Acids bases and salts
Cards (30)
- Acid + Metal → Salt + Hydrogen
- Acid + Base → Salt + Water
- Acid + Carbonate → Salt + water + carbon dioxide
- Acid + alkali → Salt + water
- Acid + ammonia → Salt
- Hydrochloric acid = HCl (aq)
- Sulfuric acid = H2SO4
- Nitric acid = HNO3 (aq)
- A salt is a compound formed when an H+ in an acid is replaced with a postive (metal) ion
- A hydrated salt has water within its structure
- Anhydrous salt contains no water molecules
- Water of crystallisation is when molecules are trapped in a lattice (crystal)
- A base is a solution that accepts protons· A base that is soluble in water is an alkali· Alkali form OH- ions in water
- An acid releases H+ ions when added to water. A proton donor
- Strong acids fully dissociate when disolved in water
- Weak acids partiallly dissociate when dissolved in water· This means that a strong acid produces more H+ ions has a lower pH than a weak acid with the same concentration
- Molecular formula = the actual number of atoms of each element in a molecule, a multiple of the emperical formula
- Emperical formula = the simplest whole number ratio of atoms of each element in a compound
- Number of moles of a substance = Mass of a substance / Mr of substance
- Molar mass is the mass of one mole of a substance in grams.
- Moles = Number of particles/6.02x10^23
- Relative isotopic mass = The mass of one isotope compared to 1/12 the mass of carbon 12
- Relative atomic mass = The mean mass of an atom of an element compared to 1/12th the mass of an atom of carbon-12
- Mass number = number of protons + number of neutrons in an atom of an element
- Atomic number = number of protons in an atom of an element.
- Isotope = Atom of the same element with a different number of neutrons but the same number of protons
- PV = nRT· P = Pressure pa· V = vol cm· n = Number of moles· R = Gas constant Jmol-1k-1· T = temprature kelvin
- Moles = Volume of gas / Volume of container x 24
- Moles = Volume x concentration
- Number of molesof gas = volume of gas / 24