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swat32
3 years ago
13

Choose the aqueous solution that has the highest boiling point.These are all solutions of nonvolatile solutes and you shouldassu

me ideal van't Hoff factors where applicable.
a. 0.100 m NaNO3
b. 0.100m Li2SO4
c. 0.200m C3H8O3
d. 0.060m Na3PO4
Chemistry
1 answer:
lesya [120]3 years ago
4 0

<u>Answer:</u> The correct answer is Option b.

<u>Explanation:</u>

The expression of elevation in boiling point is given as:

\Delta T_b=i\times k_b\times m

where,

\Delta T_b = Elevation in boiling point

i = Van't Hoff factor  

T_b = change in boiling point

k_b = boiling point constant

m = molality

For the given options:

<u>Option 1:</u>  0.100 m NaNO_3

Value of i = 2

So, molal concentration will be = (0.100)\times 2=0.200m

<u>Option 2:</u>  0.100 m Li_2SO_4

Value of i = 3

So, molal concentration will be = (0.100)\times 3=0.300m

<u>Option 3:</u>  0.200 m C_3H_8O_3

Value of i = 1  (for non-electrolytes)

So, molal concentration will be = (0.200)\times 1=0.200m

<u>Option 4:</u>  0.060 m Na_3PO_4

Value of i = 4

So, molal concentration will be = (0.060)\times 4=0.24m

As, the molal concentration of Li_2SO_4 is the highest, so its boiling point will be the highest.

Thus, the order of increasing boiling points follows:

NaNO_3=C_3H_8O_3

Hence, the correct answer is Option b.

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Answer : The enthalpy of neutralization is, 56.012 kJ/mole

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First we have to calculate the moles of HCl and NaOH.

\text{Moles of HCl}=\text{Concentration of HCl}\times \text{Volume of solution}=0.400mole/L\times 0.200L=0.08mol

\text{Moles of NaOH}=\text{Concentration of NaOH}\times \text{Volume of solution}=0.400mole/L\times 0.200L=0.08mol

The balanced chemical reaction will be,

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From the balanced reaction we conclude that,

As, 1 mole of HCl neutralizes by 1 mole of NaOH

So, 0.08 mole of HCl neutralizes by 0.08 mole of NaOH

Thus, the number of neutralized moles = 0.08 mole

Now we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water = 200mL+200L=400mL

\text{Mass of water}=\text{Density of water}\times \text{Volume of water}=1g/ml\times 400mL=400g

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q=m\times c\times (T_{final}-T_{initial})

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q = heat absorbed = ?

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T_{final} = final temperature of water = 27.78^oC=273+25.10=300.78K

T_{initial} = initial temperature of metal = 25.10^oC=273+27.78=298.1K

Now put all the given values in the above formula, we get:

q=400g\times 4.18J/g^oC\times (300.78-298.1)K

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n = number of moles used in neutralization = 0.08 mole

\Delta H=\frac{-4480.96J}{0.08mole}=-56012J/mole=-56.012kJ/mol

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of neutralization is, 56.012 kJ/mole

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