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3 years ago

What is the precipitate that will form from the reaction of barium chloride dihydrate with sodium sulfate decahydrate?

2 answers:

4 0

<span>immediate milky appearance
after 5-10 minutes a precipitate of BaSO4 will settle out of solution the the solution will be clear.
</span>but mostly a white precipitate

MakcuM [25]3 years ago

4 0

The formation of an insoluble salt on mixing of two solutions which contains soluble salts is refer to a precipitation reaction. The insoluble salt formed in the reaction is said to be a precipitate and can be separated by filtration or any other separation method.

The formula for barium chloride dihydrate is $BaCl_2.2H_2O$ .

The formula for sodium sulfate decahydrate is $Na_2SO_4.10H_2O$ .

The hydrates on the above compounds represents that they are in the aqueous phase. So, the reaction is:

$BaCl_2(aq) + Na_2SO_4(aq) \rightarrow BaSO_4(s) + NaCl(aq)$

The above equation is not balanced as the number of atoms of elements on the reactant side is not equal to the number of atoms of elements on the product side. So, in order to balance the reaction, $NaCl$ on the reactant side is multiplied by 2. Thus, the balanced chemical equation is:

$BaCl_2(aq) + Na_2SO_4(aq) \rightarrow BaSO_4(s) + 2NaCl(aq)$

Hence, the precipitate that will form from the reaction of barium chloride dihydrate with sodium sulfate decahydrate is barium sulfate, $BaSO_4$ .

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2 years ago

How many atoms are in 1.204x10^22 moles of arsenic?

ra1l [238]

Answer:

<h2>0.02 moles </h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

We have

$n = \frac{1.204 \times {10}^{22} }{6.02 \times {10}^{23} } \\ = 0.02$

We have the final answer as

<h3>0.02 moles</h3>

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7 0

2 years ago

An iron(iii) sulfate hydrate is 18.4% water. What is the formula of the hydrate? What is the name of the hydrate?

aleksley [76]

Answer:- Formula of the hydrate is $Fe_2(SO_4)_3.5H_2O$ and it's name is Iron(III)sulfate pentahydrate.

Solution:- As per the given information, there is 18.4% water in the hydrate. If we assume the mass of the hydrate as 100 grams then there would be 18.4 grams of water and 81.6 grams of Iron(III)sulfate present in the hydrate.

Molar mass for Iron(III)sulfate is 399.88 gram per mol and the molar mass for water is 18.02 gram per mol.

We will calculate the moles of Iron(III)sulfate and water present in the compound on dividing their grams by their molar masses as:

$81.6gFe_2(SO_4)_3(\frac{1mol}{399.88g})$

= $0.204molFe_2(SO_4)_3$

$18.4gH_2O(\frac{1mol}{18.02g})$

= $1.02molH_2O$

Now, the next step is to calculate the mol ratio and for this we divide the moles of each by the least one of them means whose moles are less. Here, the moles of Iron(III)sulfate are less than moles of water. So, we divide the moles of each by 0.204.

$Fe_2(SO_4)_3=\frac{0.204}{0.204}$ = 1

$H_2O=\frac{1.02}{0.204}$ = 5

There is 1:5 mol ratio between Iron(III)sulfate and water. So, the formula of the hydrate is $Fe_2(SO_4)_3.5H_2O$ and the name of the hydrate is Iron(III)sulfate pentahydrate.

3 0

3 years ago