DP Chemistry Questionbank

• Syllabus

Topic 8: Acids and bases

Sub sections and their related questions

8.1 Theories of acids and bases

• 15M.2.hl.TZ1.2c: Predict and explain the pH of the following aqueous solutions, using equations to support your...
• 15M.2.hl.TZ1.8d.i: State the formula of the conjugate base of chloroethanoic acid,...
• 15M.2.hl.TZ2.7e.ii: Define the term weak base according to the Brønsted–Lowry theory.
• 15M.2.sl.TZ1.6e: Explain whether BF3 can act as a Brønsted-Lowry acid, a Lewis acid or both.
• 15M.2.sl.TZ2.5f.ii: Define the term weak base according to the Brønsted-Lowry theory.
• 15M.2.sl.TZ2.5f.iii: Deduce the formulas of conjugate acid-base pairs in the reaction...
• 14M.1.hl.TZ2.26: What is the conjugate base of phenol,...
• 14M.1.sl.TZ1.21: Which are acid-base pairs according to the Brønsted‒Lowry theory? I.    ...
• 14N.2.hl.TZ0.9g: Describe what is meant by a weak Brønsted-Lowry base, including an equation for the reaction of...
• 14N.2.sl.TZ0.6d.iv: State the formula of the conjugate base of...
• 13N.1.hl.TZ0.25: What are the conjugate acid–base pairs in the following...
• 13N.2.hl.TZ0.7b.ii: Explain the behaviour of HF in terms of the Brønsted–Lowry theory of acids.
• 13N.1.sl.TZ0.21: What are the conjugate acid–base pairs in the following...
• 13N.2.sl.TZ0.5c.i: Define a Brønsted–Lowry acid.
• 13M.1.hl.TZ2.26: Which of the following is an example of a Lewis acid–base reaction, but not a Brønsted–Lowry...
• 13M.2.hl.TZ2.6b.i: Define an acid according to the Brønsted–Lowry theory and the Lewis theory.   Brønsted–Lowry...
• 12N.1.sl.TZ0.22: Which row correctly describes...
• 12N.2.sl.TZ0.5b.i: Define an acid according to the Brønsted–Lowry and Lewis theories.   Brønsted–Lowry...
• 10N.2.hl.TZ0.7d: The reaction between \({{\text{N}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(aq)}}\) and HCl(aq)...
• 10N.1.sl.TZ0.21: What is the conjugate base of \({{\text{H}}_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}\)...
• 09N.1.hl.TZ0.24: According to the Brønsted-Lowry theory, how does each species act in the equilibrium...
• 09N.1.sl.TZ0.22: What is the formula of the conjugate base of the hydrogenphosphate ion, \({\rm{HPO}}_4^{2 -...
• 09N.2.sl.TZ0.6a.i: For each of the reactions A and B, deduce whether water is acting as an acid or a base and...
• 10M.2.sl.TZ1.3b.iii: State an equation, including state symbols, for the reaction of ethanoic acid with water....
• 10M.1.sl.TZ2.22: Which species behave as Brønsted-Lowry acids in the following reversible...
• 09M.2.sl.TZ1.6c.i: Define a Brønsted-Lowry acid.
• 09M.2.sl.TZ1.6c.ii: Deduce the two acids and their conjugate bases in the following...
• 09M.1.sl.TZ2.21: Which are definitions of an acid according to the Brønsted-Lowry and Lewis theories?
• 09M.2.sl.TZ2.1b.vii: The other product of the reaction is ethanoic acid,...
• 11M.2.hl.TZ1.8a.i: Define the terms acid and base according to the Brønsted-Lowry theory. Distinguish between a weak...
• 11M.1.sl.TZ1.22: Consider the equilibrium...
• 11M.2.sl.TZ1.5c.i: Define the terms acid and base according to the Brønsted-Lowry theory and state one example of a...
