Molar mass of calcium carbonate/calcium valence = 50,04345
equivalent weight of calcium phosphate
because its molecular weight is 100.....
Limestone loses mass when heated because of a chemical change: the gas carbon dioxide (CO2) is released by a chemical process when the rock is heated. The heat turns some of the calcium carbonate of the limestone into calcium oxide (quicklime) and carbon dioxide.
Calcium Stearate is prepared by melting stearic acid and adding the stochiometric equivalent weight of calcium hydroxide (hydrated lime). The liquid is then mixed until the reaction is completed. It is usually then spray dried into a powder.
Equivalent weight ofc11h17n3os2 from molecular weight271.402
E.W= Molecular weight / # of ions = 100.09 (mg/mmol) /2 (meq/mmol) =50.043 mg/meq
equivalent weight of calcium phosphate
Dolomite is a type of carbonate material that is made up of calcium magnesium carbonate. The weight of dolomite depends on how big the chunk is that you're looking at.
1. Weight a sample (m1) of approx. 5 g from the mixture and put in a beaker.2. Add approx. 50 mL water and stir vigourously.3. Transfer quantitatively the suspension on a preweighed sintered glass filter (m2).4. Calcium carbonate being insoluble in water remain on the filter.5. Dry the filter at 110 0C and weigh (m3).6. Calculate the weight of CaCO3: m4 = m3 -m2.7. Calculate the percentage of calcium carbonate: m5 = (m4 x 100)/m1.
55
because its molecular weight is 100.....
Because it has decomposed to carbon dioxide and calcium oxide, and the carbon dioxide is gaseous, has dispersed into the natural atmosphere, and therefore is no longer part of the weight.
They need a good blood supply, calcium and to be mechanically stressed by movements of the body and by bearing weight.
yes it is also used in order to increase the weight of the soap
140.944
Take water in a beaker. Add sodium carbonate to it and stir till sodium carbonate dissolves. However for scientific or any practical purpose, take a fixed weight of sodium carbonate and dissolve in a definite volume of water and calculate the concentration in terms of molarity or weight per volume etc.
CaCO3(s) ==heat==> CaO(s)+CO2(g) The correct chemical expression you need is NOT 'heated' , but 'Thermal Decomposition'. Calcium carbonate when heated to about 900 oC ( red glowing heat) will undergo thermal decomposition , to form calcium oxide((quick)lime) and carbon dioxide. Visually, you don't see anything. Calcium carbonate is white in coliur as is Calcium Oxide. You do not see carbon dioxide being given off. The only way to check is by weighing the mass of calcium carbonate. Heat it. Re-weigh when cool. It shoulk be of less weight. The difference being the mass of CO2 liberated, which you cannot weigh.