Enter your answer in the provided box. What is the pH of 275.0 mL of an aqueous solution containing 0.753 g of HCl?
Enter your answer in the provided box.
What is the pH of 275.0 mL of an aqueous solution containing 0.753 g of HCl?
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:
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Moles of the HCl = 0.753/36.45 0.0207
Concentration of the solution can be calculated as :
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Concentration of the solution (moles of HCl Volume of solution)x1000 (0.0207/275)1000 = 0.0753M
As the HCl is completely is io...
![H 0.0753M
log [H
-log [0.753]
= 1.12
pH](https://prod-qna-question-images.s3.amazonaws.com/qna-images/answer/4fa31e93-8540-4917-acdc-4379a0e22c77/12c70bbf-14af-4df1-8c16-bf24876f4a80/dwiw8x.png)
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H 0.0753M log [H -log [0.753] = 1.12 pH
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