• 11M.1.sl.TZ2.20: Which is not a conjugate acid-base pair? A.     \({\text{HN}}{{\text{O}}_{\text{3}}}\) and...
• 11M.2.sl.TZ2.5a.v: Explain, using the Brønsted-Lowry theory, how water can act either as an acid or a base. In each...
• 12M.1.sl.TZ2.21: What is the Brønsted–Lowry conjugate base of \({{\text{H}}_{\text{2}}}{\text{PO}}_4^ - \)? A.  ...
• 12M.2.sl.TZ2.6b.i: State the equation for the reaction of ammonia with water.
• 12M.2.sl.TZ2.6b.ii: Explain why ammonia can act as a Brønsted–Lowry base.
• 11N.1.sl.TZ0.21: Which descriptions are correct for both a Brønsted–Lowry acid and a Lewis acid?
• 16M.1.sl.TZ0.19: Which is a conjugate...
• 16M.2.sl.TZ0.1b: Phosphine is usually prepared by heating white phosphorus, one of the allotropes of phosphorus,...
• 16M.2.hl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) State the hybridization of the...
• 16M.2.hl.TZ0.1b: Phosphine is usually prepared by heating white phosphorus, one of the allotropes of phosphorus,...
• 16N.1.sl.TZ0.19: Which species behave as Brønsted–Lowry bases in the following reaction?  H2SO4 + HNO3  H2NO3+ +...
• 17M.1.sl.TZ1.19: Which is an acid-base conjugate pair? A.     H3O+ / OH– B.     H2SO4 / SO42– C.     CH3COOH /...
• 17M.1.hl.TZ1.24: Which species produced by the successive dissociations of phosphoric acid, H3PO4,...
• 17M.1.hl.TZ1.26: Which species acts as a Lewis and Brønsted–Lowry base? A.      [Al(H2O)6]3+ B.      BF3 C.    ...
• 17M.1.sl.TZ2.20: Which of the following is correct? A.     A weak acid is a proton donor and its aqueous solution...
• 17M.2.sl.TZ2.7a.i: Identify the amphiprotic species.
• 17M.2.sl.TZ2.7a.ii: Identify one conjugate acid-base pair in the reaction.
• 17M.2.sl.TZ2.7b.i: Calculate the amount, in mol, of NaOH(aq) used.
• 17N.2.sl.TZ0.5b.i: Identify two different amphiprotic species in the above reactions.
• 17N.2.sl.TZ0.5b.ii: State what is meant by the term conjugate base.
• 17N.2.sl.TZ0.5b.iii: State the conjugate base of the hydroxide ion, OH–.
• 17N.2.sl.TZ0.5c: A student working in the laboratory classified HNO3, H2SO4, H3PO4 and HClO4 as acids based on...
• 18M.1.hl.TZ1.24: What describes HPO42−? A.     Amphiprotic but not amphoteric B.     Amphoteric but not...
• 18M.2.hl.TZ1.5c: Write an equation to show ammonia, NH3, acting as a Brønsted–Lowry base and a different equation...
• 18M.1.sl.TZ1.19: Which classification is correct for the reaction? H2PO4−(aq) + H2O(l) → HPO42−(aq) + H3O+(aq)
• 18M.2.sl.TZ2.2d: Outline why H3PO4/HPO42− is not a conjugate acid-base pair.

8.2 Properties of acids and bases

• 15M.1.sl.TZ1.21: Which gas in the atmosphere causes the pH of unpolluted rain to be approximately 6? A.   ...
• 14M.2.hl.TZ1.1d: Magnesium sulfate is one of the products formed when acid rain reacts with dolomitic limestone....
• 14M.2.hl.TZ1.8a: Outline how electrical conductivity can be used to distinguish between a...
• 14M.1.sl.TZ2.21: Which compound reacts with calcium oxide, CaO? A.     \({{\text{K}}_{\text{2}}}{\text{O}}\) B....
• 14M.2.sl.TZ1.1e: (i)     State the equation for the reaction of sulfuric acid with magnesium...
