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AnnZ [28]
3 years ago
14

Determine the amount of water that must be added to a 2-litre solution of sulphuric acid to dilute it from a pH of 2.7 to a pH o

f 3.
Chemistry
1 answer:
Ksivusya [100]3 years ago
4 0

Answer:

Volume of water added = 2.0 L

Explanation:

Initial pH of the solution = 2.7

[H^+] concentration in 2 L solution of sulfuric acid,

pH = -log[H^+]

[H^+] = 10^{-pH}\ M

[H^+] = 10^{-2.7} = 0.001995\ M = 0.002\ M

Final pH of the solution = 3

Final [H^+] concentration of sulfuric acid,

[H^+] = 10^{-pH}\ M

[H^+] = 10^{-3} = 0.001\ M

Now,

M_1V_1=M_2V_2

0.002 \times 2.0 = 0.001 \times V_2

V_2 = \frac{0.002 \times 2.0}{0.001} = 4.00\ L

Volume added = Final volume - Initial volume

                        = 4.0 - 2.0 = 2.0 L

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Explanation:

Given parameters:

T1 = 27°C

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Unknown:

P2 = ?

Solution:

Using a derivative of the combined gas law where we assume that the gas has a constant volume, we can solve for the unknown.

 At constant volume:

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  Take the given temperature to K

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T2 = 127 + 273  = 400K

 Input the variables:

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  P2 = 135.1‬kPa

learn more:

Boyle's law brainly.com/question/8928288

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Then you divide the moles of Ar by the total number of moles: 
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