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Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL?
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Commercially available concentrated hydrochloric acid contains 38% H2S...
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Commercially available concentrated hydrochloric acid contains 38% H2S...
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a) Calculation of Molarity:
To calculate the molarity of the solution, we need to first find the molar mass of hydrochloric acid (HCl). The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl), which is approximately 36.46 g/mol.
Now, let's assume we have 100 g of the concentrated hydrochloric acid solution. Since it contains 38% HCl by mass, the mass of HCl in the solution would be 0.38 * 100 g = 38 g.
To calculate the number of moles of HCl, we divide the mass of HCl by its molar mass:
38 g / 36.46 g/mol ≈ 1.04 mol
Finally, to calculate the molarity, we divide the number of moles of HCl by the volume of the solution in liters:
Molarity (M) = Number of moles / Volume (in liters)
M = 1.04 mol / 1 L = 1.04 M
Therefore, the molarity of the solution is approximately 1.04 M.
b) Calculation of Volume:
To calculate the volume of concentrated H2SO4 required to make 1 liter of 0.10 M HCl, we need to use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of the concentrated H2SO4
V1 = volume of concentrated H2SO4 to be calculated
M2 = final molarity of HCl (0.10 M)
V2 = final volume of HCl (1 L)
Substituting the values into the equation, we have:
M1 * V1 = M2 * V2
V1 = (M2 * V2) / M1
V1 = (0.10 M * 1 L) / (1.04 M) ≈ 0.096 L
Therefore, approximately 0.096 liters (or 96 mL) of concentrated H2SO4 is required to make 1 liter of 0.10 M HCl.
a) Calculation of Molarity:
To calculate the molarity of the solution, we need to first find the molar mass of hydrochloric acid (HCl). The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl), which is approximately 36.46 g/mol.
Now, let's assume we have 100 g of the concentrated hydrochloric acid solution. Since it contains 38% HCl by mass, the mass of HCl in the solution would be 0.38 * 100 g = 38 g.
To calculate the number of moles of HCl, we divide the mass of HCl by its molar mass:
38 g / 36.46 g/mol ≈ 1.04 mol
Finally, to calculate the molarity, we divide the number of moles of HCl by the volume of the solution in liters:
Molarity (M) = Number of moles / Volume (in liters)
M = 1.04 mol / 1 L = 1.04 M
Therefore, the molarity of the solution is approximately 1.04 M.
b) Calculation of Volume:
To calculate the volume of concentrated H2SO4 required to make 1 liter of 0.10 M HCl, we need to use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of the concentrated H2SO4
V1 = volume of concentrated H2SO4 to be calculated
M2 = final molarity of HCl (0.10 M)
V2 = final volume of HCl (1 L)
Substituting the values into the equation, we have:
M1 * V1 = M2 * V2
V1 = (M2 * V2) / M1
V1 = (0.10 M * 1 L) / (1.04 M) ≈ 0.096 L
Therefore, approximately 0.096 liters (or 96 mL) of concentrated H2SO4 is required to make 1 liter of 0.10 M HCl.
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Commercially available concentrated hydrochloric acid contains 38% H2S...
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Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL?
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Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL?.
Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Commercially available concentrated hydrochloric acid contains 38% H2SO4 by mass A)what is the molarity of the solution (density of solution is equals to 1.3 gram centimetre cube) B)what volume of concentrated H2SO4 is required to make 1 litre of 0.10 M HCL?.
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