Chemistry

posted by .

A 5 gram sample of a hydrate of BaCL2 was heated, and only 4.3g of the anhydrous salt remained. What percentage of water was in the hydrate?

  • Chemistry -

    How much water water was evolved? That is 5g - 4.3 g = 0.7g
    %H2O = (0.7/5)*100 = ?

  • Chemistry -

    14%

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry 11

    Hi, I am stuck on a couple questions in chemistry 11. The questions are 1. Calculate the number of moles of the anhydrous salt left behind 2. Calculate the number of moles of water removed by heat from your sample of hydrate. 3. Calculate …
  2. chemistry

    If 4.36g of a hydrate of the salt baCl2 is heated and in the process losses 0.6431g of mass, show all your work to calculate the amount of water X in the hydrate, BaCl2.XH2O
  3. chemistry

    if 4.36g of a hydrate of the salt baCl2 is heated and in the process losses 0.6431g of mass, show all your work to calculate the amount of water X in the hydrate, BaCl2.XH2O
  4. chemistry

    A 2.50 g sample of a hydrate of calcium sulphate losses 0.523 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
  5. chemistry

    A 2.500 gram sample of hydrate of calcium sulfate loses 0.532 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
  6. chemistry

    I need help with this lab. Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate: 93.000g Mass of crucible and pure salt: 91.196g I need to calculate the following: 1. mass of water in hydrate …
  7. chemistry

    a 5.00g sample of a hydrate of barium chloride was heated, and only 4.30g of the anhydrous salt remained. what is the formula of the hydrate?
  8. chemistry

    A 2.50g sample of a hydrate of calcium nitrate was heated, and only 1.70g of the anhydrous salt remained. what is the formula of the hydrate?
  9. Chemistry

    Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass of salt 91.196g 1. Calculate the following: a:mass of water in the hydrate sample (g) b:number of moles of water in the sample c:mass of pure salt in the sample (g) …
  10. Chemistry

    7. A student conducts an experiment on a different hydrate. The empty crucible is heated to a constant mass of 24.330. A sample of the unidentified hydrate is placed in the crucible, and the total mass is 31.571 g. The crucible and …

More Similar Questions