• 14M.2.sl.TZ1.7a: Outline how electrical conductivity can be used to distinguish between a...
• 13M.2.hl.TZ2.6d.i: Describe qualitatively the action of an acid–base indicator.
• 10N.1.hl.TZ0.27: Which solutions have a pH less than 7? I.    ...
• 10N.2.hl.TZ0.6c: A small piece of magnesium ribbon is added to solutions of nitric and hydrocyanic acid of the...
• 10N.2.sl.TZ0.6d: A small piece of magnesium ribbon is added to solutions of nitric and nitrous acid of the same...
• 09N.1.hl.TZ0.25: If \({\text{20 c}}{{\text{m}}^{\text{3}}}\) samples of...
• 09N.2.hl.TZ0.8b: Describe qualitatively the action of an acid-base indicator.
• 09M.2.hl.TZ2.7a.ii: State an equation for the reaction of magnesium carbonate with dilute hydrochloric acid.
• 16M.3.sl.TZ0.2b: (i) State the colour change of the indicator that the student would see during his titration...
• 16M.3.sl.TZ0.2c: Suggest why, despite preparing the solution and performing the titrations very carefully, widely...
• 16N.1.sl.TZ0.20: What occurs when solid sodium hydrogen carbonate reacts with aqueous sulfuric acid?  A. Bubbles...
• 16N.1.sl.TZ0.27: A student carried out a titration to determine the concentration of an acid and found that his...
• 16N.2.sl.TZ0.2c: 5.00 g of an impure sample of hydrated ethanedioic acid, (COOH)2•2H2O, was dissolved in water to...
• 16N.2.hl.TZ0.2c: 5.00 g of an impure sample of hydrated ethanedioic acid, (COOH)2•2H2O, was dissolved in water to...
• 17M.2.sl.TZ1.2f.ii: Suggest one disadvantage of using this smoke in an enclosed space.
• 17M.3.sl.TZ1.2a: Deduce why more heat was produced in mixture B than in mixture A.
• 17M.3.sl.TZ1.2b: Deduce why the temperature is higher in mixture C than in mixture D.
• 17M.2.sl.TZ2.1c.i: Some oxides of period 3, such as Na2O and P4O10, react with water. A spatula measure of each...
• 17M.2.hl.TZ2.8b.v: State a technique other than a pH titration that can be used to detect the equivalence point.
• 17N.3.sl.TZ0.2a: State an equation for the reaction of magnesium hydroxide with hydrochloric acid.
• 18M.2.hl.TZ2.2d.iii: Outline, using an equation, why sodium ethanoate is basic.
• 18M.1.sl.TZ1.20: What are the products of the reaction between sulfuric acid and sodium hydrogen carbonate? A.   ...
• 18M.1.sl.TZ2.19: Activity series of selected...

8.3 The pH scale

• 15M.1.sl.TZ2.22: \({\text{10.0 c}}{{\text{m}}^{\text{3}}}\) of a solution of a strong acid with a pH of 3 is added...
• 15M.2.sl.TZ1.6c.ii: Suggest the pH of the solutions formed in part (c) (i).
• 14M.2.hl.TZ1.6d: (i)     Determine the mass of copper produced at one of the electrodes in cell 2 if the tin...
• 14M.2.hl.TZ2.6d: (i)     One group suggested recording how long it takes for the pH of the solution to change by...
• 14M.1.sl.TZ1.22: A solution of \({\text{50 c}}{{\text{m}}^{\text{3}}}\) hydrochloric acid has a pH of 4. What is...
• 14M.2.sl.TZ2.5d: (i)     One group suggested recording how long it takes for the pH of the solution to change by...
• 14N.2.hl.TZ0.1a: Use the data in the table to identify the most acidic water sample.
• 14N.2.hl.TZ0.1c: Determine the ratio of \({\text{[}}{{\text{H}}^ + }{\text{]}}\) in bottled water to that in rain...
