Grab a calculator and a copy of the periodic table

(This test has only 10 questions, but may take 15 - 20 mins).
1. The correct formula for the concentration of a solution in mol/dm3 is..
  • A.   concentration = number of moles x volume in cm3
  • B.   concentration = number of moles x volume in dm3
  • C.   concentration = number of moles ÷ volume in cm3
  • D.   concentration = number of moles ÷ volume in dm3
2. Calculate the concentration of a solution made by dissolving 0.40 moles of potassium nitrate in water producing 100 cm3 of solution.
  • A.   40 mol/dm3
  • B.   4.0 mol/dm3
  • C.   0.040 mol/dm3
  • D.   0.0040 mol/dm3
3. Which solution contains the greatest number of moles?
  • A.   20 cm3 of 2.0 mol/dm3 hydrochloric acid
  • B.   40 cm3 of 1.0 mol/dm3 hydrochloric acid
  • C.   60 cm3 of 1.0 mol/dm3 sodium hydroxide
  • D.   80 cm3 of 0.5 mol/dm3 sodium hydroxide
4. 1.0dm3 of ethanoic acid solution, CH3COOH, contains 6.0 g of ethanoic acid

[Mr value of CH3COOH = 60].
The concentration of the ethanoic acid solution, in mol/dm3, is..

  • A.   0.1
  • B.   0.6
  • C.   1.0
  • D.   10
5. Sodium hydroxide solution can be neutralized using dilute ethanoic acid. The equation for the reaction is:                            

NaOH(aq) + CH3COOH(aq) → CH3COONa(aq) + H2O(l)

Calculate the volume of 0.200 mol/dm3 ethanoic acid needed to exactly neutralize 0.0025 moles of sodium hydroxide solution.

  
  • A.   0.0125 cm3   
  • B.   1.25 cm3    
  • C.   12.5 cm3
  • D.   12.5 dm3

Q6-7:
A student plans to titrate 25.0 cm3 of sulfuric acid with 0.200 mol/dm3 sodium hydroxide solution using phenolphthalein as an indicator.
The piece of apparatus which should be used to measure the..

  
6. ..volume of sulfuric acid is a .
7. ..volume of sodium hydroxide is a .
8. 0.30 moles of barium chloride solution was added to 0.20 moles of magnesium sulfate solution in the following precipitation reaction:

BaCl2(aq) + MgSO4(aq) → BaSO4(s) + MgCl2(aq)

How many moles of barium sulfate, BaSO4, would be produced?

  • A.   0.20
  • B.   0.25
  • C.   0.30
  • D.   0.50

Q9-10:
A student added excess sodium hydrogen carbonate to 35.0 cm3 of 0.500 mol/dm3 citric acid solution. She measured the temperature change and calculated that 1500 J of energy was absorbed during the reaction.

  
9. How many moles of citric acid were used?
  • A.   17.5      
  • B.   14.3
  • C.   0.0175
  • D.   0.0143
10. Calculate the enthalpy change for the reaction, ΔH, in kilojoules per mole of citric acid.
  • A.   +85.7 kJ/mol
  • B.   -85.7 kJ/mol
  • C.   +104.9 kJ/mol
  • D.   -104.9 kJ/mol