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Questions and Answers
What is the molarity of a solution containing 1.5 mol of NaCl dissolved in 0.500 L of solution?
What is the molarity of a solution containing 1.5 mol of NaCl dissolved in 0.500 L of solution?
How do you express the moles of solute when given a mass of 22.4 g of HCl?
How do you express the moles of solute when given a mass of 22.4 g of HCl?
What is the first step in calculating the molarity of a solution?
What is the first step in calculating the molarity of a solution?
If 42.23 g of NH4Cl is dissolved to make 500.0 mL of solution, what is necessary to calculate its molarity?
If 42.23 g of NH4Cl is dissolved to make 500.0 mL of solution, what is necessary to calculate its molarity?
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Why is the term 'aq' sometimes added after a solute in a solution?
Why is the term 'aq' sometimes added after a solute in a solution?
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Which conversion factor is essential for calculating the number of moles from mass for HCl?
Which conversion factor is essential for calculating the number of moles from mass for HCl?
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If you have a solution with a molarity of 0.394 M HCl, how many moles of HCl are in 1.56 L of solution?
If you have a solution with a molarity of 0.394 M HCl, how many moles of HCl are in 1.56 L of solution?
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Which of the following is a common misconception about molarity calculations?
Which of the following is a common misconception about molarity calculations?
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What is the molarity of a solution containing 53.50 g of NH4Cl in 0.5000 L of solution?
What is the molarity of a solution containing 53.50 g of NH4Cl in 0.5000 L of solution?
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How many moles of NaCl are present in 0.5000 L of a 4.69 M solution?
How many moles of NaCl are present in 0.5000 L of a 4.69 M solution?
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If 66.2 g of C6H12O6 is dissolved to make 235 mL of solution, what is its molarity?
If 66.2 g of C6H12O6 is dissolved to make 235 mL of solution, what is its molarity?
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Which of the following correctly describes the relationship of concentration and stoichiometry in a chemical reaction?
Which of the following correctly describes the relationship of concentration and stoichiometry in a chemical reaction?
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How would you describe the process of determining the moles of solute given its concentration and volume?
How would you describe the process of determining the moles of solute given its concentration and volume?
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What is the mass of solute needed to prepare 1.00 L of a 2.00 M NaCl solution?
What is the mass of solute needed to prepare 1.00 L of a 2.00 M NaCl solution?
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If 137 g of NaCl is dissolved in 500 mL, what is the concentration in mol/L?
If 137 g of NaCl is dissolved in 500 mL, what is the concentration in mol/L?
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Which factor is essential when using molarity as a conversion factor?
Which factor is essential when using molarity as a conversion factor?
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What is the mass of the solution when 25.0 g of sugar is dissolved in 100.0 g of water?
What is the mass of the solution when 25.0 g of sugar is dissolved in 100.0 g of water?
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How is percent by mass calculated in a solution?
How is percent by mass calculated in a solution?
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What is the mass/mass percent concentration of a saline solution with 36.5 g of NaCl in 355 g of solution?
What is the mass/mass percent concentration of a saline solution with 36.5 g of NaCl in 355 g of solution?
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To prepare a 5.00% NaCl solution with a total mass of 3000.0 g, what mass of NaCl is needed?
To prepare a 5.00% NaCl solution with a total mass of 3000.0 g, what mass of NaCl is needed?
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In a solution prepared using 15.8 g of dextrose in a total mass of 200.0 g, what is the mass/mass percent concentration?
In a solution prepared using 15.8 g of dextrose in a total mass of 200.0 g, what is the mass/mass percent concentration?
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If you need to express mass percent as a conversion factor, which of the following is correct?
If you need to express mass percent as a conversion factor, which of the following is correct?
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If a solution has a mass of 255 g and 25 g sugar dissolved in it, what would be the percent by mass of sugar?
If a solution has a mass of 255 g and 25 g sugar dissolved in it, what would be the percent by mass of sugar?
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When calculating the amount of solute needed for a specific concentration, what must be known?
When calculating the amount of solute needed for a specific concentration, what must be known?
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Flashcards
Mass percent concentration
Mass percent concentration
The mass of solute divided by the mass of solution, multiplied by 100%.
Mass of solution
Mass of solution
The total mass of solute and solvent in a solution. Units are grams.
Percent by mass calculation
Percent by mass calculation
Calculating the percentage of a solute in a solution by dividing the mass of the solute by the mass of the solution and multiplying by 100.
