Solubility Concepts and Experiments

Which factor does NOT significantly influence the solubility of solid substances in a liquid?

How does the solubility of most solid substances change as temperature increases?

At approximately what temperature is the solubility of sodium sulfate ($Na_2SO_4$) at its maximum value according to the text?

What happens to the solubility of gases in liquids as the temperature increases?

In the experiment for determining the solubility of NaCl, what is the purpose of adding sodium chloride to water until undissolved salt remains?

During the NaCl solubility experiment, what is assumed when transferring 50 mL of the saturated solution to the evaporating dish?

In experiment 2.3, after evaporation, the mass of the dry sodium chloride is determined. What does the mass represent?

Which statement is correct regarding the solubility of NaCl?

What is the molality of a solution formed by dissolving 32.0 g of $CaCl_2$ in 271 g of water?

How many gram equivalents are present in 49 g of $H_2SO_4$?

What is the number of equivalents in 0.25 mol of $H_3PO_4$ when it is completely neutralized to $PO_4^{3-}$?

What is the normality of a solution containing 0.75 equivalents of solute in 250 mL of solution?

What mass of $Na_2CO_3$ is required to prepare 200 mL of a 0.2 N solution?

A 0.8 M solution of $H_3PO_4$ is prepared. Assuming complete dissociation, what is the normality of this solution?

If 1 L of a solution contains 4 equivalents of solute, what is its normality?

What is the 'z' value for $Al_2(SO_4)_3$ in a precipitation reaction?

If 0.2 moles of $H_3PO_4$ is converted to $H_2PO_4^-$, how many equivalents are present?

A solution has a normality of 0.48 N and contains $Al_2(SO_4)_3$. If the volume is 250 mL, what is the mass of $Al_2(SO_4)_3$?

Why are gas molecules in the gaseous state far apart?

What effect does increasing external heat have on the solubility of a gas in a liquid?

According to Henry’s Law, if the partial pressure of a gas above a solution increases, what happens to the solubility of the gas?

What is the unit of the Henry's law constant (k) when concentration is measured in molarity (M) and pressure in atmospheres (atm)?

Which of the following best describes the relationship in the equation $C_1/P_1 = C_2/P_2$?

Which gases do not generally follow Henry's law?

A carbonated beverage is bottled under pressure. What happens when the bottle's cap is removed?

If the solubility of nitrogen gas is $6.8 \times 10^{-4}$ mol/L at 1 atm, what would be its concentration at a partial pressure of 0.78 atm at the same temperature?

A solution of carbon dioxide ($CO_2$) has a concentration of 0.032 M at 3.0 atm. If the pressure is increased to 5.0 atm at the same temperature, what is the new concentration of $CO_2$?

According to Henry's Law, what happens to the concentration of a dissolved gas if the pressure above it is doubled?

Why does the solubility of solids or liquids in liquid solvents not change significantly with pressure?

What does the term 'molarity' represent?

What must be determined experimentally for each combination of gas, solvent, and temperature when applying Henry’s law?

If the temperature of a gas-liquid solution increases, what initially happens to the solubility of the gas?

Which of the following actions will not increase the solubility of a gas in a liquid?

What is the mass percentage of a solution prepared by dissolving 25 g of salt in 225 g of water?

A solution is made by mixing 40 mL of ethanol with 160 mL of water. What is the volume percent of ethanol in the solution?

If a solution contains 5 mg of a pollutant in 2 kg of water, what is the concentration of the pollutant in ppm?

A solution has a concentration of 8 ppm. If the solution is aqueous, what does this concentration mean in mg/L?

What does a 75% (v/v) solution of glycerol in water mean?

A solution of sodium chloride (NaCl) in water is prepared. The mole fraction of NaCl is 0.30. What is the mole fraction of water?

What is the mass per cent of a solution if 15.0 g of a solute is dissolved in 135 g of water?

A 100 mL solution contains 5 g of solute. What is the concentration in % (w/v)?

If a water sample contains 3.0 ppb of a contaminant, what does this mean in terms of mass ratio?

What is the volume percent of a solution if 30 mL of a solute is diluted with 120 mL of solvent?

How would you make a 25% (w/w) solution using 50 grams of a solute?

If a solution contains 50 ppm of a metal ion, and the solution's volume is 2 liters, approximately how many mg of the metal ion are present?

A solution is made by dissolving 12g of solid in water to make 300 mL of final volume. What is the % (w/v) of the solution?

Which scenario requires the use of parts per million (ppm) or parts per billion (ppb)?

If a solution contains 0.05 moles of solute and 0.45 moles of solvent, what is the mole fraction of the solute?

A solution contains 0.25 moles of solute and 2.5 moles of solvent. What is the mole fraction of the solute?

What is the mole percent of a solution containing 1 mole of solute and 3 moles of solvent?

If 8 grams of a solute with a molar mass of 40 g/mol is dissolved in enough solvent to make 200 mL of solution, what is the molarity of the solution?

Which of the following is NOT a drawback of using molarity as a measure of concentration in precise work?

How many moles of NaCl are needed to prepare 500 mL of a 0.25 M solution?

Which concentration unit is defined as the number of moles of solute per kilogram of solvent?

What is the molality of a solution prepared by dissolving 18 g of glucose (C6H12O6) in 200 g of water? (Molar mass of glucose = 180 g/mol)

Which of the following remains constant with changes in temperature?

What information is required to calculate the normality of a solution?

If a solution has a normality of 2 N, how many gram equivalents of solute are present in 500 mL of the solution?

What does 'z' represent in the formula: equivalent weight = molar mass / z

To prepare 1 liter of a 0.5 M solution of a substance with a molar mass of 100 g/mol, how many grams of the substance are required?

A 300 g solution contains 30 g of solute, what is the mass percent of the solute?

Which of the following concentration units is most affected by changes in temperature?

If 20g of a substance with a molar mass of 50g/mol is dissolved in 500g of solvent, what is the molality of the solution? (in mol/kg)