1. 1 Acids and Bases ICS Madrid

2. 2 Revision l When an acid reacts with a base, which compound(s) are formed? l What is the name of H 2 SO 4 ? l What is the formula for phosphoric acid? l Give four properties of acids. l Give four properties of bases.

3. 3 Acids and bases: revision l What is the charge on the hydroxonium ion? l If the hydrogen ion concentration is 10 -10 M, is the solution acidic, alkaline, or neutral? l If the [H + ] in a solution is 1 x 10 -1 mol/dm 3, what is the [OH - ]?

4. 4 pH and concentration of strong acids and bases l If the hydrogen ion concentration is 10 -7 M, what is the pH of the solution? l If the hydroxide ion concentration is 10 -10 M, what is the pH of the solution? l If the pH is 9, what is the concentration of the hydroxide ion?

5. 5 l If the pH is 6, what is the concentration of the hydrogen ion? l How many free hydrogen ions are there in one litre of water? l A litre of impure water has 10 -4 mol of hydroxide ions. What is the concentration of hydrogen ions in this sample of water?

6. 6 l What is the concentration of hydrogen ions in a neutral solution? l What is value of the ion-product constant for water? l For a solution to be classified as acidic, the hydrogen-ion concentration must be _____ than the hydroxide-ion concentration.

7. 7 questions l A solution in which the hydroxide ion concentration is 1 x 10 -4 M is ______. l A solution in which the hydroxide ion concentration is 1 x 10 -8 M is ______. l The formula of the hydrogen ion is often written as ______.

8. 8 l The products of self-ionization of water are _____. l Which is most basic: a) [OH 1- ] = 1 x 10 -4 M, or b) [H 1+ ] = 1 x 10 -11 M? l In a neutral solution, the [H 1+ ] is ______. l What is pH?

9. 9 l Which type of solution is one with a pH of 8? l An indicator is what type of compound? l In the reaction of aluminum bromide with ionised sodium bromide, which compound is the Lewis acid?

10. 10 l In the reaction of water with hydrogen ions, which compound is the Lewis base? l What is an acid according to Arrhenius? l What type of acid (mono-, di-, or triprotic) is sulphuric acid? l Which hydrogens can ionise in a compound?

11. 11 l Which hydroxides can ionise in a compound? l Which hydroxide compound yields the lowest concentration of hydroxide ions in aqueous solution: a) magnesium hydroxide, or b) potassium hydroxide?

12. 12 l Which acid is monoprotic: a) H 2 SO 4, or b) CH 3 COOH? l Which acid is dibasic a) H 2 SO 4, or b) CH 3 COOH?

13. 13 l Which is an Arrhenius base: a) LiOH, or b) CH 3 COOH? l What is an acid, according to Bronsted? l Which of the following is a Bronsted-Lowry base, but not an Arrhenius base: a) sodium hydroxide, or b) ammonia?

14. 14 l Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base: a) water, or b) sodium chloride? l What type of acid or base is the ammonium ion? l What is a conjugate acid made from?

15. 15 l What is transferred between a conjugate acid-base pair? l What is the term used to describe a substance that can be both an acid and a base? l In the reaction: NH 4 + + H 2 O  NH 3 + H 3 O +, water is acting as a(n) ______.

16. 16 l In the reaction: CO 3 - + H 2 O  HCO 3 - + OH -, the carbonate ion is acting as a(n) _____. l What does amphoteric mean? l Identify the Bronsted-Lowry bases in this reaction: H 2 S + H 2 O  H 3 O + + HS -.

17. 17 l Which of the following represents a Bronsted-Lowry conjugate acid-base pair: a) NH 4 1+ and NH 3 or b) SO 3 2- and SO 2 ? l According to the Bronsted-Lowry theory, water acts as a base when it ______.

18. 18 l What are the acids in the following equilibrium reaction: CN - + H 2 O  HCN + OH - l What is an “acid”, according to Lewis? l Which acid is only a Lewis acid, and not any other kind: a) water, or b) boron trifluoride?

19. 19 l A hydrogen ion is what type of acid? l A Lewis acid is a substance that can _____. l What is the acid dissociation constant of a weak acid, if a concentration of 0.3 M gives a hydrogen ion concentration of 0.001 M?

20. 20 l What is the hydrogen ion concentration, if the acid dissociation constant is 1 x 10 -6 M and the acid concentration is 0.01 M? l What characterizes a “strong” acid or base?

21. 21 l The acid dissociation constant for an acid dissolved in water is equal to the ______. l What is another name for the acid dissociation constant? l What is the value of the acid dissociation constant for a weak acid?

22. 22 l How many ionization constants are associated with sulphuric acid? l Which ionization constant is the largest for phosphoric acid?

23. 23 l Which of the following acids can be concentrated, but is always weak: a) ethanoic acid b) nitric acid? l K a for HF = 6.7 x 10 -4. If we have a 0.1 M solution, then [HF] is _______ than [H + ] x [F - ].

24. 24 l A 0.12 M solution of an acid that ionises only slightly in solution would be termed ___ and ___. l Which of the following pairs consists of a weak acid and a strong base: a) sulphuric acid and sodium hydroxide, or b) acetic acid and sodium hydroxide?

25. 25 l What does “strong” mean when referring to acids and bases? l Ethanoic acid ionizes in water as: 1%  CH 3 COOH + H 2 O  CH 3 COO - + H 3 O + @ 99% The ethanoate ion (CH 3 COO - ) is therefore a good _______

26. 26 l A 12.0 M solution of an acid that ionises completely in solution would be termed ___ and ____.