Conversion factor (mass percent)
Conversion factor (mass percent)
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Solute
Solute
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Solvent
Solvent
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Mass/Mass percent concentration
Mass/Mass percent concentration
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Calculating solute mass
Calculating solute mass
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Molarity
Molarity
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Molarity units
Molarity units
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Calculating Molarity
Calculating Molarity
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Converting mass to moles
Converting mass to moles
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Solution volume
Solution volume
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Volume of solution (in calculation)
Volume of solution (in calculation)
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Molarity (M)
Molarity (M)
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Moles of solute
Moles of solute
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Volume of solution
Volume of solution
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Concentration as Conversion Factor
Concentration as Conversion Factor
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Stoichiometry and Concentration
Stoichiometry and Concentration
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Solving for moles in a solution
Solving for moles in a solution
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Significant Figures in Calculations
Significant Figures in Calculations
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Study Notes
Chapter Overview
- Solutions are crucial in various chemical, biological, and industrial applications.
- Aqueous solutions (where substances dissolve in water) are a focus of this chapter.
- Solutions can involve all states (gas-gas, solid-solid, liquid-solid, liquid-liquid).
- This chapter primarily concentrates on aqueous solutions.
Tragedy in Cameroon - Lake Nyos
- In 1986, a gas cloud from Lake Nyos (Cameroon) killed over 1,700 people.
- The gas was primarily carbon dioxide, released after a lake overturn.
- The carbon dioxide was dissolved in the water and released into the atmosphere.
- The incident prompted investigations into other African lakes, specifically Lake Kivu.
Solutions - Homogeneous Mixtures
- The major component of a solution is the solvent.
- The minor component of a solution is the solute.
- The overall phase of a solution is identical to the solvent's phase.
- Examples:
- Salt water: solid NaCl in liquid water
- Air: gaseous O2 in gaseous N2
- Table 13.2.1 demonstrates various solution types with illustrations.
Like Dissolves Like
- Polar compounds dissolve polar compounds.
- Nonpolar compounds dissolve nonpolar compounds.
- Polar compounds do not dissolve in nonpolar compounds, and vice versa.
- This principle is summarized in Table 13.2.2.
- Intermolecular forces (London dispersion forces, dipole-dipole interactions, hydrogen bonding) determine solubility.
Solutions of Solids Dissolved in Water
- Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
- A saturated solution is one where the maximum amount of solute is dissolved.
- These solutions are saturated or unsaturated.
- The solubility of solids typically increases with temperature.
- Supersaturated solutions can hold more solute than their saturated counterparts.
- Table 13.3.1 lists the solubility of specific ionic compounds.
Electrolyte Solutions
- Electrolytes are compounds that yield ions in solution.
- Strong electrolytes dissociate nearly completely in solution.
- Weak electrolytes dissociate partially.
- Nonelectrolytes do not dissociate.
- Conductivity measurements can distinguish these types of solutions.
- Table 13.3.2 displays conductivity examples.
Solutions of Gases in Water
- Gas solubility typically decreases with increasing temperature.
- Gas solubility increases with increased pressure.
- Thermal pollution (e.g., hot water discharge from industries) can decrease the amount of dissolved oxygen in water, impacting aquatic life.
- This is described by Henry's law and Figure 13.4.1.
Specifying Solution Concentration - Mass Percent
- Mass percent (%m/m) = (mass of solute / mass of solution) * 100%
- Quantitative expressions for solution concentration.
- Allows measuring ratios of solute to solution.
Specifying Solution Concentration - Molarity
- Molarity (M) = (moles of solute / liters of solution).
- A crucial concentration expression for chemical calculations.
Solution Dilution
- M1V1 = M2V2.
- M1 & M2 represent initial and final concentrations, while V1 & V2 represent initial and final volumes.
- Diluting a solution involves adding more solvent without altering the amount of solute.
Solution Stoichiometry
- Using concentration to calculate reactant/product amounts in solution-based reactions.
Freezing Point Depression and Boiling Point Elevation
- Colligative properties depend on solute concentration.
- Freezing point of solutions is lower than the pure solvent.
- Boiling point of solutions is higher than the pure solvent.
- Formulas for freezing point depression and boiling point elevation involve molality and van't Hoff factor.
Osmosis
- Osmosis is the solvent's movement across a semipermeable membrane from a lower to a higher concentration of solute
- Osmotic pressure is directly related to solute concentration and is crucial in biological systems.
- Osmosis explains why IV fluids must be isotonic to prevent cell damage.
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Description
Explore the crucial role of solutions in chemical, biological, and industrial applications with a focus on aqueous solutions. This chapter delves into the composition of solutions, the impact of a historical tragedy in Cameroon due to gas release, and the fundamental concepts of homogeneous mixtures.
