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Proton Transfer Reactions (DP IB Chemistry: SL): Exam Questions

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11 mark

Using your knowledge of the Brønsted-Lowry theory, which of the following correctly describes ammonia?

  • neutral

  • acid

  • base

  • amphoteric

Choose your answer

21 mark

In the Brønsted–Lowry theory of acids and bases, the difference between a conjugate acid and its conjugate base is the presence of which of the following?

  • a positive charge

  • a pair of electrons

  • a proton

  • a hydrogen atom

Choose your answer

31 mark

Which of the following ions or compounds is amphiprotic?

  • P4O10

  • PO43−

  • HCO3−

  • Al2O3

Choose your answer

41 mark

In the following reaction, identify which two species are acting as Brønsted–Lowry acids

H3PO4 (aq) + OH− (aq)  ⇋ H2PO4− (aq) + H2O (l)

  • H2PO4− (aq) and OH− (aq)

  • H3PO4 (aq) and H2PO4− (aq)

  • H2PO4− (aq) and H2O (l)

  • H3PO4 (aq) and H2O (l)

Choose your answer

51 mark

Potassium hydrogen carbonate reacts vigorously with dilute sulfuric acid. Identify the correct formulas of the substances produced in the reaction

  • K2SO4 + H2O + CO2

  • K2SO4 + CO2

  • KSO4 + H2O + CO2

  • KSO4 + H2CO3

Choose your answer

61 mark

Copper(II) sulfate can be made by the reaction between dilute sulfuric acid and which of the following?

I. Cu

II. CuO

III. CuCO3

  • I and II only

  • I and III only

  • II and III only

  • I, II and III

Choose your answer

71 mark

Which statement is correct for the following equation?

HSO4- (aq) + OH- (aq) ⇌ SO4- (aq) + H2O (l)

  • OH- and H2O are an acid and conjugate base pair

  • SO4- is acting as Brønsted–Lowry acid

  • HSO4- and SO4- are a base and conjugate acid pair

  • OH- and H2O are a base and conjugate acid pair

Choose your answer

81 mark

Which row shows the correct acid and base needed to make the salt specified? 

 

Acid

Base

Salt

A

NaHCO3

SO2

Na2SO4

B

HNO3

SO3

(NH4)2SO4

C

H2SO4

ZnO

ZnSO3

D

H2SO4

NH4OH

(NH4)2SO4

    Choose your answer

    91 mark

    Which is a conjugate acid-base pair?

    HCO3- (aq) + H2O (l)  ⇌ CO32- (aq) + H3O+ (aq)

    • HCO3- / H3O+

    • HCO3- / CO32- 

    • H2O / CO32- 

    • HCO3- / H2O

    Choose your answer

    101 mark

    Which coefficients balance the following acid-base equation?

    Al(OH)3 (s) + HNO3 (aq)  → Al(NO3)3 (aq) + H2O (l)

    A

    3

    1

    3

    1

    B

    2

    2

    1

    3

    C

    1

    3

    1

    3

    D

    1

    2

    1

    2

      Choose your answer

      111 mark

      Four 1.0 M solutions of HCl, NH3, NaOH and CH3COOH have been mislabelled, but a student has a pH meter to test the pH of the solutions at 25 °C. Arrange the solutions in order of increasing pH:

      • HCl (aq) < NH3 (aq) < NaOH (aq) < CH3COOH (aq)

      • CH3COOH (aq) < HCl (aq) < NH3 (aq) < NaOH (aq)

      • HCl (aq) < CH3COOH (aq) < NH3 (aq) < NaOH (aq)

      • NaOH (aq) < NH3 (aq) < CH3COOH (aq) < HCl (aq)

      Choose your answer

      121 mark

      Below are four statements about acid and bases. Which is the correct one?

      • Strong acids are good proton donors and have weak conjugate bases.

      • Strong bases are good proton donors and have weak conjugate acids.

      • Weak acids are poor proton acceptors and have strong conjugate bases.

      • Strong acids are good proton donors and have strong conjugate bases.

      Choose your answer

      131 mark

      Which statement is correct about the action of weak acids and their conductivity?

      • Weak acids are proton donors and their solutions are good conductors.

      • Weak acids are proton donors and their solutions are poor conductors.

      • Weak acids are proton acceptors and their solutions are good conductors.

      • Weak acids are proton acceptors and their solutions are good conductors.

      Choose your answer

      141 mark

      The correct expression for the ionic product of water at 25 ℃ is

      • begin mathsize 16px style K subscript w equals fraction numerator left square bracket H to the power of plus right square bracket left square bracket O H to the power of minus right square bracket over denominator left square bracket H subscript 2 O right square bracket end fraction end style

      • H2O (l) ⇌ H+ (aq) + OH- (aq)

      • Kw = [H+][OH-]

      • 1 x 10-14 mol2 dm-6

      Choose your answer

      151 mark

      34.3 cm3 of 0.125 mol dm-3 sodium hydroxide solution reacts with 26.0 cm3 of sulfuric acid. What is the concentration of the acid?

