Molar mass of calcium carbonate/calcium valence = 50,04345
Limestone is composed of at least 50% calcium carbonate (CaCO3) by weight. Therefore, the minimum amount of calcium carbonate in a limestone rock would be 50%.
The equivalent weight of calcium phosphate is calculated by dividing the molar mass of calcium phosphate by the valency factor of the phosphate ion. Since calcium phosphate is a salt with the formula Ca₃(PO₄)₂, its molar mass is calculated by adding the molar masses of calcium and phosphorus (since there are three calcium ions and two phosphate ions in the formula). The valency factor of phosphate ion is 2 since it can donate or accept 2 electrons.
The molecular weight of calcite, a mineral composed of calcium carbonate (CaCO3), is approximately 100.09 g/mol.
Calcium carbonate loses mass when heated because it decomposes into calcium oxide (quicklime) and carbon dioxide. This decomposition reaction releases carbon dioxide gas, causing the mass of the calcium carbonate to decrease.
Calcium carbonate is commonly used to express water hardness because it is a major component of the mineral deposits that form in plumbing and appliances. It is also a stable compound that is not affected by changes in pH, making it a reliable indicator of overall water hardness.
E.W= Molecular weight / # of ions = 100.09 (mg/mmol) /2 (meq/mmol) =50.043 mg/meq
Limestone is composed of at least 50% calcium carbonate (CaCO3) by weight. Therefore, the minimum amount of calcium carbonate in a limestone rock would be 50%.
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.
THE QUESTION !!! A student wanted to find the mass of calcium carbonate in an indigestion tablet. She crushed up a tablet and added an excess of HCL acid (25cm3 of 1.00 mol/dm3). She the titrated the excess against 0.5 mol/dm3 of NaOH requiring 25.8cm3 of the NaOH. Calculate the mass off calcium carbonate in the tablet.
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.
They need a good blood supply, calcium and to be mechanically stressed by movements of the body and by bearing weight.
Calcium carbonate loses weight when heated because it undergoes thermal decomposition, releasing carbon dioxide gas to form calcium oxide (quicklime). This process is known as calcination, where the compound breaks down into simpler substances at high temperatures.
The equivalent weight of calcium chloride (CaCl2) is 55.5 g/mol. This is the amount of the compound that can donate or accept one mole of electrons in a reaction.
To calculate the equivalent weight of an oxide, you first determine its molecular weight. Then you look at how many oxygen atoms are present in the formula of the oxide and divide the molecular weight by that number of oxygen atoms. This result is the equivalent weight of the oxide.
The equivalent weight of calcium phosphate is calculated by dividing the molar mass of calcium phosphate by the valency factor of the phosphate ion. Since calcium phosphate is a salt with the formula Ca₃(PO₄)₂, its molar mass is calculated by adding the molar masses of calcium and phosphorus (since there are three calcium ions and two phosphate ions in the formula). The valency factor of phosphate ion is 2 since it can donate or accept 2 electrons.
No, calcium carbonate is not typically used in soap manufacturing. It is more commonly used in industries such as food, pharmaceuticals, and construction due to its properties as a dietary supplement, binder, or filler.
The molecular weight of calcite, a mineral composed of calcium carbonate (CaCO3), is approximately 100.09 g/mol.