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acids and bases:
chemistry - acids and bases:
Question | Answer |
---|---|
1. Bronsted-Lowry acid? | proton donor |
2. Bronsted-Lowry base? | proton acceptor |
3. Bronsted-Lowry acid-base reaction? | reaction involving the transfer of a proton |
4. Monoprotic acid? | released one H+ per molecule |
5. Diprotic acid? | releases two H+ per molecule |
6. Examples a monoprotic acid? | HCl HNO3 CH3COOH |
7. Example of a diprotic acid? | H2SO4 |
8. pH? | -log(10)[H+] |
9. [H+]? | 10^-pH |
10. Decimal places for pH? | 2DP |
11. What is Kw used for? | strong bases |
12. Kw calculation? | 10^-14/ [OH-] then put into pH |
13. Calculating pH of solution | [OH-] x (old volume / new volume) then put into Kw then into pH |
14. Nitric acid and hydrochloric acids are? | strong monoprotic acids |
15. Carboxylic acids are? | weak monoprotic acids |
16. Sulfuric acids is? | strong diprotic acid |
17. sodium hydroxide and potassium hydroxide are? | strong monoprotic bases |
18. ammonia is? | weak monoprotic base |
19. Ba(OH)2 is? | strong diprotic base |
20. What is Ka used for? | weak acids |
21. Calculating Ka? | Ka = [H+]^2 / [HA] |
22. Pka? | -log(10)(Ka) |
23. How to calculate Ka from pKa? | Ka = 10^-pKa |
24. Units for Ka? | moldm^-3 |
25. Bigger Ka value means? | stronger acid |
26. Smaller Ka value means? | weaker acid |
27. Bigger pKa value means? | bigger pKa means weaker acid |
28. Smaller pKa value means? | smaller pKa means stronger acid |
29. Correlation between temperature, Kw and pH? | as temperature increases, kW increases so Ph decreases to oppose change when the equilibrium shifts right |
30. Strong acid definition? | covalent molecules that dissolve in water + completely dissociate |
31. Where does the equilibrium lie for a reaction with a strong acid? | fully dissociate so lies far right |
32. Weak acid definition? | covalent molecules that dissolve in water + partially dissociate |
32. Where does the equilibrium lie for a reaction with a strong acid? | lies far left so is a reversible reaction arrow |
33. Definition of a base? | any substance that reacts with an acid and accepts a proton from it |
34. Definition of an alkali? | any substance which produces OH- when in aqueous solution (all alkalis are bases) |
35. If Ka<1? | then acid is weak if Ka<1 |
36. If Ka>1? | then acid is strong is Ka>1 |
37. Calculation for new concentration? | new concentration = (amount in moles of solute) / (new total volume of solution) x 100 |
38. Endpoint? | point in titration when volume of reactant (acid/alkali) added causes colour of indicator to change |
39. Indicator? | made from different dyes which change colour at different [H+(aq)] -> change over narrow pH range |
40. Equivalence point? | point rapid change of pH showing vertical inflection (volume same no. mol of H+ and OH-) |
41. Arrow used for indicators? | reversible |
42. Inflection? | vertical curve showing rapid pH change |
43. Strong acid vs Weak base? | equivalence point pH 3-8 initial = pH 1 |
44. Strong acid vs Strong base? | equivalence point pH 3-10 initial = pH 1 |
45. Weak acid vs Strong base? | equivalence point pH 6-10 initial = pH 3 |
46. Weak acid vs Weak base? | equivalence point pH 3-4 no major inflection |
47. Steps for neutralisation? | 1- moles H+ and OH- 2- which in excess 3- conc = (left over mol/total vol) 4. put into pH |