• 14N.2.hl.TZ0.1e: The acidity of non-polluted rain water is caused by dissolved carbon dioxide. State an equation...
• 14N.2.sl.TZ0.1a: Use the data in the table to identify the most acidic water sample.
• 14N.2.sl.TZ0.1c: Determine the ratio of \({\text{[}}{{\text{H}}^ + }{\text{]}}\) in bottled water to that in rain...
• 14N.2.sl.TZ0.1d: The acidity of non-polluted rain water is caused by dissolved carbon dioxide. State an equation...
• 13N.2.hl.TZ0.7d.i: Neelu and Charles decided to solve the problem by determining the volume of...
• 13N.2.hl.TZ0.7d.iv: Francisco and Shamiso decided to measure the pH of the initial solution, HQ, and they found that...
• 13N.2.sl.TZ0.5c.iii: Neelu and Charles decided to solve the problem by determining the volume of...
• 13N.2.sl.TZ0.5c.iv: Neelu and Charles decided to compare the volume of sodium hydroxide solution needed with those...
• 13N.2.sl.TZ0.5c.vi: Francisco and Shamiso decided to measure the pH of the initial solution, HQ, and they found that...
• 13M.2.hl.TZ1.1f.ii: With reference to the graph on page 4, describe the effect of increasing temperature on the...
• 13M.1.sl.TZ1.22: A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must...
• 13M.2.sl.TZ2.3a.i: Deduce the change in hydrogen ion concentration, \({\text{[}}{{\text{H}}^ + }{\text{]}}\).
• 12N.2.sl.TZ0.5b.vi: When lime was added to a sample of soil, the pH changed from 5 to 7. Calculate the factor by...
• 09N.2.hl.TZ0.8c.ii: Calculate the pH of a solution prepared by mixing \({\text{50.0 c}}{{\text{m}}^{\text{3}}}\) of...
• 09N.2.sl.TZ0.6c.i: Calculate the hydrogen ion concentrations in the two solutions and identify the stronger acid.
• 09N.2.sl.TZ0.6c.ii: Determine the ratio of the hydrogen ion concentrations in the two solutions X and Y.
• 09M.1.hl.TZ1.27: What is the correct expression for the ionic product constant of water, \({K_{\text{w}}}\)? A.  ...
• 09M.1.sl.TZ2.23: An example of a strong acid solution is perchloric acid, \({\text{HCl}}{{\text{O}}_{\text{4}}}\),...
• 11M.2.hl.TZ1.8d: Determine the pH of the solution resulting when \({\text{100 c}}{{\text{m}}^{\text{3}}}\) of...
• 11M.2.sl.TZ1.5c.iii: Black coffee has a pH of 5 and toothpaste has a pH of 8. Identify which is more acidic and deduce...
• 11M.1.sl.TZ2.22: The pH of a solution changes from \({\text{pH}} = 2\) to \({\text{pH}} = 5\). What happens to the...
• 12M.1.sl.TZ2.22: Three aqueous solutions of nitric acid are listed below. W.    ...
• 11N.2.hl.TZ0.4a: State the expression for the ionic product constant of water, \({K_{\text{w}}}\).
• 11N.1.sl.TZ0.22: What is the pH of the solution formed when \({\text{10 c}}{{\text{m}}^{\text{3}}}\) of HCl(aq)...
• 16M.2.sl.TZ0.2b: (i) State the equation for the reaction of this oxide of phosphorus with water. (ii) Predict how...
• 16M.2.hl.TZ0.1d: Impurities cause phosphine to ignite spontaneously in air to form an oxide of phosphorus and...
• 16N.2.sl.TZ0.2b: Suggest why it is more convenient to express acidity using the pH scale instead of using the...
• 17M.1.hl.TZ1.25: What is the pH of 1.0 × 10−3 mol dm−3 sodium hydroxide, NaOH(aq)? Kw = 1.0 × 10−14 A.     3 B....
