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bogdanovich [222]
3 years ago
13

During the course of your experiment you have obtained the following data: mass of the hydrate: 1.973 g mass of the anhydrate: 1

.196 g The formula of the anhydrous salt: CaCl2 Calculate the following: (round to correct the number of significant figures and include units as required). mass of water loss in . number of moles of anhydrous salt after heating, in moles number of moles of water lost, in moles • number of moles of water per mole of hydrate, in moles (round to the whole number) provide the formula of a hydrate Note: you will not be able to add the bscript and leave one space between ionic compound and water.
Chemistry
1 answer:
Helen [10]3 years ago
5 0

Answer:

See explanation

Explanation:

Mass of water lost = mass of hydrated salt - mass of anhydrous salt

Mass of water lost = 1.973 g - 1.196 g = 0.777g

Number of moles of water lost = 0.777g/18g/mol = 0.043 moles

Number of moles of anhydrous salt = 1.196 g /111g/mol = 0.011 moles

To obtain the number of moles of water of crystalization per hydrate molecule;

Number of moles of anhydrous salt = number of moles of hydrated salt

0.011 = 1.973 /111 + 18x

0.011(111 + 18x) = 1.973

1.221 + 0.198x = 1.973

0.198x = 1.973 - 1.221

x= 4

Hence, there are 4 moles of water per hydrate molecule. The formula of the hydrate is CaCl2.4H2O

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Explanation:

Hello!

In this case, since we are asked to note down the complete molecular equation, complete ionic equation and the net ionic equation for the reaction between acetic acid (weak acid) and barium hydroxide (strong base), we proceed as shown below:

- Complete molecular equation:

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2CH_3COOH(aq)+Ba^{2+}(aq)+2OH^-(aq)\rightarrow Ba^{2+}(aq)+2CH_3COO^-(aq)+2H_2O(l)

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2CH_3COOH(aq)+2OH^-(aq)\rightarrow 2CH_3COO^-(aq)+2H_2O(l)\\\\CH_3COOH(aq)+OH^-(aq)\rightarrow CH_3COO^-(aq)+H_2O(l)

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