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What is the molarity of a solution containing 5 g of NaOH in 450 mL?
What is the molarity of a solution containing 5 g of NaOH in 450 mL?
- 0.125 M
- 0.567 M
- 0.450 M
- 0.278 M (correct)
How is molality defined?
How is molality defined?
- Mass of solute per volume of solution
- Moles of solute per liter of solution
- Volume of solute per mass of solvent
- Moles of solute per kilogram of solvent (correct)
Why is molarity considered a function of temperature?
Why is molarity considered a function of temperature?
- It varies with the mass of the solvent
- Volume changes with temperature (correct)
- It depends on the mass of the solute
- It is independent of the solution's composition
What mass of KCl corresponds to a 1.00 mol kg solution?
What mass of KCl corresponds to a 1.00 mol kg solution?
What is the molality of 2.5 g of ethanoic acid in 75 g of benzene?
What is the molality of 2.5 g of ethanoic acid in 75 g of benzene?
How does total vapor pressure over a solution relate to the mole fraction of one component?
How does total vapor pressure over a solution relate to the mole fraction of one component?
What happens to the total vapor pressure over the solution as the mole fraction of component 2 increases?
What happens to the total vapor pressure over the solution as the mole fraction of component 2 increases?
Which statement correctly describes the graphical representation of vapor pressure vs. mole fraction?
Which statement correctly describes the graphical representation of vapor pressure vs. mole fraction?
What could be concluded if the total vapor pressure has a maximum value of $p_2$?
What could be concluded if the total vapor pressure has a maximum value of $p_2$?
In the context of the solution described, what is indicated by a minimum value of total vapor pressure at $p_1$?
In the context of the solution described, what is indicated by a minimum value of total vapor pressure at $p_1$?
What does Dalton conclude about the concentration of dissolved gas in a solution?
What does Dalton conclude about the concentration of dissolved gas in a solution?
In the equation p = KH x, what does KH represent?
In the equation p = KH x, what does KH represent?
What relationship does Henry's law illustrate?
What relationship does Henry's law illustrate?
Why do different gases have different KH values at the same temperature?
Why do different gases have different KH values at the same temperature?
If you were to plot partial pressure versus mole fraction of a gas in solution, what type of graph would you expect?
If you were to plot partial pressure versus mole fraction of a gas in solution, what type of graph would you expect?
What causes the decrease in the vapour pressure of a solution compared to that of the pure solvent?
What causes the decrease in the vapour pressure of a solution compared to that of the pure solvent?
How does the addition of non-volatile solutes, like sucrose or urea, affect the vapour pressure of water?
How does the addition of non-volatile solutes, like sucrose or urea, affect the vapour pressure of water?
According to Raoult's law, the partial vapour pressure of each component in a binary solution is proportional to what?
According to Raoult's law, the partial vapour pressure of each component in a binary solution is proportional to what?
What is the relationship between the amount of non-volatile solute and the decrease in vapour pressure?
What is the relationship between the amount of non-volatile solute and the decrease in vapour pressure?
Which statement accurately describes the effect of solute on the solvent's vapour pressure?
Which statement accurately describes the effect of solute on the solvent's vapour pressure?
What does it indicate when the enthalpy of mixing of two pure components is zero?
What does it indicate when the enthalpy of mixing of two pure components is zero?
What characterizes a solution that behaves ideally?
What characterizes a solution that behaves ideally?
Which of the following pairs of substances is likely to form an ideal solution?
Which of the following pairs of substances is likely to form an ideal solution?
What is the result of a non-ideal solution exhibiting positive deviation from Raoult’s law?
What is the result of a non-ideal solution exhibiting positive deviation from Raoult’s law?
In terms of volume, what happens when two ideal components are mixed?
In terms of volume, what happens when two ideal components are mixed?
Which condition defines a non-ideal solution?
Which condition defines a non-ideal solution?
What kind of deviation occurs when the vapor pressure of a solution is lower than predicted?
What kind of deviation occurs when the vapor pressure of a solution is lower than predicted?
Which of the following statements is true regarding ideal solutions?
Which of the following statements is true regarding ideal solutions?
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Study Notes
Molarity Calculation
- Molarity (M) is calculated as moles of solute per liter of solution.
- For NaOH, with a mass of 5 g, the number of moles is 0.125 mol using the molar mass of 40 g/mol.
- The volume of the solution is converted from 450 mL to 0.450 L.
- Molarity of the NaOH solution is calculated as 0.125 mol × 1000 mL/L ÷ 450 mL, yielding 0.278 M.
Molality Definition
- Molality (m) is defined as the number of moles of solute per kilogram of solvent.
- A 1.00 mol/kg solution of KCl indicates that 1 mol (74.5 g) of KCl is dissolved in 1 kg of water.
- Molality is independent of temperature, unlike molarity, which is temperature-dependent due to volume change.
Example of Molality Calculation
- For 2.5 g of ethanoic acid (CH3COOH) in 75 g of benzene, the calculation of molality involves determining moles of ethanoic acid and converting the mass of benzene to kg (0.075 kg).
Henry's Law
- Henry’s Law states that the partial pressure of a gas in vapor phase is proportional to its mole fraction in solution, expressed as p = KH x, where KH is the Henry’s law constant.
- The relationship between solubility of gas and partial pressure highlights that different gases have distinct KH values at a given temperature.
Vapor Pressure and Mole Fractions
- Total vapor pressure over a solution is influenced by the mole fraction of components.
- It varies linearly, indicating that as the mole fraction of one component increases, the vapor pressure changes correspondingly.
- The minimal and maximal vapor pressures in a binary solution depend on the volatility of the components.
Raoult's Law
- Raoult’s Law states that the partial vapor pressure of each volatile component is directly proportional to its mole fraction in the solution.
- For ideal solutions, the mixing process leads to no heat absorption or evolution (ΔmixH = 0) and the volume of mixing is negligible (ΔmixV = 0).
- Ideal behavior is observed when intermolecular forces are consistent among A-A, B-B, and A-B types.
Non-Ideal Solutions
- Non-ideal solutions deviate from Raoult’s law under certain concentrations, exhibiting either positive or negative deviations.
- Positive deviation results in higher vapor pressure than predicted by Raoult's law, while negative deviation results in lower vapor pressure.
- Vapor pressure vs. mole fraction plots illustrate these deviations for non-ideal solutions.
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