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Acid-Base Equilibria
AQA A Level Chemistry
Question | Answer |
---|---|
What are the Bronsted Lowery definitions of an acid and a base? | An Acid is a proton donor and a Base is a proton acceptor |
What is the conjugate acid of NH3? | NH4+ |
What is the conjugate base of CH3COOH? | CH3COO- |
What is the conjugate acid of HNO3? | H2NO3+ |
Names the Acid Base conjugate pairs in this reaction H3O+ + HSO4- → H2SO4 + H2O | H3O+ Acid H2O Base. HSO4- Base H2SO4 acid. |
Give the formula of Hydroxonium Ion | H3O+ |
Describe the bonding in the Hydroxonium Ion | Covalent and Dative Covalent Bonding |
Define a strong acid | An acid that completely dissociates in aqueous solution |
Define a weak acid | An acid that partially dissociates in aqueous solution. |
What is the general formula for the acid dissociation constant? | Ka= [H+][A-]/ [HA] |
What is the definition of pH? | pH= -log10[H+(aq)] |
What is the pH of a solution with a [H+] of 1.23x10-4 mol dm-3 | 3.91 |
What is the pH of a solution with a [H+] of 7.89 x10-15 mol dm-3 | 14.1 |
Rearrange the definition of pH to make [H+(aq)] the subject | [H+(aq) = 10-pH |
What is the [H+(aq)] of a solution with a pH of 9.2? | 6.31x10-10 moldm-3 |
Calculate the pH of the solution formed by adding of 250 cm3 of water to 50 cm3 of 0.200 mol dm-3 HNO3 | 1.48 |
Calculate the pH of the following solution 100 g dm-3 H2SO4 | -0.31 |
What is the formula of the ionic prodcut of water Kw | Kw = [H+][OH-] |
What is the relationship between pH and pOH? | pH + pOH = 14 |
Calculate the pH of the following solution: 0.20 mol dm-3 Ba(OH)2 | 13.6 |
Calculate the pH of the solution formed by the addition of 100 cm3 of water to 25 cm3 of 0.100 mol dm-3 NaOH | 12.3 |
Write a general equation for the dissociation of a weak acid | "HA(aq) → A¯(aq) + H+(aq) |
What are the two assumptions one makes when calculating the pH of a weak acid? | "The amount of HA at equilibrium is equal to the amount of HA put into the solution and [H+(aq)]= [A¯(aq)] |
What does the general formula for the acid dissociation constant become when these two assumptions are applied? | "Ka = [H+(aq)]2/[HA(aq)] |
Write the fomula you use to calculate the pH of a weak acid. | [H+(aq)] = √ [HA(aq)] Ka |
Calculate the pH of the following weak acid: 0.200 mol dm-3 butanoic acid (Ka = 1.51 x 10-5 mol dm-3) | 2.76 |
Calculate the Ka value for phenylethanoic acid given that a 0.100 mol dm-3 solution has a pH of 2.66 | 4.79 x 10-5 mol dm-3 |
Write the seven steps for the calculation of the pH of a solution formed by the reactions between a weak acid and a strong base if the acid is in excess. | Calculate moles HA (it is still HA and not H+ as it is a weak acid), Calculate moles OH, Calculate moles XS HA, Calculate moles HA left and A- formed, Calculate [HA] leftover and [A-] formed, Use Ka to find [H+], Find pH |
Write the six steps for the calculation of the pH of a solution formed by the reactions between a weak acid and a strong base if the OH- is in excess. | Calculate moles HA (it is still HA and not H+ as it is a weak acid), Calculate moles OH, Calculate moles XS OH, Calculate [OH-], Use Kw to find [H+], Find pH |
Calculate the pH of the solution formed when 50 cm3 of 0.500 mol dm-3 ethanoic acid (pKa = 4.76) is added to 50 cm3 of 0.250 mol dm-3 KOH | 4.76 |
What is a titration? | " a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete. |
What is the equivalence point of a titration? | "the point at which the titration reaction is complete |
Define what types of substances are suitable to be indicators | They are weak acids whose conjugate base is a different colour to the acid. |
How do you select a suitable indicator for a particular type of titration. | The pH range of the suitable indicator fits within the vertical section of the titration curve. |
"Methyl Orange has a pH range of 3.1-4.4 for what types of titration Is it suitable? | Strong acid, Strong base. Strong acid, Weak Base |
"Phenolpthalein has a pH range of 8.3-10.0 for what types of titration Is it suitable? | Strong acid, Strong base. Weak acid, Strong Base |
What is the typical equivalence point of a strong acid strong base titration? | 7 |
What is the typical equivalence point of a strong acid weak base titration? | 5 |
What is the typical equivalence point of a weak acid strong base titration? | 9 |
What is the typical pH range of the vertical section of a strong acid strong base titration curve? | 3 to 10 |
What is the typical pH range of the vertical section of a weak acid strong base titration curve? | 7 to 11 |
What is the typical pH range of the vertical section of a strong acid weak base titration curve? | 3 to 7 |
Explain how one can use a titration curve to calculate Ka of a weak acid. | "Half way to the equivalence point [HA(aq)] = [A¯ (aq) ], so pKa = pH |
Define what is a buffer solution | "Solutions which resist changes in pH when small quantities of acid or alkali are added. |
Describe the most common way of making a buffer solution. | "A buffer solution is made from a weak acid and the salt of the weak acid. |
Describe an additional way of making a buffer solution | "Adding a measured amount of hydroxide ions to a weak acid |
What are the two assumption we make when calculate the pH of a buffer solution. | "All the A- ions come from the salt, Almost all the HA molecules put into the buffer remain unchanged |
What does the general formula for the acid dissociation constant become when the assumptions for a buffer solution are applied? | " Ka = [H+(aq)] x [salt]/ [acid] |
"What happens if an acidic substance is added to a buffer? | " "Any rise in [H+(aq)] disturbs the equilibrium. Some A-(aq) ions from the salt react with the extra H+(aq) ions to form HA(aq) and water. A significant fall in pH is prevented. |
Calculate the pH of the following buffer solutions made by mixing 50.0 cm3 of 1.00 mol dm-3 methanoic acid (Ka = 1.78 x 10-4 mol dm-3 with 20.0 cm3 of 1.00 mol dm-3 sodium methanoate | 3.35 |
"Calculate the pH of the following buffer solution made by mixing 100 cm3 of 1.00 mol dm-3 ethanoic acid (Ka = 1.78 x 10-4 mol dm-3 ) is mixed with 50.0 cm3 of 0.8000 mol dm-3 sodium hydroxide. | " 3.57 |