Year 11 Water Practice Quiz 1 Solution
/ 50
1. Which word describes the water part of seawater? Multiple Choice: 1 mark each
a) solute.
b) solvate.
c) solvent.
d) solution.
2. Which of the following is not a reason for the importance of water to life on Earth?
a) It allows substances to dissolve and move around inside cells.
b) It can dissolve a wide variety of polar substances because it is a non-polar molecule.
c) It is a reactant in the photosynthesis reaction.
d) It helps regulate the temperature of the planet.
3. Construct Lewis dot diagrams of the following:

Water (H2O)

Oxygen (O2)

Hydrogen Sulfide (H2S)

Ammonia (NH3)

Carbon dioxide (CO2)
5 marks
4. A liquid has a density of 1.5 g/cm3. What volume will 6g of the liquid occupy?
Density = mass / volume
1 mark
volume = mass / density = 6 ÷ 1.5 = 4 cm3
5. Why does water have a higher boiling point than hydrogen sulphide?
a) Water has a higher density.
b) Water often has impurities dissolved in it.
c) The molecular weight of water is greater than that molecular weight of hydrogen sulfide.
d) Hydrogen bonding in water.
6. Write an ionic equation for calcium hydroxide dissolving in water.
1 mark
Ca(OH)2(s) → Ca2+(aq) + 2OH-(aq)
7. What is the heat capacity of water?
a) 4 J/g.K.
b) 418 J/g.K.
c) 6 kJ/g.K
d) 4.18 J/g.K
8. Write a net ionic equation of the formation of the precipitate when lithium chloride is mixed with silver
nitrate. 2 marks
Ag+(aq) + Cl-(aq) → AgCl (s)
9. Which statement best defines hydrogen bonding?
a) An force of attraction between the hydrogen atoms in a molecule and the unbonded pair of electrons
of an oxygen, nitrogen or fluorine atom of another molecule.
b) An force of attraction between the hydrogen atoms in a molecule and the unbonded pair of electrons of
an oxygen, nitrogen or fluorine atom of the same molecule.
c) A force of repulsion between hydrogen atoms in the same molecule.
d) A force of attraction between hydrogen atoms in different molecules.
10. Which list contains only polar molecules?
a) Water, ammonia, hydrogen chloride.
b) Ammonium, water, hydrogen.
c) Benzene, kerosene, carbon dioxide
d) Sodium chloride, water, potassium iodide.
11. Name three types of intermolecular forces in order of decreasing strength.

Hydrogen bonding

Dipole-dipole

Dispersion
3 marks
12. Which statement is true?
a) H2O has a lower boiling point than H2S because of hydrogen bonding.
b) H2S has a higher boiling point than H2O because of hydrogen bonding.
c) H2S has a higher boiling point than H2O because it has a higher molecular weight.
d) H2O has a higher boiling point than H2S because of hydrogen bonding.
13. Identify the main type of intermolecular forces for each of the following substances.

Water (Hydrogen bonding)

Helium (Dispersion)

Nitrogen dioxide (Dipole-dipole)
14. Glycerine [C3H5(OH)3] is a highly viscous liquid. Why?
a) It is used to make explosives.
b) Hydrogen bonding.
c) It is a sweet liquid that can be used in place of honey for cooking.
d) It has a low melting point.
15. Which of the following substances are highly soluble in water?
a) Salts, alcohols, oxygen.
b) Sodium chloride, ethanol, ammonia.
c) Oxygen, ammonia, carbon dioxide.
d) Calcium carbonate, sodium chloride, magnesium oxide.
3 marks
16. What is the chemical formula of the precipitate when solutions of sodium chloride and silver (I) nitrate are
mixed?
a) SiCl.
b) NaNO3.
c) ClNO3.
d) AgCl.
17. Which of the following is a solubility rule?
a) All ionic substances are soluble.
b) All ionic substances are soluble in water.
c) Most carbonates are soluble in water.
d) Most carbonates are insoluble in water.
18. Write an equation for the reaction between calcium nitrate and ammonium carbonate solutions. Show all
states.
3 marks
Ca(NO3)2(aq) + (NH4)2CO3(aq) → Ca CO3(s) + 2NH4NO3(aq)
19. How is molarity defined?
a) The number of moles of solute per litre of solution.
b) The number of moles of solvent per litre of solution.
c) The number of moles of solute per litre of solvent.
d) The mass of solute per litre of solution.
20. What is the molarity of 300ml of solution containing 20g of lithium nitrate?
2 marks
v=0.3L, m=20g, M=6.941+14.01+3x16.00 = 68.951
n=m/M = 20/68.951 = 0.29
c=n/v = 0.29/0.3 = 0.967M
21. What is the volume of 700ml of 0.5M CaCl2 solution diluted to 0.23M?
2 marks
C1=0.5, V1 = 0.7, C2 = 0.23, V2=?
C1V1 = C2V2 V2=C1V1/C2 = 0.5 x 0.7 / 0.23 =1.52L
22. How much heat is required to raise the temperature of 2kg of water by 3 degrees?
3 marks
q=mCΔT= 2000 x 4.18 x 3 = 25080 J
23. What is the name of the piece of equipment used to experimentally measure the heat absorbed or released
in processes?
a) Joulometer.
b) Calorimeter.
c) Kelivometer.
d) Heatometer.
24. Why is thermal pollution an issue?
a) Aquatic organisms will become lazy.
b) The blood of aquatic organisms will boil.
c) The solubility of oxygen decreases with increasing temperature.
d) Aquatic plants lose the ability to photosynthesize at high temperatures.
25. Which words describe the giving out and taking in of heat?
2 marks
Exothermic and endothermic, respectively
26. Thermodynamically, what type of process is dissolving sodium hydroxide in water?
2 marks
An exothermic process
27. Give an example of an exothermic chemical reaction.
1 mark
Combustion reactions are examples of exothermic reactions. e.g. CH4 + 2O2 → CO2 + 2H2O
28. What is the term for solvent molecules surrounding solute molecules when in solution?
2 marks
solvation
29. Classify the following substances as soluble or insoluble in water.
Ethanol
Soluble
Calcium carbonate
Insoluble
Sodium chloride
Soluble
Kerosene
Insoluble
1 mark each