When a 8.192 g sample of bluish-green crystals of hydrated nickel(II) sulfate is heated, all of...
Question:
When a {eq}8.192\ g {/eq} sample of bluish-green crystals of hydrated nickel(II) sulfate is heated, all of the water of hydration is lost leaving {eq}4.826\ g {/eq} of anhydrous nickel(II) sulfate. Write the formula of the hydrated crystal, showing the number of moles of water-bound per mole of salt.
Hydrated Salts:
When removing water from a reaction carried out in an aqueous environment, the use of anhydrous salts can come in handy. Once placed in water, this type of salt entraps water and becomes a hydrated salt. The number of water molecules that each particle of anhydrous salt can trap depends from one salt to another.
Answer and Explanation: 1
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View this answerThe given 4.826 g provides the mass of nickel (II) sulfate free of water. We can convert this to moles using its molar mass, 154.76 g/mol:
{eq}\rm...
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Hydrates: Determining the Chemical Formula From Empirical Data
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Chapter 9 / Lesson 8
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Learn the anhydrate definition and what a hydrated compound is. Understand what an anhydrate is, the hydrate formula, and how to find the formula of the hydrate.
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