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Based on Table G, which compound has the greatest solubility in 100. grams of water at 10.°C?*
Based on Table G, which compound is less soluble in water as the temperature increases from 0°C to 100°C?*
Based on Table G, which solute sample in 100.g of water at 40.°C can produce a solution equilibrium in a closed system?*
Base your answers to questions 4 on the information below.
Ammonium chloride is dissolved in water to form a 0.10 M NH4Cl(aq) solution. This dissolving process is represented by the equation below.
Determine the minimum mass of NH4Cl(s) required to produce a saturated solution in 100. grams of water at 40.°C.*
Base your answers to questions 5 on the information below and on your knowledge of chemistry.
The compounds KNO3 and NaNO3 are soluble in water.
Compare the boiling point of a NaNO3 solution at standard pressure to the boiling point of water at standard pressure.*
Base your answers to questions 6 on the information below and on your knowledge of chemistry.
Baking soda, NaHCO3, can be commercially produced during a series of chemical reactions called the Solvay process. In this process, NH3(aq), NaCl(aq), and other chemicals are used to produce NaHCO3(s) and NH4Cl(aq).
To reduce production costs, NH3(aq) is recovered from NH4Cl(aq) through a different series of reactions. This series of reactions can be summarized by the overall reaction represented by the unbalanced equation below.
NH4Cl(aq) + CaO(s) → NH3(aq) + H2O(ℓ) + CaCl2(aq)
Determine the mass of NH4Cl that must be dissolved in 100. grams of H2O to produce a saturated solution at 70.°C.*
Base your answers to questions 7 on the information below and on your knowledge of chemistry.
In a laboratory investigation, a student is given a sample that is a mixture of 3.0 grams of NaCl(s) and 4.0 grams of sand, which is mostly SiO2(s). The purpose of the investigation is to separate and recover the compounds in the sample. In the first step, the student places the sample in a 250-mL flask. Then, 50. grams of distilled water are added to the flask, and the contents are thoroughly stirred. The mixture in the flask is then filtered, using the equipment represented by the diagram below.
Based on Table G, state evidence that all of the NaCl(s) in the flask would dissolve in the distilled water at 20.°C.*
What is the mass of KNO3(s) that must dissolve in 100. grams of water to form a saturated solution at 50.°C?*
Determine the mass of KNO3 that dissolves in 100. grams of water at 40.°C to produce a saturated solution.*
Base your answers to questions 10 on the information below and on your knowledge of chemistry.
A solution is made by dissolving 70.0 grams of KNO3(s) in 100. grams of water at 50.°C and standard pressure.
Determine the number of additional grams of KNO3 that must dissolve to make this solution saturated.*
Using Table G, determine the minimum mass of NaCl that must be dissolved in 200. grams of water to produce a saturated solution at 90.°C.*
Base your answers to questions 12 on the information below and on your knowledge of chemistry.
A saturated solution of sulfur dioxide is prepared by dissolving SO2(g) in 100. g of water at 10.°C and standard pressure.
Based on Table G, state the general relationship between solubility and temperature of an aqueous SO2 solution at standard pressure.*
Base your answers to questions 13 on the information below and on your knowledge of chemistry.
A 100.-gram sample of liquid water is heated from 20.0°C to 50.0°C. Enough KClO3(s) is dissolved in the sample of water at 50.0°C to form a saturated solution.
Based on Table G, determine the mass of KClO3(s) that must dissolve to make a saturated solution in 100. g of H2O at 50.0°C.*
Base your answers to questions 14 on the information below and on your knowledge of chemistry.
A sample of normal rainwater has a pH value of 5.6 due to dissolved carbon dioxide gas from the atmosphere. Acid rain is formed when other gases, such as sulfur dioxide, dissolve in rainwater, which can result in lake water with a pH value of 4.6. The equation below represents the reaction of water with SO2(g).
Based on Table G, describe what happens to the solubility of SO2(g) as the temperature increases from 10.°C to 30.°C at standard pressure. [1]*
