An IB Periodic Table is required

Calculators should not be used for multiple choice questions!
1. What is the concentration of a solution (in mol dm-3) which contains 4.00g of sodium hydroxide, NaOH, in 500cm3 of solution?
  • A.   2.00 x 10-3
  • B.   0.0200
  • C.   0.200
  • D.   5.00
2. Which solution contains the greatest number of moles of ions?
  • A.   20cm3 of 0.2mol dm-3 NaCl
  • B.   10cm3 of 0.2mol dm-3 FeCl3
  • C.   50cm3 of 0.1mol dm-3 CuSO4
  • D.   40cm3 of 0.1mol dm-3 Na2SO4
3. What mass of solid is required to produce 200cm3 of a standard sodium carbonate solution, Na2CO3, of concentration 0.100 mol dm-3?

 

 volumetric flask
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  • A.   2.12g
  • B.   10.6g
  • C.   53.0g
  • D.   212g
4. What volume, in cm3, of 0.50 mol dm-3 KOH is required to neutralize 0.010 mole oxalic acid?

C2H2O4(aq) + 2KOH(aq) → K2C2O4(aq) + 2H2O(l)

  • A.   0.04
  • B.   0.10
  • C.   10
  • D.   40

5. 25.00cm3 of 0.0146mol dm-3 sodium hydroxide solution, NaOH, reacted exactly with 10.35cm3 of phosphoric acid solution, H3PO4.
What was the concentration of the phosphoric acid solution?

  • A. 
 $${0.02500 \times 0.0146 \times 3} \over{0.01035}$$
  • B. 
 $${0.02500 \times 0.0146} \over{3 \times 0.01035}$$
  • C. 
 $${0.02500 \times 0.0146} \over{0.01035}$$
  • D. 
$${25 \times 0.0146 \times 3} \over{10.35}$$
6. A precipitate of aluminium hydroxide was produced by the following reaction:

Al2(SO4)3(aq) +6NaOH(aq) → 2Al(OH)3(s) + 3Na2SO4(aq)

How many moles of aluminium hydroxide were formed when O.4 moles of aluminium sulfate solution and 1.2 moles of sodium hydroxide solution were mixed?

  • A.   0.2
  • B.   0.4
  • C.   0.8
  • D.   1.6

7. A solution containing iron(II) ions required 8.20cm3 of  0.010mol dm-3 acidified potassium manganate(VII) solution, KMnO4, for complete reaction.

The ionic equation for the reaction is:

5Fe2+(aq) + MnO4-(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq)  + 4H2O(l)

What amount (in moles) of iron(II) ions was contained in the sample?

Theresa Knott
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 titration apparatus
  • A.   8.20 x 10-5
  • B.   4.10 x 10-4
  • C.   0.082
  • D.   0.410
8. 0.50 moles of ammonium iron(II) sulfate hexahydrate, (NH4)2Fe(SO4)2.6H2O was dissolved in water to produce 2.0dm3 of solution. What is the concentration (in mol dm-3) of ammonium ions in the solution?
  • A.   0.10
  • B.   0.25
  • C.   0.50
  • D.   1.25
9. 0.2 moles of barium chloride solution were reacted with 0.3 moles of copper(II) sulfate solution in the following precipitation reaction:

BaCl2(aq) + CuSO4(aq) → BaSO4(s) + CuCl2(aq)

Which reactant is limiting and how many moles of copper(II) ions will remain in solution at the end of the reaction?

  
  Limiting reactant Moles of Cu2+ ions remaining in solution
A Barium chloride 0.3
B Barium chloride 0.1
C Copper(II) sulfate 0.3
D Copper(II) sulfate 0.1
10. An ethanoic acid/sodium ethanoate buffer solution was made by adding 25cm3 of 0.10 mol dm-3 sodium hydroxide solution, NaOH, to 25cm3 of 0.20 mol dm-3 ethanoic acid, CH3COOH.

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

What was the concentration (in mol dm-3) of ethanoic acid in the final buffer mixture?

  • A.   0.025
  • B.   0.050
  • C.   0.10
  • D.   0.20