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WorksheetsTEKS 10.B
Total questions: 22
Worksheet time: 1hrs 6mins
10B. (#1)
Precipitates are insoluble substances that result from reactions between aqueous solutions. Two solubility rules are shown.
Solubility Rules;
All nitrates are soluble. All halides are soluble except for Ag+, Pb+2 and Hg+22
Which compounds form a yellow precipitate in the reactdion:
Pb(NO3 )2 + KI --> PbI2 + KNO3 ?
Pb(NO3 )2
KI
PbI2
KNO3
10B. (#2)
Which mixture can be separated through filtration because one of the substances is insoluble in water?
NaClO3 and Pb(ClO3)2
Na2SO4 and SrSO4
NaNO3 and Pb(NO3) 2
NaC2H3O2 and Pb(C2H3O2) 2
10B. (#3)
Which substance is soluble in an aqueous solution?
Pb(CO3)2
Ag3PO4
Sn(CrO4)2
NH4Cl
10B. (#4)
Which reactions produced precipitates?
1) Ba(NO3)2(aq) + Na2CO3(aq) --> BaCO3(s) + 2BaNO3(aq)
2) FeO3(s) + CO(g) --> Fe(l) + CO2(g)
3) Pb(NO3)2(aq) + 2 NH4I(aq) --> PbI2(s) + 2 NH4NO3(aq)
4) CH4 (g)+ O2(g) --> CO2(g) + H2O(l)
1,2
2,3
3,4
1,3
10B. (#5)
In a reaction between calcium hydroxide, Ca(OH)2 and lithium sulfide, Li2S, which of the following if any, would be the solid precipitate in water?
calcium sulfide, CaS
lithium hydroxide, LiOH
calcium sulfide (CaS) and lithium hydroxide (NaOH)
no precipitate produced
10E. (#1)
When the ends of two wires, from a circuit containing a battery and a lightbulb, are placed into a beaker containing an aqueous solution the light bulb glows brightly. From this observation, you can conclude the solution is probably —
a concentrated but weak base
a strong acid
a pH neutral sample of a polar compound
an acid added to a base
10E. (#2)
Which of the following describes a solution containing an electrolyte?
The solute particles are so firmly bonded that they do not break apart.
The solute particles permit the passage of an electric current.
It is unstable, and all the solute will precipitate if the solution is disturbed.
It cannot contain any more solute particles
10E. (#3)
Which of the following containers most likely containers sugar, C12H22O11?
Container A because it forms ions.
Container B because it forms ions.
Container A because it does not form ions.
Container B because it does not form ions.
10E. (#5)
Which of the following is a strong electrolyte when dissolved in water?
NaNO3
C12H22O11
C2H5OH
CH4
10E. (#6)
Classify Solution A and Solution B from the above image. (refer to your questionnaire)
A is an electrolyte, B is a nonelectrolyte.
A is a nonelectrolyte, B is an electrolyte.
Both A and B are electrolytes.
Both A and B are nonelectrolytes
10E. (#1)
If a solute is saturated at 42 g per 100 g H2O and 25oC, what would it be at 40g per 100 g H2O?
Saturated
Supersaturated
Unsaturated
Not enough information given
10E. (#2)
Which substance makes an unsaturated solution at a
temperature of 50 °C ?
80 g KCl
80 g KNO3
80 g KBr
80 g NaClO3
10E. (#3)
A chemistry student prepares a saturated
solution of KNO3 in 100 g water at 50°C. Then
she rapidly cools the solution to 40°C. Use
the graph to estimate how much solute will
likely precipitate. (or Refer to your graph on the questionnaire)
about 17 g
about 58 g
about 75 g
about 90 g
10E. (#4)
A student attempts to dissolve 60g of KCl in 100g of H20 at 60oC, but there some amount of KCl that will not
dissolve. Approximately how much solute is at the bottom?
16 grams
44 grams
56 grams
0 grams.
10E. (#5)
Which of the following creates a saturated solution when dissolved in 100g of H20 at 60 degrees C?
102g of KNO3
64g of KCl
48g of NaNO3
131g KI
10E. (#6)
A student is asked to determine whether a given solution is unsaturated, saturated, or supersaturated. The
student drops a tiny crystal of the solute into the solution and observes carefully for any change in the size of
the crystal. Which of the following statements is true?
No observable change means the solution is supersaturated.
A decrease in crystal size means the solution is unsaturated.
A decrease in crystal size means the solution is saturated.
An increase in crystal size means the solution is unsaturated.
10E.(#7)
A chemist is trying to increase the amount of a solid in a saturated solution. The best way to do this would be to-
A C
B D
Add more salt and stir
Add more salt and chill the solution in a freezer
Add more salt and heat while stirring
Add more salt and reduce the pressure
10F. (#1)
Three cups of carbonated soda are lowered into cups of water at varying temperatures. (Refer to the drawing in your questionnaire.) All other factors being equal, in which cup does the greatest release of dissolved gas occur and why?
Cup A, due to decreased solubility of gases at lower temperatures.
Cup B, because room temperature is ideal for the release of all gases.
Cup C, due to decreased solubility of gases at higher temperatures.
All cups will release the gas at same rate because temperature is not a factor.
10F. (#2)
Which of the following actions is most likely to speed up dissolution?
Crystals of sodium carbonate (Na2CO3) are crushed into a powder before being added to the solvent.
Water is cooled to 15°C before the solute is added.
An aqueous solution of sodium chloride (NaCl) is placed in a pressurized container.
Lithium iodide (LiI) is added to water and left to sit without stirring.
10F. (#3)
The diagram below shows a cube of sodium chloride beginning to dissolve in water. (Refer to your questionnaire.)
Which of the following changes will cause the cube to dissolve more quickly?
swirling the flask
removing the stopper
pouring off half the water
decreasing the water temperature
10F. (#4)
Fish need oxygen to survive. Goldfish in a crowded
aquarium have a better chance of survival in cold water than in warm water because:
In warm water, solubility of oxygen gas increases
In cold water, solubility of oxygen gas decreases
In cold water, solubility of oxygen gas increases
Water temperature does not affect solubility of oxygen gas
10F. (#5)
A chemist needs to increase the rate of dissolution
of an anti-cancer therapeutic in water. Which of
the following will not affect dissolution of a solid
chemical?
Raising the temperature of the solution.
Crushing the chemical into powder
Increasing pressure on the solution
Rapidly stirring the solution.
