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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?
Correct answer is '9'. Can you explain this answer?
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How many litres of water must be added to 1 litre of an aqueous solut...
Calculating the Concentration of HCl in the Solution
To find the amount of water that needs to be added to the solution, we first need to calculate the concentration of HCl in the original solution.
The pH of a solution is a measure of its acidity. It is defined as the negative logarithm (base 10) of the concentration of hydronium ions ([H3O+]) in the solution.
The pH of the original solution is given as 1. This means that the concentration of hydronium ions in the solution is 10^(-1) M.
Calculating the Concentration of H3O+
The pH of the final solution is given as 2. This means that the concentration of hydronium ions in the final solution is 10^(-2) M.
Calculating the Concentration of OH-
The concentration of hydroxide ions ([OH-]) in a solution can be calculated using the equation Kw = [H3O+][OH-], where Kw is the ion product of water and is equal to 1.0 x 10^(-14) at 25°C.
Since we know the concentration of hydronium ions in the final solution is 10^(-2) M, we can rearrange the equation to solve for [OH-].
Kw = [H3O+][OH-]
1.0 x 10^(-14) = (10^(-2))([OH-])
[OH-] = (1.0 x 10^(-14))/(10^(-2))
[OH-] = 1.0 x 10^(-12) M
Calculating the pOH of the Final Solution
The pOH of a solution is the negative logarithm (base 10) of the concentration of hydroxide ions ([OH-]) in the solution.
pOH = -log([OH-])
pOH = -log(1.0 x 10^(-12))
pOH ≈ 12
Calculating the pH of the Final Solution
The pH and pOH of a solution are related by the equation pH + pOH = 14.
pH + 12 = 14
pH = 14 - 12
pH = 2
Determining the Volume of Water to be Added
To calculate the volume of water to be added, we need to determine the change in concentration of hydronium ions in the solution.
The change in concentration can be calculated using the formula:
Change in concentration = Initial concentration - Final concentration
Change in concentration = (10^(-1)) - (10^(-2))
Change in concentration = 10^(-1) - 10^(-2)
Change in concentration = 0.1 - 0.01
Change in concentration = 0.09 M
The volume of water to be added can be calculated using the formula:
Change in volume = (Change in concentration) * Initial volume
Change in volume = (0.09 M) * 1 L
Change in volume = 0.09 L
Therefore, 0.09 liters (or 90 mL) of water must be added to 1 liter of the original solution to create an aqueous solution with a pH of
To find the amount of water that needs to be added to the solution, we first need to calculate the concentration of HCl in the original solution.
The pH of a solution is a measure of its acidity. It is defined as the negative logarithm (base 10) of the concentration of hydronium ions ([H3O+]) in the solution.
The pH of the original solution is given as 1. This means that the concentration of hydronium ions in the solution is 10^(-1) M.
Calculating the Concentration of H3O+
The pH of the final solution is given as 2. This means that the concentration of hydronium ions in the final solution is 10^(-2) M.
Calculating the Concentration of OH-
The concentration of hydroxide ions ([OH-]) in a solution can be calculated using the equation Kw = [H3O+][OH-], where Kw is the ion product of water and is equal to 1.0 x 10^(-14) at 25°C.
Since we know the concentration of hydronium ions in the final solution is 10^(-2) M, we can rearrange the equation to solve for [OH-].
Kw = [H3O+][OH-]
1.0 x 10^(-14) = (10^(-2))([OH-])
[OH-] = (1.0 x 10^(-14))/(10^(-2))
[OH-] = 1.0 x 10^(-12) M
Calculating the pOH of the Final Solution
The pOH of a solution is the negative logarithm (base 10) of the concentration of hydroxide ions ([OH-]) in the solution.
pOH = -log([OH-])
pOH = -log(1.0 x 10^(-12))
pOH ≈ 12
Calculating the pH of the Final Solution
The pH and pOH of a solution are related by the equation pH + pOH = 14.
pH + 12 = 14
pH = 14 - 12
pH = 2
Determining the Volume of Water to be Added
To calculate the volume of water to be added, we need to determine the change in concentration of hydronium ions in the solution.
The change in concentration can be calculated using the formula:
Change in concentration = Initial concentration - Final concentration
Change in concentration = (10^(-1)) - (10^(-2))
Change in concentration = 10^(-1) - 10^(-2)
Change in concentration = 0.1 - 0.01
Change in concentration = 0.09 M
The volume of water to be added can be calculated using the formula:
Change in volume = (Change in concentration) * Initial volume
Change in volume = (0.09 M) * 1 L
Change in volume = 0.09 L
Therefore, 0.09 liters (or 90 mL) of water must be added to 1 liter of the original solution to create an aqueous solution with a pH of
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Community Answer
How many litres of water must be added to 1 litre of an aqueous solut...
Initial pH = 1, i.e. [H+] = 0.1 moles/litre
New pH = 2, i.e. [H+] = 0.01 moles/litre
In case of dilution: M1V1 = M2V2
0.1 x 1 = 0.01 x V2
V2 = 10 litres
Volume of water added = 9 litres
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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?Correct answer is '9'. Can you explain this answer?
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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?Correct answer is '9'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 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?Correct answer is '9'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 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?Correct answer is '9'. Can you explain this answer?.
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?Correct answer is '9'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 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?Correct answer is '9'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 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?Correct answer is '9'. Can you explain this answer?.
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