      • 0.16 mol dm–3

      • 0.33 mol dm–3

      • 0.08 mol dm–3

      • 3.03 mol dm–3

      Choose your answer

      161 mark

      90 cm3 of water is added to 10 cm3 of hydrochloric acid with a pH of 2. What is the new pH of the acid?

      • 1

      • 3

      • 5

      • 7

      Choose your answer

      171 mark

      Which of the following is true about weak acids?

      I. They are poor conductors of electricity

      II. They have a high pH

      III. They react with carbonates to produce carbon dioxide

      • I and II only

      • I and III only

      • II and III only

      • I, II and III

      Choose your answer

      181 mark

      Which is true about 1.0 mol dm-3 solutions of weak and strong acids?

      • Magnesium will react with strong acids but not weak acids

      • Fewer moles of base are needed to neutralise weak acids

      • Sodium carbonate reacts more slowly with weak acids

      • Weak acids have a lower pH than strong acids

      Choose your answer

      191 mark

      Four solutions, K, L, M and N have the following properties

      K: pH= 8       L: [H+] = 1 x 10-3 mol dm-3 M: pH= 5    N: [H+] = 1 x 10-7 mol dm-3

      What is their correct order of increasing acidity?

      • K < L < M < N

      • N < L < M < K

      • K < N < M < L

      • N < M < L < K

      Choose your answer

      201 mark

      Two beakers contain solutions of hydrochloric acid at pH = 2 and pH = 4.

      How does the concentration of hydrogen ions in the beaker at pH = 4 compare to the concentration in the beaker at pH = 2?

      • Twice as large

      • Half as much

      • begin mathsize 16px style 1 over 10 end style of the value

      • begin mathsize 16px style 1 over 100 end style of the value

      Choose your answer

      211 mark

      A sample of acid rain water is tested and found to be pH 4. How does its hydrogen ion concentration compare to pure water? 

      • 1000 times more concentrated

      • 3 times more concentrated

      • 1000 times less concentrated

      • 3 times less concentrated

      Choose your answer

      22
      Sme Calculator      1 mark

      Which of the following best describes the general shape of a pH curve for a titration involving a strong base and a strong acid?

      • The pH starts low and rises sharply, with the equivalence point below pH 7

      • The pH starts high and falls gradually, with no clear equivalence point

      • The pH starts high and then decreases sharply, with the equivalence point at pH 7

      • The pH remains constant throughout the titration

      Choose your answer

      11 mark

      The typical reactions of dilute acids include them being able to react with

      I. NaHCO3

      II. Mg

      III. Cu

      • I and II only

      • I and III only

      • II and III only

      • I, II and III

      Choose your answer

      21 mark

      The following reaction occurs between concentrated sulfuric and nitric acids.

      H2SO4 + HNO3 ⇋  H2NO3+ + HSO4-

      Identify the two species which are acting as Brønsted–Lowry bases.

      • H2NO3+ and HSO4-

      • HNO3 and H2NO3+

      • H2SO4 and HSO4- 

      • HNO3 and HSO4-

      Choose your answer

      31 mark

      What role does each species play in the equilibrium below according to Brønsted-Lowry theory?

      CH3COOH + HCl  ⇌ CH3COOH2+ + Cl-

       

      CH3COOH

      HCl

      CH3COOH2+

      Cl-

      A

      acid

      base

      base

      acid

      B

      acid

      base

      acid

      base

      C

      base

      acid

      base

      acid

      D

      base

      acid

      acid

      base

        Choose your answer

        41 mark

        Perbromic acid, HBrO4 , is an example of a strong acid when dissolved in water. What is true about perbromic acid?

        • HBrO4 is largely found as molecules in the solution

        • HBrO4 solution reacts only with strong bases

        • HBrO4 is fully dissociated in solution

        • HBrO4 has a pH greater than 7

        Choose your answer

        51 mark

        Potassium hydrogenphosphate has the formula K2HPO4.

        What is the conjugate base of K2HPO4?

        • H2PO4-

        • KHPO42-

        • PO43-

        • KH2PO4

        Choose your answer

        61 mark

        For the equilibrium equation shown, which species are Brønsted-Lowry acids?

        H3NSO3 (aq) + 2NH3 (aq) ⇌ HNSO32- (aq) + 2NH4+ (aq)

        • NH4+ and NH3

        • NH4+ and HNSO32-

        • H3NSO3 and HNSO32-

        • H3NSO3 and NH4+

        Choose your answer

        71 mark

        Which would be formed when calcium oxide reacts with hydrochloric acid ?

