Acids

• OCR-A acids are proton donors and bases are proton acceptors.
• When acids and bases react with water, they form a reversible reaction.
• Acids can be represented as HA, which stands for an acid plus water and forms a hydroxo ion, also known as a hydronium ion.
• Bases can be represented as BH plus, which forms an OH minus and makes the base alkaline.
• Acids produced as H+ ions, while bases produce OH- ions.
• Acids and bases can be categorized as weak or strong.
• Weak acids include ethanoic acid and carboxylic acids with a COOH group at the end.
• These reactions are reversible and dissociate, meaning they break up.
• Strong acids, also known as mineral acids, include hydrochloric acid, sulfuric acid, and nitric acid.
• These acids are not reversible and are assumed to dissociate fully.
• Fill the volumetric flask to the graduation line, measure to the bottom of the meniscus, and mix thoroughly.
• Titrations can be used to work out the concentration of an acid or an arc.
• 18.3 centimeters cubed of naught 0.25 moles DMT HCl was required to neutralize 25 centimeters cubed of tastic hydroxide.
• The mass of solid sodium hydroxide required to make 250 centimeters cubes of 0.75 moles PDM cubed sodium hydroxide solution is 0.75 moles times the relative formula mass in grams per mole.
• To fully dissolve a solid sodium hydroxide, use deionized water and stir to ensure the solid is dissolved fully.
• Transfer the dissolved sodium hydroxide into a volumetric flask using a funnel to avoid losing any of the product.
• The concentration of potassium hydroxide can be calculated using titration calculations.
• Strong bases include sodium hydroxide and potassium hydroxide.
• These bases are also assumed to dissociate fully.
• A weak base is an example of ammonia.
• These reactions are weak and rely on water.
• The ionic equation for the reaction of lithium carbonate with nitric acid is: Li2CO3 + 2HNO3 → LiNO3 + CO2 + H2O.
• Magnesium oxide reacts with hydrochloric acid to form magnesium chloride and water.
• Metal hydroxides react with acids to form salt and water, which is similar to oxides and hydroxides.
• In titrations, molar calculations are used to determine the concentration of an acid or base in a solution.
• Metal carbonates react with acids to form salt, water, and carbon dioxide, which is different from oxides and hydroxides.
• Lithium carbonate reacts with nitric acid to form lithium nitrate, carbon dioxide, and water.
• Sodium sulfate, Na2SO4, reacts with water to form sodium sulfate and water.
• Metal oxides react with acids to form salt and water, which is the same as oxides and hydroxides.
• The number of moles in a substance in a solution can be calculated from concentration and volume, using the equation: moles = concentration * volume.
• The ionic equation for the reaction of sodium sulfate with water is: Na2SO4 + H2O → Na2SO4 + H+ + OH-.
• The ionic equation for the reaction of magnesium oxide with hydrochloric acid is: MgO + HCl → MgCl2 + H2O.
• Metals react with acids to form salts and hydrogen gas.
• The ionic equation for the reaction between calcium and sulfuric acid is Ca + H2SO4 → CaSO4 + H2.
• Calcium reacts with sulfuric acid to form calcium sulfate and hydrogen.
• Phosphoric acid is a triprotic acid, producing three protons in solution.
• The ionic equation can be simplified by removing spectator ions.
• Salts are the other neutral of an acid-base reaction.
• Examples of acids include hydrochloric acid, nitric acid, and sulfuric acid.
• Nitric acid is a monoprotic acid, producing one mole of H+ ions in solution.