• 17M.2.sl.TZ2.7b.iii: Calculate [H+] in the NaOH solution.
• 17N.1.sl.TZ0.18: What will happen if the pressure is increased in the following reaction mixture at...
• 17N.1.sl.TZ0.19: 10.0 cm3 of an aqueous solution of sodium hydroxide of pH = 10 is mixed with 990.0 cm3 of...
• 17N.1.sl.TZ0.20: Which statement is incorrect for a 0.10 mol dm–3 HCOOH solution? A. pH = 1 B. [H+] <<...
• 18M.1.hl.TZ1.25: What is the pH of a solution in which the hydroxide ion concentration is 1 × 10−11 mol dm−3 at...
• 18M.2.sl.TZ2.2c: Outline why pH is more widely used than [H+] for measuring relative acidity.

8.4 Strong and weak acids and bases

• 15M.2.hl.TZ1.8a: (i)     Outline the difference in dissociation between strong and weak acids of the same...
• 15M.1.sl.TZ1.22: Which compound is a strong acid? A.     \({\text{N}}{{\text{H}}_{\text{3}}}\) B.    ...
• 15M.2.sl.TZ1.6d: Describe three tests that can be carried out in the laboratory, and the expected results, to...
• 15M.2.sl.TZ2.5f.iv: Outline an experiment and its results which could be used to distinguish between a strong base...
• 14M.2.hl.TZ1.8a: Outline how electrical conductivity can be used to distinguish between a...
• 14M.2.hl.TZ2.5b.i: Chloric(I) acid is a weak acid, but hydrochloric acid is a strong acid. Outline how this is...
• 14M.2.hl.TZ2.5b.ii: State a balanced equation for the reaction of chloric(I) acid with water.
• 14M.2.hl.TZ2.5b.iii: Outline, in terms of the equilibrium in aqueous chlorine, why it is dangerous to use an acidic...
• 14M.2.hl.TZ2.5b.iv: Suggest why a covalent molecule, such as chloric(I) acid, is readily soluble in water.
• 14M.2.sl.TZ1.7a: Outline how electrical conductivity can be used to distinguish between a...
• 14M.2.sl.TZ2.4c.i: Chloric(I) acid is a weak acid, but hydrochloric acid is a strong acid. Outline how this is...
• 14M.2.sl.TZ2.4c.ii: State a balanced equation for the reaction of chloric(I) acid with water.
• 14M.2.sl.TZ2.4c.iii: Outline, in terms of the equilibrium above, why it is dangerous to use an acidic toilet cleaner...
• 14M.2.sl.TZ2.4c.iv: Suggest why a covalent molecule, such as chloric(I) acid, is readily soluble in water.
• 14N.1.sl.TZ0.22: A student adds 0.3 g of magnesium metal to equal volumes of hydrochloric acid and ethanoic acid...
• 14N.3.sl.TZ0.26a.ii: State and explain how the presence of a halogen substituent might affect the acidity of...
• 13N.1.hl.TZ0.26: Which group of three compounds contains only weak acids and bases?
• 13N.1.hl.TZ0.28: The table below shows data for the \({{K_{\text{a}}}}\) and \({{\text{p}}{K_{\text{b}}}}\) values...
• 13N.2.hl.TZ0.7d.iii: Neelu and Charles decided to compare the volume of sodium hydroxide solution needed with those...
• 13N.1.sl.TZ0.22: Which group of three compounds contains only weak acids and bases?
• 13N.2.sl.TZ0.5c.ii: Distinguish between the terms strong acid and weak acid.
• 13N.2.sl.TZ0.5c.v: State a suitable choice for both the strong acid and the weak acid.   Strong acid:   Weak acid:
• 13N.2.sl.TZ0.5c.vi: Francisco and Shamiso decided to measure the pH of the initial solution, HQ, and they found that...
