Chapter 8: Problem 280
Calculate the weight in grams of sulfuric acid in \(2.00\) liters of \(0.100\) molar solution. (MW of \(\mathrm{H}_{2} \mathrm{SO}_{4}=98.1 .\) )
Short Answer
Expert verified
There are 19.62 grams of sulfuric acid (H₂SO₄) in 2.00 liters of 0.100 molar solution.
Step by step solution
01
Write down the given information
We have a 0.100 molar (M) solution of H₂SO₄ with a volume of 2.00 liters, and we know that the molecular weight of H₂SO₄ is 98.1 g/mol.
02
Use the molarity formula to find the moles of H₂SO₄ present in 2.00 liters of the solution
We can use the formula \(molarity = \frac{moles}{volume}\) to determine the moles of H₂SO₄ present in the solution. Rearrange the formula for moles:
\(moles = molarity \times volume\)
Now, we can plug in the values:
\(moles = 0.100M \times 2.00L = 0.200\, moles\)
There are 0.200 moles of H₂SO₄ present in 2.00 liters of the solution.
03
Use the molecular weight (MW) of H₂SO₄ to convert moles to grams
We know that 1 mole of H₂SO₄ weighs 98.1 grams. Using this, we can determine the weight of 0.200 moles of H₂SO₄ by using the conversion factor:
\(grams\, of\, H_{2}SO_{4} = moles\, of\, H_{2}SO_{4} \times \frac{98.1\, grams\, of\, H_{2}SO_{4}}{1\, mole\, of\, H_{2}SO_{4}}\)
Plug in the values:
\(grams\, of\, H_{2}SO_{4} = 0.200\, moles \times \frac{98.1\, g}{1\, mol} = 19.62\, grams\)
04
Write down the final answer
There are 19.62 grams of sulfuric acid (H₂SO₄) in 2.00 liters of 0.100 molar solution.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Molar Solution
Short Description:
A molar solution is one that expresses concentration, specifically, how many moles of a solute are present in one liter of solution. The concept of molar solution is a fundamental aspect of chemistry, particularly useful when mixing solutions with precise concentrations.
Understanding Molar Solutions:
When dealing with chemical solutions, knowing the exact concentration is crucial for predicting reactions and calculating yields. One common unit of concentration is molarity, which is measured in moles per liter (mol/L or M). For example, if a solution is labeled as '0.100 M H₂SO₄', it means that in every liter of this solution, 0.100 moles of sulfuric acid are dissolved.
Calculating the Amount:
To determine the amount of solute in a certain volume of molar solution, multiply the molarity by the volume in liters. This gives the number of moles of the solute present, which can subsequently be converted to grams using the molecular weight. It's a simple yet powerful way to scale reactions or to prepare a variety of solutions in laboratory settings.
A molar solution is one that expresses concentration, specifically, how many moles of a solute are present in one liter of solution. The concept of molar solution is a fundamental aspect of chemistry, particularly useful when mixing solutions with precise concentrations.
Understanding Molar Solutions:
When dealing with chemical solutions, knowing the exact concentration is crucial for predicting reactions and calculating yields. One common unit of concentration is molarity, which is measured in moles per liter (mol/L or M). For example, if a solution is labeled as '0.100 M H₂SO₄', it means that in every liter of this solution, 0.100 moles of sulfuric acid are dissolved.
Calculating the Amount:
To determine the amount of solute in a certain volume of molar solution, multiply the molarity by the volume in liters. This gives the number of moles of the solute present, which can subsequently be converted to grams using the molecular weight. It's a simple yet powerful way to scale reactions or to prepare a variety of solutions in laboratory settings.
Molecular Weight
Short Description:
Molecular weight (MW), also known as molecular mass, is defined as the mass of one mole of a substance. It is typically expressed in units of grams per mole (g/mol). Understanding the molecular weight of compounds is imperative for molarity calculations and converting moles to grams.
Importance in Calculations:
The molecular weight serves as the conversion factor needed for transitioning between the mass of a compound and the number of moles. With the molecular weight, scientists can easily relate a compound's mass in grams to the amount of substance in terms of moles.
How to Determine Molecular Weight:
Molecular weight can be calculated by summing the atomic weights of all the atoms present in a molecule. For instance, the molecular weight of sulfuric acid (H₂SO₄) is calculated by adding the atomic weights of two hydrogen atoms, one sulfur atom, and four oxygen atoms, which totals to 98.1 g/mol.
Molecular weight (MW), also known as molecular mass, is defined as the mass of one mole of a substance. It is typically expressed in units of grams per mole (g/mol). Understanding the molecular weight of compounds is imperative for molarity calculations and converting moles to grams.
Importance in Calculations:
The molecular weight serves as the conversion factor needed for transitioning between the mass of a compound and the number of moles. With the molecular weight, scientists can easily relate a compound's mass in grams to the amount of substance in terms of moles.
