Acid-base calculations questions

Assignment: Questions on Topic 18.2: Acid-base calculations

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Calculate the pH of:

i. 10.0 cm3 of 1.00 x 10−2 mol dm−3 hydrochloric acid solution.

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ii. 100 cm3 of 1.00 x 10−2 mol dm−3 hydrochloric acid solution.

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iii. 10.0 cm3 of 2.00 x 10−4 mol  dm−3 nitric acid solution.

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iv. 10.0 cm3 of 1.00 x 10−2 mol dm−3 sodium hydroxide solution.

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v. 10.0 cm3 of 1.00 x 10−3 mol dm−3 sulfuric acid solution. (Assume H2SO4 behaves as a strong diprotic acid.)

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vi. 20.0 cm3 of 1.00 x 10−3 mol dm−3 barium hydroxide solution, Ba(OH)2(aq).

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A solution has a pH of 3.60. Calculate:

i. the hydrogen ion concentration.

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ii. the hydroxide ion concentration.

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iii. the pH if the solution is diluted ten times (assume it is a strong acid as the degree of dissociation increases with dilution for weak acids).

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State the equations for the reaction of i. ethanoic acid and ii. ammonia with water.

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Calculate the pH of:

i.  1.00 x 10−3 mol dm−3 ethanoic acid solution, CH3COOH(aq). Ka(CH3COOH) = 1.8 x 10−5 at 298 K.

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ii. 3.00 x 10−2 mol dm−3 ammonia solution, NH3(aq). Kb(NH3) = 1.8 x 10−5 at 298 K.

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Use Section 21 of the IB Chemistry data booklet to calculate:

i.  the pH of 4.00 x 10−4 mol dm−3 propanoic acid solution, C2H5COOH(aq).

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ii. the pH of 1.00 x 10−5 mol dm−3 ethylamine (ethanamine) solution, C2H5NH2(aq).

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Use Section 21 of the IB data booklet to put the following in order of decreasing acid strength:
water, ethanoic acid, phenol, chloroethanoic acid, ethanol, propanoic acid, benzoic acid.

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The graph shows how the ionic product of water changes with temperature. Use the graph to determine:
 

i.  the value of Kw at 80 oC.

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ii.  the hydrogen ion concentration at 70 oC.

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iii. the hydroxide concentration at 70 oC.

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iv. the pH at 50 oC.

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v.  the pOH at 80 oC.

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