• 13N.2.sl.TZ0.5c.vii: Suggest a method, other than those mentioned above, that could be used to solve the problem and...
• 13M.1.sl.TZ1.22: A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must...
• 13M.2.sl.TZ1.1d: A solution of HA is a weak acid. Distinguish between a weak acid and a strong acid.
• 13M.2.sl.TZ1.1e: Describe an experiment, other than measuring the pH, to distinguish HA from a strong acid of the...
• 13M.2.hl.TZ2.1h.i: Following the experiment, the students proposed the following hypothesis: “Since sulfuric acid...
• 13M.2.hl.TZ2.1h.ii: The students also explored the role of sulfuric acid in everyday processes and found that...
• 13M.2.hl.TZ2.6b.ii: Ethanoic acid is an example of a weak acid. Distinguish between a strong acid and a weak acid in...
• 13M.2.hl.TZ2.7e.ii: State why dilute sulfuric acid needs to be added in order for the current to flow in the...
• 13M.1.sl.TZ2.21: Which list contains only strong bases? A.     ammonia, sodium hydroxide, ethylamine B.   ...
• 13M.1.sl.TZ2.22: Which products would be formed when hydrochloric acid reacts with magnesium oxide? A.   ...
• 12N.1.hl.TZ0.28: Which salts will dissolve in water to give solutions with a pH above 7? I.    ...
• 12N.1.sl.TZ0.22: Which row correctly describes...
• 12N.2.sl.TZ0.5b.iv: Distinguish between a strong acid and a weak acid in terms of their dissociation in aqueous...
• 10N.2.hl.TZ0.6b: (i)     Distinguish between the terms strong and weak acid and state the equations used to show...
• 10N.2.hl.TZ0.6d: (i)     Calculate the volume of the sodium hydroxide solution required to react exactly with a...
• 10N.1.sl.TZ0.22: A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must...
• 10N.2.sl.TZ0.6c: The nitrite ion is present in nitrous acid, HNO2, which is a weak acid. The nitrate ion is...
• 10N.2.sl.TZ0.6e: (i)     Calculate the volume of the sodium hydroxide solution required to react exactly with a...
• 10N.2.sl.TZ0.6f: The graph below shows how the conductivity of the two acids changes with...
• 09N.2.sl.TZ0.6a.ii: In reaction B, identify the stronger base, \({\text{NH}}_2^ - \) or...
• 09N.2.sl.TZ0.6a.iii: In reactions A and B, identify the stronger acid, \({\text{NH}}_4^ + \) or...
• 09N.2.sl.TZ0.6b: Describe two different experimental methods to distinguish between aqueous solutions of a strong...
• 10M.2.hl.TZ2.7a: (i)     State the expression for the ionic product constant of water, \({K_{\text{w}}}\). (ii)  ...
• 10M.1.sl.TZ2.23: Which of the following are weak acids in aqueous solution? I.    ...
• 10M.2.sl.TZ2.6a: (i)     State the equilibrium constant expression for the dissociation of water. (ii)    ...
• 09M.1.sl.TZ1.22: For equal volumes of \({\text{1.0 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) solutions of...
• 09M.1.sl.TZ1.23: When equal volumes of four \({\text{0.1 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) solutions are...
• 09M.2.sl.TZ1.6d.i: Define the term weak acid and state the equation for the reaction of ethanoic acid with water.
• 09M.2.sl.TZ1.6d.ii: Vinegar, which contains ethanoic acid, can be used to clean deposits of calcium carbonate from...
• 09M.1.sl.TZ2.22: Which list contains only strong acids? A.    ...
• 09M.1.sl.TZ2.23: An example of a strong acid solution is perchloric acid, \({\text{HCl}}{{\text{O}}_{\text{4}}}\),...
• 09M.2.sl.TZ2.2c: Suggest one method, other than measuring pH, which could be used to distinguish between solutions...
• 11M.2.hl.TZ1.8a.i: Define the terms acid and base according to the Brønsted-Lowry theory. Distinguish between a weak...