        • Calcium chloride and carbon dioxide

        • Calcium chloride, hydrogen gas and water

        • Calcium, hydrogen gas and water

        • Calcium chloride and water

        Choose your answer

        81 mark

         What is the sum of the coefficients when the following acid-base equation is balanced?

        _HNO3 (aq) + _Mg(HCO3)2 (s) →  _Mg(NO3)2 (aq) + _H2O (l) + _CO2  (g)

        • 5

        • 6

        • 7

        • 8

        Choose your answer

        91 mark

        Which oxides react with calcium oxide?

        I. SO2

        II. NO2

        III. K2O

        • I and II only

        • I and III only

        • II and III only

        • I, II and III

        Choose your answer

        101 mark

        Which row correctly describes the reaction specified?

         

        Reaction

        Energy change

        A

        metal displacement

        endothermic

        B

        neutralisation

        exothermic

        C

        combustion

        endothermic

        D

        melting ice

        exothermic

          Choose your answer

          111 mark

          Determine which of the following solutions would be basic at 25 °C?

          Kw = 1.0 × 10−14 mol2 dm-6

          • [H+] = 1.0 × 10−2 mol dm−3

          • [OH−] = 1.0 × 10−12 mol dm−3

          • solution of pH = 5.00

          • [H3O+] = 1.0 × 10−12 mol dm−3

          Choose your answer

          121 mark

          Carbon dioxide reacts with water at 25 °C to form carbonic acid which can be represented in the following equation

          CO2(g)  +  H2O(l)  ⇋  H+(aq)  +  HCO3−(aq)

          If the pressure is raised, what will happen to the position of equilibrium and the pH?

          • The equilibrium shifts to the right and pH increases

          • The equilibrium shifts to the right and pH decreases

          • The equilibrium shifts to the left and pH increases

          • The equilibrium shifts to the left and pH decreases

          Choose your answer

          131 mark

          When comparing the separate reactions of 0.5 g magnesium metal with excess equal volumes and concentrations of hydrochloric acid and ethanoic acid you can say that the

          • Hydrochloric acid reacts faster than ethanoic acid as its pH is higher

          • More gas is produced with hydrochloric acid than with ethanoic acid

          • An equal volume of gas is produced with both hydrochloric acid and ethanoic acid.

          • Ethanoic acid reacts more slowly than hydrochloric acid because its pH is lower 

          Choose your answer

          141 mark

          In the table below are the formulae of some acids and bases. Which row shows only weak acids and weak bases?

          A

          CH3NH2

          Ba(OH)2

          HCOOH

          B

          CH3CH2COOH

          C6H5NH2

          HCOOH

          C

          NH3

          HNO3

          CH3CH2COOH

          D

          NH3

          KOH

          H2CO3

            Choose your answer

            151 mark

            Three solutions of hydrochloric acid of different concentrations are shown below

            X.   0.100 mol dm-3

            Y.   0.001 mol dm-3

            Z.   0.010 mol dm-3

            If these solutions are arranged from lowest to highest pH, then the order is  

            • X﹤ Y ﹤ Z

            • X﹤ Z ﹤ Y

            • Y﹤ X ﹤Z

            • Y﹤ Z ﹤ X

            Choose your answer

            161 mark

            Which of the following statements is correct? 

            • As temperature increases, the pH value of pure water decreases

            • As temperature decreases, the pH value of pure water decreases

            • The pH of water is unaffected by temperature 

            • Pure water is not neutral 

            Choose your answer

            171 mark

            Equal volumes of hydrochloric acid of different concentrations are added to four beakers, A, B, C and D. Equal volumes of 1.0 mol dm-3 sodium hydroxide are then added to the beakers and the pH is measured.

            Beaker

            A

            B

            C

            D

            pH

            1

            5

            7

            13

            Which beaker contains the most concentrated solution of hydrochloric acid?

            • Beaker A

            • Beaker B

            • Beaker C

            • Beaker D

            Choose your answer

            11 mark

            Some species may be classified as amphiprotic, some as amphoteric and some as both. Which of the following applies to HPO42−?

            • Amphiprotic but not amphoteric

            • Amphoteric but not amphiprotic

            • Amphiprotic and amphoteric

            • Neither amphiprotic nor amphoteric

            Choose your answer

            21 mark

            The aromatic compound phenol, C6H5OH, behaves as a weak acid, due the presence of a hydroxyl group on the benzene ring. What is the correct formula of the conjugate base formed when phenol dissociates?

            • C6H4--OH 

            • C6H5-OH2+

            • C6H5-O-

            • C6H6+-OH 

            Choose your answer

            31 mark

            What is the sum of the coefficients when the following acid-base equation is balanced?

            _Al2(CO3)3 (s) + _HNO3 (aq)  ⇌ _Al(NO3)3 (aq) + _H2O (l) +  _CO2 (g)

            • 6

            • 7

            • 14

            • 15

            Choose your answer

            41 mark

            Which of the following substances can be used to prepare magnesium sulfate by a neutralization reaction with dilute sulfuric acid?

