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How many litres of water must be added to 1 litre of an aqueous solution of HCl with pH = 1 to create an aqueous solution with pH = 2?
- a)0.9 L
- b)2.0 L
- c)9.0 L
- d)0.1 L
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
How many litres of water must be added to 1 litre of an aqueous soluti...
Initial pH = 1, i.e. [H+] = 0.1 mole/litre
New pH = 2, i.e. [H+] = 0.01 mole/litre
In case of dilution: M1V1 = M2V2
0.1 1 = 0.01 V2
V2 = 10 litres
Volume of water added = 9 litres
New pH = 2, i.e. [H+] = 0.01 mole/litre
In case of dilution: M1V1 = M2V2
0.1
×
×
V2 = 10 litres
Volume of water added = 9 litres
Most Upvoted Answer
How many litres of water must be added to 1 litre of an aqueous soluti...
Given:
pH of the initial solution = 1
pH of the final solution = 2
To find:
How many litres of water must be added to 1 litre of the initial solution to create a solution with pH = 2?
Solution:
Step 1: Calculate the concentration of H+ ions in the initial solution.
pH is a measure of the concentration of H+ ions in a solution. The lower the pH value, the higher the concentration of H+ ions.
Since the pH of the initial solution is 1, the concentration of H+ ions can be calculated using the equation:
pH = -log[H+]
1 = -log[H+]
[H+] = 10^-1 M
The concentration of H+ ions in the initial solution is 10^-1 M.
Step 2: Calculate the concentration of H+ ions in the final solution.
Since the pH of the final solution is 2, the concentration of H+ ions can be calculated using the equation:
pH = -log[H+]
2 = -log[H+]
[H+] = 10^-2 M
The concentration of H+ ions in the final solution is 10^-2 M.
Step 3: Calculate the number of moles of H+ ions in the initial solution.
The number of moles of H+ ions can be calculated using the equation:
moles = concentration × volume
moles = (10^-1 M) × (1 L)
The number of moles of H+ ions in the initial solution is 10^-1 moles.
Step 4: Calculate the number of moles of H+ ions in the final solution.
The number of moles of H+ ions can be calculated using the equation:
moles = concentration × volume
moles = (10^-2 M) × (1 L + x)
The number of moles of H+ ions in the final solution is 10^-2 moles.
Step 5: Equate the number of moles of H+ ions in the initial and final solutions.
10^-1 moles = 10^-2 moles
1 = 0.1 + 0.01x
0.99 = 0.01x
x = 0.99 / 0.01
x = 99
Step 6: Calculate the volume of water that needs to be added.
The volume of water that needs to be added can be calculated using the equation:
volume = x L = 99 L
Conclusion:
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How many litres of water must be added to 1 litre of an aqueous solution of HCl with pH = 1 to create an aqueous solution with pH = 2?a)0.9 Lb)2.0 Lc)9.0 Ld)0.1 LCorrect answer is option 'C'. Can you explain this answer?
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