Properties of Solutions
Types of Solutions
Ionization and Dissociation
Saturation
Miscellaneous
100
The relationship between the concentration of the chemicals and their colors and conductivity in solutions
What is they are positively correlated with one another means?
100
An example of a non-electrolyte.
What is a molecular compound
100
What is the crystalization equation for KNO3(s)?
K+(aq) + NO3- (aq)→ KNO3(s)
100
The mass of NaCl that can be dissolved in 100 mL of water at 80 degrees
What is 40 g?
100
The chemical species when Na2SO4 (s) is in water.
What is Na+ (aq), SO42-(aq), H2O(l) ?
200
What are the potential identities of solutions that are orange-yellow at high concentrations and pale yellow at low concentrations?
What is Iron (III)
200
The definition of a saturated solution.
What is a solution in which no more solute will dissolve at a specified temperature ? (maximum solute concentration)
200
What is the ionization equation of NaCl when the solution is saturated
What is NaCl (s) ⇌ Na+(aq) +Cl-(aq)
200
What chemical's solubility is the most impacted by changing temperature
What is KNO3?
200
What are the spectator compounds for the reaction between NaCl(aq) +I2(aq)
What is Na+(aq)?
300
What is blueish green when burnt and blue-green when it is high concentration at a solution?
What is Copper (I)?
300
The definition of dynamic equilibrium. When does Dynamic equilibrium happen?
What is two opposing processes occur at the same rate at the same time? What is saturated solutions?
300
The dissociation equation for K2SO4(s) in a saturated solution
What is K2SO4(s) ⇌ 2 K+(aq) + SO42- (aq)
No double arrow means no mark
300
When 70 g of KClO3 is added to 100 g of water at 60 degrees, how much KCO3 will remain solid, and how much of it will undergo dissolution?
What is 40 g? What is 30g?
300
What properties of water allow water to dissolve ionic compounds?
What is a Highly polar nature? What is Hydrogen bond?
400
List all observations expected for NaOH (aq) in water
What is the identity of a solution that conducts electricity, turns red litmus paper blue, blue litmus paper blue, and is yellow when burnt?
400
Explain the process used in making supersaturated solutions
What is heating up the solvent and increasing the solubility of the solvent, followed by adding the solute until it reaches saturation and rapid cooling.
400
Write the balanced skeleton equation and the total and net ionic equation for the reaction between solid copper and silver nitrate.
What is Cu(s) + 2AgNO3(aq) -> CuNO3(aq)+2Ag(s)
What is Cu(s) + Ag+(aq)+NO3-(aq) -> Cu2+(aq)+NO3-(aq)+Ag(s)
What is Cu(s) + Ag+(aq) -> Cu2+(aq)+Ag(s)
400
Is 110 g of KNO3 soluble at 500 mL of water at 30 degree?
What is yes?
400
Ammonium Nitrate and water are used in cold packs. These packs can be used in place of ice to keep food cool. Purpose a hypothesis to explain how a cold pack may work.
Endothermic reaction. The energy released during water ammonium/ water nitrate bond is less than ionic bond breaking between ammonium and nitrate
500
Three cups of solutions containing Cesium Hydroxide, Potassium Chloride, and Ammonium Hydroxide. List out a set of tests that can be used to separate the three chemicals what expectation for each test.
What is using ClO4- to separate Cs? What is a flame test?
500
What chemicals can be used in separate solutions containing Fe(NO3)2 and CuClO3? Write out the balanced skeleton equation, total ionic equations and net ionic equations
What is F-/Cl-/Br-/I-? Answer may vary.
500
Write the balanced skeleton equation and the total and net ionic equation for the reaction between (1.0 mol/L) NaIO3 and Iron (II) sulfate. What are the observations?
What is 2NaIO3(aq)+FeSO4(aq) ->Fe(IO3)2(s)+Na2SO4(aq)
What is 2Na++IO3-(aq)+Fe2+(aq)+SO42-(aq) ->Fe(IO3)2(s)+2Na++SO42-(aq)
What is IO3(aq)+Fe2+(aq) ->Fe(IO3)2(s)
What is the formation of the precipitate? Will the solution turn less lime green? Will the new solution be yellow when placed under the flame test?
500
What is the maximum amount of NH3 that can be soluble in 60mL of water? What is the optimal temperature to dissolve it?
What is 54g? What is 0 degree?
500
When metal strips were placed on Hydrochloric acid in a beaker, students could feel the beaker temperature increasing. Explain this phenomenon using terminologies such as bonds and energy.
The beaker temperature increasing implies reactions between Hydrochloric acid and metal strip releases energy. Therefore it is an exothermic reaction. Meaning energy used in bond breaking is less then energy released during bond formation.