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lesson 3 (part 2) chapter 2

Quiz by hamada amin

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20 questions
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  • Q1

    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]

    7Na₂SO₄·H₂O

    Na₂SO₄·H₂O

    Na₂SO₄·14H₂O

    Na₂SO₄·7H₂O

    300s
  • Q2

    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]

    10 mol

    12 mol

    3 mol

    6 mol

    300s
  • Q3
    300s
  • Q4

    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 .

    crucible C, B, then A

    crucible C, A, then B

    crucible A, B, then C

    crucible B, A, then C

    120s
  • Q5

    The following data were collected during the gravimetric analysis of a sample of hydrated calcium chloride (CaCl₂·xH₂O)

    What is the number of moles of water of crystallisation (x) in the hydrated calcium chloride sample? Give your answer to the nearest two decimal places. [Ca=40g/mol,Cl=35.5g/mol,O=16g/mol,H=1g/mol]

    Question Image

    2.00 mol

    0.02 mol

    1.00 mol

    0.36 mol

    300s
  • Q6

    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]

    286 g

    1‎800 g

    180 g

    106 g

    300s
  • Q7

    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]

    3MgCl₂·7H₂O

    MgCl₂·3.5H₂O

    MgCl₂·H₂O

    MgCl₂·6H₂O

    300s
  • Q8

    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]

    11 mol

    1 mol

    2 mol

    3 mol

    300s
  • Q9

    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]

    97.56 g

    48.78 g

    120.00 g

    126.00 g

    300s
  • Q10

    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]

    a tetrahydrate

    a pentahydrate

    an octahydrate

    a monohydrate

    300s
  • Q11

    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]

    0.48

    0.69

    0.90

    1.17

    300s
  • Q12
    300s
  • Q13

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

    neutralisation

    precipitation

    volatilisation

    titration

    120s
  • Q14

    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]

    FeSO4 , 0.022

    FeCl3 , 0.019

    FeSO4 , 0.044

    FeCl3 , 0.056

    300s
  • Q15

    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]

    64.3%

    18.6%

    38.5%

    4.3%

    300s

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