On heating 5.36 g of sodium sulfate crystals, 2.52 g of water is vaporised; thus, it can be concluded that the molecular formula of these crystals is .[Na=23g/mol,S=32g/mol,O=16g/mol,H=1g/mol]

How many moles of water are present in each mole of a hydrated chloride salt (XCl₂·nH2O) , given that 0.2 mol of XCl₂ combines with 21.6 g of water to form this salt?

[Cl=35.5 g/mol , O=16g/mol , H=1g/mol]

Crucibles A, B, and C each contain 0.1mol of CoCl₂ ·6H₂O , CuSO₄·5H₂O , and CoSO₄·7H₂O respectively. After heating them at a high temperature, the loss in mass from greatest to smallest is .

Sodium carbonate, Na₂CO₃ (also known as washing soda, soda ash, and soda crystals), is the anhydrous form of sodium carbonate decahydrate (Na₂CO₃·10H₂O) .Thus, the mass of vaporised water from the conversion of 10 mol of the hydrated form to the anhydrous form is .[Na=23g/mol,C=12g/mol,O=16g/mol,H=1g/mol]

If 3.478 g of hydrated magnesium chloride salt is intensely heated and the mass of the vaporised water is 1.848 g,then the formula of the hydrated compound is .............. .[Mg=24g/mol,Cl=35.5g/mol,O=16g/mol,H=1g/mol]

If the percentage of water of crystallization in a sample of hydrated magnesium sulfate (MgSO₄·xH₂O) is 62.26%,determine the number of moles of water (𝑥) in each mole of hydrated magnesium sulfate. [Mg=24g/mol,S=32g/mol,O=16g/mol,H=1g/mol]

If 200 grams of magnesium sulfate heptahydrate (MgSO₄·7H₂O) is strongly heated until the mass becomes constant, calculate, to the nearest two decimal places, the remaining mass of the anhydrous magnesium sulfate. [Mg=24g/mol , S=32g/mol,O=16g/mol,H=1g/mol]

When a sample of 10 g of strontium hydroxide was intensely heated, 5.42 g was lost. It could be concluded that the sample is in  form. [Sr=87.62g/mol,O=16g/mol,H=1g/mol]

If silver nitrate was added to 0.50 g of barium chloride sample, followed by adding sodium phosphate till complete precipitation, then the total weight of white precipitate formed would be ............................... g.

[Ba=137g/mol , Cl=35.5g/mol,Ag=108g/mol,P=31g/mol,O=16g/mol]

Ashless filter paper is used in chemical analysis by the  method because it does not leave ash after it is completely ignited.

Sodium hydroxide was used to differentiate between FeSO4 and FeCl3 solutions. If 0.05 g of a reddish-brown precipitate was formed, then the solution was  and the weight of the added NaOH was  g.

[Fe=56g/mol,Cl=35.5g/mol,S=32g/mol,O=16g/mol,H=1g/mol,Na=23g/mol]

If the addition of an excess amount of silver nitrate on an aqueous solution of ammonium chloride containing 5 g of impure ammonium chloride leads to the formation of 13 g of white precipitate, then the percentage of chlorine in the sample will be .

[N=14g/mol,H=1g/mol,Cl=35.5g/mol,Ag=108g/mol,O=16g/mol]

A magnesium halide salt has the formula MgX₂.A 0.789 g sample of MgX₂ was dissolved in 100 mL of deionised water followed by the addition of excess NaOH . The precipitate of Mg(OH)₂ was filtered, washed, and dried. 

The precipitate was found to have a mass of 0.249 g.

[Mg=24g/mol,O=16g/mol,H=1g/mol,F=19g/mol,Br=80g/mol,Cl=35.5g/mol,I=127g/mol]

According to the previous statement, symbol X represented the element .......

A student used a silver nitrate reagent to calculate the chloride content in a sodium chloride solution. After the precipitation, filtration, washing, and ignition processes, the weight of the precipitate was found to be higher than the right value. It is expected that .

Consider the following chemical reagents:

A. HCl

B. NaBr

C. NaNO₃

D. KI

All of the given chemical reagents can be utilized to determine silver salts content by the precipitation method except ..................... .

If 0.3165 g of a sample of barium ore is dissolved in nitric acid and 0.0856 g of white precipitate is obtained after the addition of an excess amount of H₂SO₄(aq),then the barium percentage in the sample of barium ore is ............. .[Ba=137g/mol,Cl=35.5g/mol,H=1g/mol,S=32g/mol,O=16g/mol]