Question
Asked Nov 6, 2019

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What is the pH of 275.0 mL of an aqueous solution containing 0.753 g of HCl?
 

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Step 1

The pH of a solution is used to specify the solution is acidic or basic in nature. The pH is a logarithmic and inversely proportional to concentration of hydrogen ion in the solution. At 25 oC  if the pH of the solution is less than 7 ,  then the  solution said to be  acidic in nature and if it is greater than 7 , then the solution is said to be basic  in nature.  If it is equal to 7, then the solution is said to be neutral.

Given:  

275.0 mL of an aqueous solution containing 0.753 g of HCl.

Therefore,  moles of the HCl:

Moles of the HCl = 0.753/36.45
0.0207
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Moles of the HCl = 0.753/36.45 0.0207

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Step 2

Concentration of the solution can be calculated as :

Concentration of the solution
(moles of HCl Volume of solution)x1000
(0.0207/275)1000
= 0.0753M
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Concentration of the solution (moles of HCl Volume of solution)x1000 (0.0207/275)1000 = 0.0753M

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Step 3

As the HCl is completely is io...

H 0.0753M
log [H
-log [0.753]
= 1.12
pH
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H 0.0753M log [H -log [0.753] = 1.12 pH

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