• 11M.2.sl.TZ1.5c.i: Define the terms acid and base according to the Brønsted-Lowry theory and state one example of a...
• 11M.2.sl.TZ1.5c.ii: Describe two different methods, one chemical and one physical, other than measuring the pH, that...
• 11M.1.sl.TZ2.21: Which \({\text{0.10 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) solution would have the highest...
• 11M.2.sl.TZ2.5a.iv: Describe two different properties that could be used to distinguish between a...
• 12M.2.sl.TZ2.6a: Distinguish between the terms strong base and weak base, and state one example of each.
• 12M.2.sl.TZ2.6c: (i)     When ammonium chloride, \({\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl(aq)}}\), is added to...
• 11N.2.sl.TZ0.7b.iii: Z is an example of a weak acid. State what is meant by the term weak acid.
• 16M.1.hl.TZ0.27: Aqueous solutions of a weak acid and a...
• 16M.2.sl.TZ0.2b: (i) State the equation for the reaction of this oxide of phosphorus with water. (ii) Predict how...
• 16N.2.sl.TZ0.2a: Distinguish between a weak acid and a strong acid. Weak acid: Strong acid:
• 17M.1.sl.TZ1.20: Which 1.0 mol\(\,\)dm–3 solution has the highest pH? A.     Ammonium chloride B.     Sulfuric...
• 17M.2.sl.TZ1.4c: Hydrazine reacts with water in a similar way to ammonia. Deduce an equation for the reaction of...
• 17M.2.sl.TZ1.4d: Outline, using an ionic equation, what is observed when magnesium powder is added to a solution...
• 17M.2.hl.TZ2.8b.v: State a technique other than a pH titration that can be used to detect the equivalence point.
• 17M.3.sl.TZ2.14b.i: Oceans can act as a carbon sink, removing some CO2(g) from the atmosphere. CO2(g)...
• 17M.3.sl.TZ2.14b.ii: Describe how large amounts of CO2 could reduce the pH of the ocean using an equation to support...
• 17M.3.hl.TZ2.4a: Identify the other product formed.
• 17N.2.hl.TZ0.1e: Suggest why the enthalpy change of neutralization of CH3COOH is less negative than that of HCl.
• 18M.2.hl.TZ1.5a: Predict, giving a reason, a difference between the reactions of the same concentrations of...
• 18M.2.sl.TZ1.5a: Predict, giving a reason, a difference between the reactions of the same concentrations of...
• 18M.1.sl.TZ2.20: Which statement is correct? A.     A strong acid is a good proton donor and has a strong...
• 18M.2.sl.TZ2.2b.ii: State and explain the effect on the rate of reaction if ethanoic acid of the same concentration...

8.5 Acid deposition

• 14M.3.hl.TZ2.18a: State what is meant by the term acid deposition.
• 14M.3.hl.TZ2.18b: Describe, using equations, the mechanism of acid deposition caused by the oxides of nitrogen,...
• 14M.3.hl.TZ2.18c: All shellfish have a calcium carbonate shell. Discuss, including a balanced equation, the...
• 14M.3.sl.TZ2.15a: State what is meant by the term acid deposition.
• 14M.3.sl.TZ2.15b: Industrial processes, such as the burning of coal, generate non-metallic oxides of carbon and...
• 14M.3.sl.TZ2.15c: All shellfish have a calcium carbonate shell. Discuss, including a balanced equation, the...
• 13N.2.hl.TZ0.3c.i: Outline the source of these oxides.
• 13N.2.hl.TZ0.3c.ii: State one product formed from their reaction with water.
• 13N.2.hl.TZ0.3c.iii: State one environmental problem caused by these atmospheric pollutants.
• 13N.2.hl.TZ0.6e.ii: Sulfur dioxide is a significant contributor to acid deposition. Identify a major, man-made source...
• 13N.2.sl.TZ0.3b.i: Outline the source of these oxides.
