Reactions with acids

• An indicator is a substance added to identify the endpoint of a titration by exhibiting a sharp change in color at the equivalence point.
• Hydrochloric acid reacts with magnesium carbonate to form magnesium chloride, water, and carbon dioxide.
• The reaction between an alkali (metal hydroxide) and an acid produces a salt and water only.
• Common indicators include phenolphthalein, methyl orange, and bromothymol blue.
• Metal oxides react with dilute acid to form salts, water, and oxygen gas.
• Acid + metal carbonate → salt + water + CO2
• Acid + metal carbonate → salt + water + carbon dioxide
• Acid strength refers to how easily an acid donates hydrogen ions (protons) into solution.
• The pH scale measures acidity or alkalinity on a logarithmic scale from 0-14, where 7 is neutral, less than 7 is acidic, and greater than 7 is basic.
• Stronger acids have higher concentrations of H+ ions compared to weaker acids.
• When magnesium carbonate is placed in hydrochloric acid, bubbles are produced due to the formation of carbon dioxide gas.
• Methyl orange changes from yellow to red when it reaches its pKa value.
• Phenolphthalein changes from colorless to pink when it reaches its pKa value.
• Stronger bases have higher pKa values than weaker ones.
• Acid + metal hydroxide → salt + water
• Base + acid → salt + water
• Weak acids produce weak bases when they dissociate.
• Acid + metal oxide → salt + water + O2
• Arrhenius bases are substances that release OH- ions into solution upon ionization.
• Bases can be classified as Arrhenius or Bronsted-Lowry based on their ability to donate H+ ions.
• Metal carbonates react with strong acids to form salts, water, and CO2 gas.
• When a strong acid reacts with a strong base, the products are a soluble salt and water.
• A strong acid reacts completely with a strong or weak base, while a weak acid only partially reacts with a strong or weak base.
• The reaction between an acid and a base produces a salt and water.
• The reaction between an acid and a base is neutralization, which produces a salt and water.
• The reaction between sodium and water produces sodium hydroxide (NaOH) and hydrogen gas (H2).
• Bases neutralize acids by donating OH- ions.
• A weak acid has a lower concentration of H+ ions compared to a strong acid at the same concentration.
• Alkali metals react vigorously with cold water to produce hydrogen gas and an alkaline solution.
• A titration curve shows the relationship between the volume of added base and the corresponding pH values obtained during a titration reaction.
• Acid strength can be determined by measuring the concentration of H+ ions released into solution.
• Bronsted-Lowry bases accept protons (H+) from other molecules or ions, forming H bonds.
• Metal oxides react with acids to form salts and water.
• Lewis bases donate pairs of electrons to form covalent bonds with Lewis acids.
• The pH scale is used to measure the concentration of hydrogen ions (H+) in a substance, ranging from 0 (very acidic) to 14 (very alkaline).
• The reaction between an acid and a base is neutralized by adding another acid or base until no more bubbles appear.
• Amphoteric substances can act as both an acid and base under different conditions.
• The reaction between an acid and a base produces a neutralization reaction where the hydrogen from the acid combines with the hydroxyl group from the base to form water.
• The reaction between an acid and a base produces a neutralization reaction.
• Aqueous solutions of metals react vigorously with dilute nitric acid (HNO3) to form nitrate salts and oxygen gas.