Acids and Bases
No description yet. This curated deck is ready for daily study.
Card preview (24)
What is a Bronsted-Lowry Acid?
A proton donor
What is a Bronsted-Lowry Base?
A proton acceptor
What does an Acid + Hydroxide produce?
Salt and water e.g. CH3COOH(aq) + NaOH(aq) NaCH4COO(aq) + H2O(l)
What does a metal oxide and acid produce?
Salt and water
What do acids and ammonia react to produce?
A salt e.g. HCl(aq) + NH3 (aq) NH4Cl(aq)
What do acids and carbonates produce?
Salt, water, Carbon dioxide
What do acids and hydrogen carbonates produce?
Salt, water, Carbon dioxide
State the color of Universal indicator at pH: 0, 4, 7, 10, 14
0 - red 4 - orange 7 - green 10 - blue 14 - purple
What does it mean if a substance is strong?
completely dissociated into ions
What does it mean if a substance is concentrated?
a high number of moles of solute per litre (dm3 ) of solution
What does it mean if a substance is corrosive?
Chemically reactive
What happens when a solution of pH 1 is diluted 10 times
It becomes pH 2
Formula for pH
-log(base 10) [ H+ ion conc.]
Formula for [H+]
10^(-pH)
What is [H+] x [OH-]
1 x 10^(-14)
How does sulphuric oxide get into the atmosphere and what is its effect?
Sulfur dioxide occurs naturally from volcanoes. It is produced industrially rom the combustion of sulfur-containing fossil fuels and the smelting of sulfde ores. S(s) + O2 (g) -> SO2 (g) In the presence ofsunlight sulfur dioxide is oxidized to sulfur trioxide. SO2 (g) + 1/2O2 (g) ->SO3 (g) The oxides can react with water in the air to form sulfurous acid and sulfuric acid: SO2 (g) + H2O(l) -> H2SO3 (aq) and SO2 (g) + H2O(l) -> H2SO4 (aq
How do Nitrogen oxides get into the atmosphere and what is the effect?
Nitrogen oxides occur naturally from electrical storms and bacterial action. Nitrogen monoxide is produced in the internal combustion engine and in jet engines. N2 (g) + O2 (g) -> 2NO(g) Oxidation to nitrogen dioxide occurs in the air. 2NO(g) + Ow (g) -> 2NO2 (g) The nitrogen dioxide then reacts with water to form nitric acid and nitrous acid: 2NO2 (g) + H2O(l) -> HNO3 (aq) + HNO2 (aq) or is oxidized directly to nitric acid by oxygen in the presence of water: 4NO2(g) + O2 (g) + 2H2O(l) 4HNO3 (aq)
What is acid deposition?
Pure rainwater is naturally acidic with a pH o 5.65 due to the presence o dissolved carbon dioxide. Acid rain since acid rain is defned as rain with a pH less than 5.6. It is the oxides o sulur and nitrogen present in the atmosphere which are responsible or acid deposition
How do we counteact acid deposition?
• Lower the amounts o NO and SO ormed, e.g. by improved engine design, the use o catalytic converters, and removing xx sulur beore, during, and ater combustion o sulur-containing uels. 2, Liming o lakes adding calcium oxide or calcium hydroxide (lime) neutralizes the acidity, increases the amount o calcium ions and precipitates aluminium rom solution. This has been shown to be eective in many, but not all, lakes where it has been tried.
What is a lewis acid?
Substances which accept a pair of electrons
What is a lewis base?
Substances which donate a pair of electrons.
How does the Kw value change with increasing temperature?
Kw increase with temp.
Formula for pOH
-log(base 10) [OH- conc]
Formula for pKw
-log(base 10) [Kw] pKw = pH + pOH = 14 pKa + pKb = pKw