Acids and Alkalis part 2 Flashcards
Recall the chemical formulae of some common compounds.
Water: H₂O
Sodium chloride: NaCl
Hydrochloric acid: HCl
Sodium hydroxide: NaOH
Recall and use state symbols.
State symbols include (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous.
Balance chemical equations.
Adjust coefficients in chemical equations so the number of atoms for each element is equal on both sides.
Recall that alkalis are soluble bases.
Alkalis are bases that dissolve in water to produce hydroxide ions (OH⁻).
Describe the reactions of alkalis with acids.
Alkalis react with acids in neutralization reactions, producing water and a salt.
Explain what happens to the ions from acids and alkalis during neutralisation.
Hydrogen ions (H⁺) from the acid react with hydroxide ions (OH⁻) from the alkali to form water.
Explain why titration is used to prepare soluble salts.
Titration accurately measures the amount of acid and alkali needed to neutralize each other, ensuring a pure salt solution.
Write balanced ionic equations.
For example, for hydrochloric acid reacting with zinc:
Zn + 2H^+ → Zn^2+ + H2
Describe the test for hydrogen.
A lit splint makes a popping sound in the presence of hydrogen gas.
Describe how to carry out an acid–alkali titration.
Use a burette to add acid to an alkali with an indicator, slowly reaching the endpoint where neutralization is complete.
Explain the general reaction between an acid and a metal to produce a salt and hydrogen.
Acid + Metal → Salt + Hydrogen
Describe the test for carbon dioxide.
Carbon dioxide turns limewater cloudy when bubbled through it.
Explain the general reaction between an acid and a metal carbonate to produce a salt, water, and carbon dioxide.
Acid + Metal Carbonate → Salt + Water + Carbon Dioxide
Recall the general rules for the solubility of common substances in water.
Most nitrates are soluble.
Most chlorides are soluble except silver and lead chlorides.
Most sulfates are soluble except barium, lead, and calcium sulfates.
Carbonates are generally insoluble except sodium, potassium, and ammonium carbonates.
Predict whether or not a precipitate will form from two solutions.
A precipitate forms if the product of two ions is insoluble according to solubility rules.
