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Acids and Bases

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

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Acids and Bases

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  1. Acids and Bases ICS Madrid

  2. Revision • When an acid reacts with a base, which compound(s) are formed? • What is the name of H2SO4? • What is the formula for phosphoric acid? • Give four properties of acids. • Give four properties of bases.

  3. Acids and bases: revision • What is the charge on the hydroxonium ion? • If the hydrogen ion concentration is 10-10 M, is the solution acidic, alkaline, or neutral? • If the [H+] in a solution is 1 x 10-1 mol/dm3, what is the [OH-]?

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

  5. If the pH is 6, what is the concentration of the hydrogen ion? • How many free hydrogen ions are there in one litre of water? • 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. What is the concentration of hydrogen ions in a neutral solution? • What is value of the ion-product constant for water? • For a solution to be classified as acidic, the hydrogen-ion concentration must be _____ than the hydroxide-ion concentration.

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

  8. The products of self-ionization of water are _____. • Which is most basic: a) [OH1-] = 1 x 10-4 M, or b) [H1+] = 1 x 10-11 M? • In a neutral solution, the [H1+] is ______. • What is pH?

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

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

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

  12. Which acid is monoprotic: a) H2SO4, or b) CH3COOH? • Which acid is dibasic • a) H2SO4, or b) CH3COOH?

  13. Which is an Arrhenius base: a) LiOH, or b) CH3COOH? • What is an acid, according to Bronsted? • Which of the following is a Bronsted-Lowry base, but not an Arrhenius base: a) sodium hydroxide, or b) ammonia?

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

  15. What is transferred between a conjugate acid-base pair? • What is the term used to describe a substance that can be both an acid and a base? • In the reaction: NH4+ + H2O  NH3 + H3O+, water is acting as a(n) ______.

  16. In the reaction: CO3- + H2O  HCO3- + OH-, the carbonate ion is acting as a(n) _____. • What does amphoteric mean? • Identify the Bronsted-Lowry bases in this reaction: H2S + H2O  H3O+ + HS-.

  17. Which of the following represents a Bronsted-Lowry conjugate acid-base pair: a) NH41+ and NH3 or b) SO32- and SO2? • According to the Bronsted-Lowry theory, water acts as a base when it ______.

  18. What are the acids in the following equilibrium reaction: CN- + H2O  HCN + OH- • What is an “acid”, according to Lewis? • Which acid is only a Lewis acid, and not any other kind: a) water, or b) boron trifluoride?

  19. A hydrogen ion is what type of acid? • A Lewis acid is a substance that can _____. • 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. 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? • What characterizes a “strong” acid or base?

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

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

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

  24. A 0.12 M solution of an acid that ionises only slightly in solution would be termed ___ and ___. • 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. What does “strong” mean when referring to acids and bases? • Ethanoic acid ionizes in water as: • 1% • CH3COOH + H2O  CH3COO- + H3O+ • @ 99% • The ethanoate ion (CH3COO-) is therefore a good _______

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

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