How to Determine Molecular Weight:
Molecular weight can be calculated by summing the atomic weights of all the atoms present in a molecule. For instance, the molecular weight of sulfuric acid (H₂SO₄) is calculated by adding the atomic weights of two hydrogen atoms, one sulfur atom, and four oxygen atoms, which totals to 98.1 g/mol.
Convert Moles to Grams
Short Description:
The process of converting moles to grams is a fundamental skill in chemistry, allowing the measurement of substances in a quantifiable and usable form.
The Conversion Process:
To convert moles of a substance to grams, multiply the number of moles by the molecular weight of the substance. This is based on the definition of a mole, which is the amount of substance that contains as many entities (atoms, molecules, or ions) as there are atoms in 12 grams of pure carbon-12.
Practical Example:
Using the example from the exercise, 0.200 moles of sulfuric acid (H₂SO₄) can be converted to grams by multiplying it by the molecular weight (98.1 g/mol):\begin{align*}\(0.200\text{ moles} \times 98.1\frac{g}{mol} = 19.62\text{ grams}\)\text{This calculation results in 19.62 grams of sulfuric acid.}\text{Such conversions are vital for various applications, from preparing solutions to measuring reactants for reactions.}\text{Remember that accurate molecular weights and correct conversion are vital for these calculations to ensure the precision of the results.}\text{By mastering this conversion process, students can adeptly manipulate and measure chemicals in both academic and professional laboratory settings.}\text{This comprehension also paves the way for advanced topics like stoichiometry and chemical equilibrium.}\text{Thus, learning to confidently convert moles to grams is not just a single skill but a stepping stone to further understanding in chemistry.}\text{Moreover, it empowers students to carry out experiments and calculations with efficacy and accuracy.}\text{Exercise improvement advice: Emphasize the unity between these concepts, showing how molar solutions relate directly to the molecular weight of a compound for converting moles to grams. This connection is key to solving many problems in chemistry.}\text{Use visuals or interactive elements when explaining these concepts to students, as it can significantly improve comprehension and retention.}\text{Providing practical examples with real-world applications will also enable students to grasp the importance and utility of these concepts beyond the textbook.}\text{Finally, encourage students to practice these calculations with diverse compounds to reinforce their understanding and build confidence in these essential chemistry skills.}\text{In summary, emphasize the interlinked nature of molar solutions, molecular weight, and the conversion of moles to grams, using varied teaching methods and practical examples to make these fundamental concepts relatable and understandable for students.}\text{By doing so, students will attain a solid foundation in chemical calculations and be better prepared for more advanced study.}
The process of converting moles to grams is a fundamental skill in chemistry, allowing the measurement of substances in a quantifiable and usable form.
The Conversion Process:
To convert moles of a substance to grams, multiply the number of moles by the molecular weight of the substance. This is based on the definition of a mole, which is the amount of substance that contains as many entities (atoms, molecules, or ions) as there are atoms in 12 grams of pure carbon-12.
Practical Example:
Using the example from the exercise, 0.200 moles of sulfuric acid (H₂SO₄) can be converted to grams by multiplying it by the molecular weight (98.1 g/mol):\begin{align*}\(0.200\text{ moles} \times 98.1\frac{g}{mol} = 19.62\text{ grams}\)\text{This calculation results in 19.62 grams of sulfuric acid.}\text{Such conversions are vital for various applications, from preparing solutions to measuring reactants for reactions.}\text{Remember that accurate molecular weights and correct conversion are vital for these calculations to ensure the precision of the results.}\text{By mastering this conversion process, students can adeptly manipulate and measure chemicals in both academic and professional laboratory settings.}\text{This comprehension also paves the way for advanced topics like stoichiometry and chemical equilibrium.}\text{Thus, learning to confidently convert moles to grams is not just a single skill but a stepping stone to further understanding in chemistry.}\text{Moreover, it empowers students to carry out experiments and calculations with efficacy and accuracy.}\text{Exercise improvement advice: Emphasize the unity between these concepts, showing how molar solutions relate directly to the molecular weight of a compound for converting moles to grams. This connection is key to solving many problems in chemistry.}\text{Use visuals or interactive elements when explaining these concepts to students, as it can significantly improve comprehension and retention.}\text{Providing practical examples with real-world applications will also enable students to grasp the importance and utility of these concepts beyond the textbook.}\text{Finally, encourage students to practice these calculations with diverse compounds to reinforce their understanding and build confidence in these essential chemistry skills.}\text{In summary, emphasize the interlinked nature of molar solutions, molecular weight, and the conversion of moles to grams, using varied teaching methods and practical examples to make these fundamental concepts relatable and understandable for students.}\text{By doing so, students will attain a solid foundation in chemical calculations and be better prepared for more advanced study.}
