium hydrogen carbonate may be used. [Pg.484]

Desvergnes describes the purification process used in various plants as follows. A wooden double-bottomed vat of 650 1. capacity is charged with 350 kg of dinitro-phenol, which is stirred with 200 1. of a 3% solution of calcium hydrogen carbonate at a temperature of 70°C. The contents of the vat are allowed to remain at rest for 1 hr, then the aqueous solution is decanted and the operation is repeated with a fresh solution of calcium hydrogen carbonate. Then the purified product is washed with cold water. The melting point of dinitrophenol obtained is about 105.5%... [Pg.484]

The compounds dissolved both in the spent calcium hydrogen carbonate solutions and in the sulphuric acid, such as mononitrophenols, dinitrophenols and picric acid, may be recovered by precipitation from the calcium hydrogen carbonate solution by acidification, and from sulphuric acid solution by dilution with water. [Pg.484]

On boiling the precipitate becomes crystalline. The precipitate is soluble in water which contains excess carbonic acid (e.g. freshly prepared soda water), because of the formation of soluble calcium hydrogen carbonate ... [Pg.283]

Excess hydrochloric acid was added to an aqneous solution of calcinm hydrogen carbonate, and the resnlting solntion was evaporated to dryness, which produced 2.29 g of solid product. Calculate the mass of calcium hydrogen carbonate in the original solntion. [Pg.276]

Some reactions, such as an explosion of nitroglycerine, inherently tend to proceed rapidly. Others, such as the reaction of solid limestone with carbon dioxide in water to form soluble calcium hydrogen carbonate, tend to proceed slowly. It may take centuries for underground streams to form caverns by reaction with limestone (see Figure 8.9). For a given reaction, chemists have no control over the nature of the reactants. [Pg.481]

Carbon dioxide in natural waters solubilizes the calcium carbonate of limestone or marble by forming soluble calcium hydrogen carbonate (bicarbonate) (Eqs. 5.8 and 5.9). This is the process, which puts bicarbonate hardness into solution in surface water or groundwater supplies. [Pg.144]

Write balanced chemical equations for each of the following processes (a) Calcium phosphate reacts with sulfuric acid to produce calcium sulfite and phosphoric acid, (b) Calcium phosphate reacts with water contaming dissolved carbon dioxide to produce calcium hydrogen carbonate and calcium hydrogen phosphate. [Pg.173]

General experience has shown that the magnitude of an isotopic fractionation significantly depends on the type of chemical bond of the investigated species in the reaction. Usually, a larger isotopic fractionation is found in exchange reactions where isotopes are covalently bound than in the case of an ionic bond. As an example, the fractionated precipitation of calcium carbonate from a calcium hydrogen carbonate solution by means of a step-by-step desorption of COj will be discussed ... [Pg.83]

Limestone is primarily calcium carbonate, CaC03. Calcium carbonate reacts with carbon dioxide and water to form calcium hydrogen carbonate, Ca(HC03)2, a water-soluble compound. Lakes in areas rich in limestone have significant concentrations of hydrogen carbonate ions. [Pg.535]

Just as in the regulation of pH in the blood, hydrogen carbonate ions produced from calcium hydrogen carbonate form a base that can neutralize acid in lakes. [Pg.535]

If the water were removed from the product mixture, calcium hydrogen carbonate. [Pg.144]

Write the formulas that correspond to the names nickel(II) hydroxide, ammonium chloride, and calcium hydrogen carbonate. [Pg.196]

The mineral adsorbs Cl and NO3 ions poorly and reversibly, whilst S04 is precipitated at the mineral surface. Phosphates are preferentially adsorbed on calcium carbonate. Soils which contain CaCOj show pH values ranging from about 7 to 8.4, due to the formation of calcium hydrogen carbonate. The formation of this compound is accelerated in biologically active soils, with a high production of carbon dioxide. Calcareous soils have a soil solution dominated by Ca + ions, and this limits swelling of soil days and prevents the dispersion of finer particles in the soil. If Ca predominates on the exchange complex of soils, the pH value is maintained above 5.5. [Pg.80]

In Table 3.36 the mean content of chemical elements in surface waters of the Earth is presented. The table shows that sodium chloride prevails in the sea waters, and calcium hydrogen carbonate in common continental waters. [Pg.161]

Calcium carbonate reacts to fonn calcium hydrogen-carbonate sdution... [Pg.198]

The culprit is a soluble compound of calcium called calcium hydrogen carbonate. When we heat water, this substance decomposes to yield carbon dioxide, which, being a gas, dissipates into the air, and calcium carbonate, a water-insoluble compound... [Pg.213]

Chemically speaking, limestone is calcium carbonate. Although calcium carbonate is insoluble in water, it does dissolve in a weakly acidic solution. Surface water is weakly acidic, because carbon dioxide in the air dissolves in rain and reacts with the water to form carbonic acid. As the acidic surface water percolates through the ground, it converts insoluble calcium carbonate to soluble calcium hydrogen carbonate. When we heat water, we reverse this reaction, causing deposits of what amounts to limestone to build. [Pg.214]

You will prepare temporarily hard water by bubbling carbon dioxide gas, CO2, through an aqueous solution of calcium hydroxide, Ca(0H)2/ until the precipitate of calcium carbonate, C COj, that first forms just dissolves as a result of formation of calcium hydrogen carbonate, Ca(HC03)2 ... [Pg.440]


See other pages where Hydrogen carbonate calcium is mentioned: [Pg.76]    [Pg.156]    [Pg.157]    [Pg.268]    [Pg.543]    [Pg.66]    [Pg.112]    [Pg.151]    [Pg.22]    [Pg.244]    [Pg.248]    [Pg.61]    [Pg.61]    [Pg.201]    [Pg.150]    [Pg.48]    [Pg.271]    [Pg.214]    [Pg.178]    [Pg.780]   
See also in sourсe #XX -- [ Pg.61 , Pg.94 ]

See also in sourсe #XX -- [ Pg.14 ]




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