            I. Mg

            II. MgO

            III. MgCO3

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

            Choose your answer

            51 mark

            Phosphoric acid is a polyprotic acid and can produce amphiprotic species when it dissociates. Which of the following species is amphiprotic?

            I. HPO42−

            II. H2PO4−

            III. PO43−

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

            Choose your answer

            61 mark

            Use the following reactions to answer the question below:

            H2O (l) + F- (aq) ⇌ HF (aq) + OH- (aq)

            H2O (l) + HNO3 (aq) → H3O+ (aq) + NO3- (aq)

            H2O (l) + CO2 (g) ⇌ H2CO3 (aq)

            H2O (aq) +  NH3 (aq) ⇌ NH4+ + OH- (aq) 

            Which of the following statements is true?

            • HNO3 and H2O both act as acids once

            • H2O is shown acting as a Bronsted-Lowry acid only

            • H2O reacts as an acid twice

            • H2O is shown as a diprotic acid

            Choose your answer

            71 mark

            Which species are Bronsted-Lowry acids in the reaction shown?

            H2PO4− (aq) + CN- (aq) ⇌  HCN (aq)  + HPO42− (aq)

            • HCN and H2PO4−

            • HCN and CN-

            • H2PO4− and HPO42−

            • HCN and HPO42−

            Choose your answer

            81 mark

            Which of the following solutions will react with a strip magnesium ribbon?

            • Sodium hydrogencarbonate

            • Sodium hydrogensulfate

            • Ammonia

            • Limewater

            Choose your answer

            91 mark

            Which substance reacts with ammonia but is not a Brønsted–Lowry acid?

            • HCl

            • CH3COOH

            • BF3

            • CF3COOH

            Choose your answer

            101 mark

            Which of the following statements is incorrect about 0.01 mol dm–3 CH3COOH?

            • the pH = 2

            • [H+] << 0.01 mol dm–3

            • [CH3COO–] is approximately equal to [H+]

            • CH3COOH is partially ionised

            Choose your answer

            111 mark

            Two flasks contain two different acids labelled as HA and HB. A student measures the pH of each flask, and finds that they are pH 1 and pH 3 respectively.

            Which of the following statements is true?

            • HA is a stronger acid than HB

            • HB is a stronger acid than HA

            • The [H3O+] in the solution of HB is 3 times greater than the [H3O+] in the solution of HA.

            • The [H3O+] in the solution of HA is 100 times greater than the [H3O+]  in the solution of HB.

            Choose your answer

            121 mark

            Which of the following solutions will have the largest amount of H+ ions in moles?

            • 20 cm3 of 2.0 mol dm−3 sulfuric acid

            • 10 cm3 of 3.0 mol dm−3 nitric acid

            • 80 cm3 of 0.5 mol dm−3 hydrochloric acid

            • 40 cm3 of 1.0 mol dm−3 ethanoic acid

            Choose your answer

            131 mark

            If the pH of two acids, X and Y, are pH 1 and pH 2 respectively, which of the following is true?

            I. X and Y could be strong or weak acids

            II. The concentration of [H+] ions in X is higher than in Y

            III. Acid X is stronger than acid Y

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

            Choose your answer

            141 mark

            A student has two flasks containing 150 cm3 of nitric acid, HNO3(aq) and ethanoic acid, CH3COOH(aq). She writes the following three statements in her notebook about the acids. Which of them are correct?

            I. HNO3 dissociates more than CH3COOH

            II. HNO3 conducts electricity better than CH3COOH

            III. more NaOH can be neutralised with HNO3 than CH3COOH

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

            Choose your answer

            151 mark

            In a titration, the equivalence point is reached when 23.70 cm3 of 0.02 mol dm-3 potassium hydroxide reacts with 0.03 mol dm-3 of sulfuric acid. What volume of acid is needed?

            • 7.9 cm3

            • 31.65 cm3

            • 15.80 cm3

            • 17.78 cm3

            Choose your answer

            161 mark

            Acid rain can be up to 50 times more acidic than normal rain, which has a pH around 5.5. What is the approximate concentration of H+ in acid rain?

            • 2.50 size 16px cross times10-3 mol dm-3 

            • 2.50 size 16px cross times 10-4 mol dm-3 

            • 2.50 size 16px cross times 10-5 mol dm-3 

            • 50.0 begin mathsize 16px style cross times end style 10-4 mol dm-3 

            Choose your answer

            171 mark

            Which is true about the hydrogensulfate ion, HSO4-, found in acid rain?

            I. It is amphiprotic

            II. It is amphoteric

            III. Sulfur is in its highest oxidation state

            • I and II only

            • I and III only

            • II and III only

            • I, II and III

            Choose your answer