• 13N.2.sl.TZ0.3b.ii: State one product formed from their reaction with water.
• 13N.2.sl.TZ0.3b.iii: State one environmental problem caused by these atmospheric pollutants.
• 13N.3.sl.TZ0.17a: The decrease in the pH of rainwater is mainly caused by oxides of non-metals, principally...
• 13N.3.sl.TZ0.17b: Explain, including an equation, the effect of the acid rain produced in (a) on certain stone...
• 13M.3.sl.TZ1.E3a: Discuss the damage to the environment caused by acid deposition.
• 13M.2.sl.TZ2.3b: Sulfuric acid present in acid rain can damage buildings made of limestone. Predict the balanced...
• 13M.3.sl.TZ2.E1a.i: State what is meant by the term acid deposition.
• 13M.3.sl.TZ2.E1a.iii: One effect of acid deposition is to decrease the pH of lake water. Suggest how this effect could...
• 12N.3.sl.TZ0.E1a: State one natural origin of acid deposition.
• 12N.3.sl.TZ0.E1b: State equations which represent chemical transformations of elemental sulfur into sulfurous acid,...
• 12N.3.sl.TZ0.E1c: Discuss the possible ways of decreasing acid deposition and its adverse effects on the environment.
• 09N.3.hl.TZ0.E3a: Outline the cause of the increase in NO levels between 5 and 8 am.
• 09N.1.sl.TZ0.23: Which pH value is that of an aqueous solution of carbon dioxide? A.     2.1 B.     5.6 C.   ...
• 09N.2.sl.TZ0.4c: In many cities around the world, public transport vehicles use diesel, a liquid hydrocarbon fuel,...
• 09M.2.sl.TZ2.2b: State one example of an acidic gas, produced by an industrial process or the internal combustion...
• 09M.3.sl.TZ2.E1a: Outline how the pollutant gases nitrogen(II) oxide, NO, nitrogen(IV) oxide,...
• 11M.2.hl.TZ1.8a.ii: Weak acids in the environment may cause damage. Identify a weak acid in the environment and...
• 11M.3.sl.TZ1.E1b.i: Outline the process responsible for the production of each acid and state an equation to show its...
• 11M.3.sl.TZ1.E1b.ii: Acid rain has caused damage to limestone buildings and marble statues. State an equation to...
• 12M.3.sl.TZ1.E2a: Explain, writing an appropriate equation, why, even in an unpolluted environment, rainwater is...
• 12M.3.sl.TZ1.E2b: (i)     Outline the major source of this gas, including an equation. (ii)     Describe,...
• 11N.3.hl.TZ0.E1c: Both of these air pollutants also contribute to acid deposition. Outline mechanisms for the...
• 11N.3.sl.TZ0.E1c: Both of these air pollutants also contribute to acid deposition. State one chemical equation for...
• 16M.1.sl.TZ0.20: Which of the following gases does not result in acid deposition? A.  CO2B.  NO2C.  NOD.  SO2
• 16M.2.sl.TZ0.2b: (i) State the equation for the reaction of this oxide of phosphorus with water. (ii) Predict how...
• 16N.2.sl.TZ0.3b: Suggest why the experiment should be carried out in a fume hood or in a well-ventilated laboratory.
• 17M.2.sl.TZ2.5c: State the equation for the reaction of NO2 in the atmosphere to produce acid deposition.
• 18M.2.hl.TZ1.5b: Dissolved carbon dioxide causes unpolluted rain to have a pH of approximately 5, but other...
• 18M.2.hl.TZ2.2e.i: Formulate the equation for the reaction of nitrogen dioxide, NO2, with water to form two acids.
• 18M.2.hl.TZ2.2e.ii: Formulate the equation for the reaction of one of the acids produced in (e)(i) with calcium...
• 18M.2.sl.TZ1.5b: Dissolved carbon dioxide causes unpolluted rain to have a pH of approximately 5, but other...