Baby
What is the difference between a solute and a solvent in a salt-water solution?
The solute is the salt (the substance being dissolved), and the solvent is the water (the substance doing the dissolving).
Which of the following is a homogeneous mixture: sand in water, oil in vinegar, or sugar dissolved in water?
Sugar dissolved in water.
Define "saturated solution" in your own words.
A saturated solution is a solution that contains the maximum amount of solute that can be dissolved in a given quantity of solvent at a specific temperature.
Explain why "like dissolves like" is the rule of thumb for solubility.
Substances with similar intermolecular forces (polar-polar or nonpolar-nonpolar) are more likely to form a solution because the energy released by forming new solute-solvent attractions offsets the energy required to break existing solute-solute and solvent-solvent bonds.
How does Henry's Law relate to the solubility of gases in liquids?
Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid (S=kPS=kP).
If a solution contains 10g of salt in 100mL of water, what is the concentration in g/mLg/mL?
0.1g/mL
Define Molarity (MM).
Molarity is the number of moles of solute per liter of solution.
Calculate the Molarity of a solution containing 0.50.5 moles of NaCl in 2.02.0 liters of water.
0.25M
If you have 500 mL500mL of a 2.0 M2.0M stock solution, how much water must you add to dilute it to a 0.5 M0.5M solution?
1500mL of water must be added (total volume becomes 2000 mL2000mL).
What is the molality (mm) of a solution made by dissolving 20 g20g of NaOH (molar mass 40 g/mol40g/mol) in 500 g500g of water?
1.0m
Does stirring a solution make it dissolve faster or slower?
Faster.
Does heating water usually increase or decrease the solubility of a solid like sugar?
Increase.
What happens to the solubility of a gas (like CO2CO2) in soda when the temperature increases?
The solubility decreases.
Explain the role of surface area in the rate of dissolution.
Increasing surface area (e.g., crushing a sugar cube) increases the rate of dissolution because more solute particles are exposed to the solvent at the same time.
Why does the solubility of gases decrease when a liquid is heated, while most solids become more soluble?
Dissolving a gas is usually an exothermic process (ΔH<0ΔH<0), so adding heat shifts the equilibrium toward the gas phase. Dissolving a solid is usually endothermic (ΔH>0ΔH>0), so adding heat shifts the equilibrium toward the dissolved state.
What is a colligative property?
A property of a solution that depends only on the number of solute particles, not on their identity.
Does adding salt to water increase or decrease its freezing point?
Decrease (Freezing point depression).
Why does salt water boil at a higher temperature than pure water?
Boiling point elevation: the solute particles reduce the vapor pressure of the solvent, requiring more energy (heat) to make the vapor pressure equal the atmospheric pressure.
(or you could just say that more stuff needs more energy/fire to boil/burn)🤷
Which solution would have a lower freezing point: 1.0 M NaCl1.0MNaCl or 1.0 M CaCl21.0MCaCl2?
1.0MCaCl2.
Calculate the freezing point depression of a solution containing 0.1 mol0.1mol of glucose in 100 g100g of water (Kf=1.86 ∘C/mKf=1.86∘C/m).
−1.86∘C
Looking at a solubility curve graph, what does the x-axis represent?
Temperature
If a point on a solubility graph is located exactly on the curve line, is the solution saturated or unsaturated?
Saturated.
If a point is located below the solubility curve line, is the solution saturated, unsaturated, or supersaturated?
Unsaturated.
Describe how you could create a supersaturated solution.
Dissolve a large amount of solute at a high temperature, then slowly cool the solution undisturbed.
How does a solubility curve for a gas differ from a solid on a standard solubility graph?
The solubility curve for a gas slopes downward as temperature increases, whereas the curve for most solids slopes upward.