Hydrates II

Name the following ionic compound: MgSO₄*7H₂O

• magnesium sulfate * hexahydarte
• magnesium sulfate hexahydarte
• magnesium sulfate heptahydrate
• magnesium sulfate* heptahydrate

Name the following hydrate:  NaCl * 5H₂O

• sodium chloride 
• sodium monochloride pentahydrate
• sodium chloride pentahydrate
• pentahydrate

A hydrate of magnesium chloride is present and the following data is collected:
mass of crucible = 22.130 grams
mass of crucible + hydrate = 25.290 grams
mass of crucible and contents after heating = 23.491 grams
What is the complete formula of this hydrate?

• MgCl₂ · 7H₂O
• MgCl₂ · 11H₂O
• MgCl₂ · 6H₂O
• MgCl₂ · 13H₂O

1. A sample of a compound has a mass of 65.00 grams when 0.457 moles are present. Is the compound lithium sulfate( Li₂SO₄) 109.9g/mol or sodium sulfate (Na₂SO₄)   142.1g/mol?

• 1. Li₂SO₄

• 1. Na₂SO₄

Crucible, cover: 17.8 g
Crucible, cover, and hydrate: 23.9g
Crucible, cover, and salt: 21.5g
Calculate % of water lost.

• 90.0%
• 60.7%
• 39.3%
• 45.5%

A 5.00 g sample of hydrated barium chloride, BaCl₂ · nH₂O, is heated to drive off the water. After heating, 4.26 g of anhydrous barium chloride, BaCl₂, remains. What is the formula of the hydrate?

Molar Mass: BaCl₂: 208.23 g/mol

Molar Mass Water: 18.02 g/mol

• BaCl₂ · 2H₂O

• BaCl₂ · 3H₂O

• 2BaCl₂ · H₂O

• BaCl₂ · 5H₂O