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Hatshy [7]
3 years ago
10

An aqueous solution of licl is 34.0 % licl. what mass of water is present in 250.0 g of the solution? (density of water is 1.00

g/ml) (solution contains only licl and water.)
Chemistry
2 answers:
adell [148]3 years ago
4 0
<span>If the aqueous solution is 34% Licl then it is 100 - 34% water = 66% From the calculation we've found out that it is 66% water. Then we need to find the weight from a 250 g solution. 66/100 * 250 = 165g Hence it is 165g</span>
Roman55 [17]3 years ago
3 0

<u>Answer:</u> Mass of water present in 250 g of solution is 165 g

<u>Explanation:</u>

A solution contains solute and solvent. A solute is defined as the substance which is present in smaller proportion and solvent is defined as the substance which is present in larger proportion.

We are given:

34 % (m/m) of LiCl

This means that 34 g of LiCl is present in 100 g of solution.

Mass of water in solution = 100 - 34 = 66 g

We need to find the mass of water present in 250 g of solution. By applying unitary method, we get:

In 100 g of solution, mass of water present in 66 g

So, in 250 g of solution, mass of water present will be = \frac{66}{100}\times 250=165g

Hence, mass of water present in 250 g of solution is 165 g

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maksim [4K]

Answer:

21.5 g.

Explanation:

Hello!

In this case, since the reaction between the given compounds is:

2Li_3P+Al_2O_3\rightarrow 3Li_2O+2AlP

We can see that according to the law of conservation of mass, which states that matter is neither created nor destroyed during a chemical reaction, the total mass of products equals the total mass of reactants based on the stoichiometric proportions; in such a way, we first need to compute the reacted moles of Li3P as shown below:

n_{Li_3P}^{reacted}=38gLi_3P*\frac{1molLi_3P}{51.8gLi_3P}=0.73molLi_3P

Now, the moles of Li3P consumed by 15 g of Al2O3:

n_{Li_3P}^{consumed \ by \ Al_2O_3}=15gAl_2O_3*\frac{1molAl_2O_3}{101.96gAl_2O_3} *\frac{2molLi_3P}{1molAl_2O_3} =0.29molLi_3P

Thus, we infer that just 0.29 moles of 0.73 react to form products; which means that the mass of formed products is:

m_{Li_2O}=0.29molLi_3P*\frac{3molLi_2O}{2molLi_3P} *\frac{29.88gLi_2O}{1molLi_2O} =13gLi_2O\\\\m_{AlP}=0.29molLi_3P*\frac{2molAlP}{2molLi_3P} *\frac{57.95gAlP}{1molAlP} =8.5gAlP

Therefore, the total mass of products is:

m_{products}=13g+8.5g\\\\m_{products}=21.5g

Which is not the same to the reactants (53 g) because there is an excess of Li₃P.

Best Regards!

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