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Acids and Bases
| Acids | Bases | |
|---|---|---|
| Taste and feel | Sour | Bitter and soapy |
| Ion in water | Give \( \ce{H+} \) (shown as \( \ce{H3O+} \)) | Give \( \ce{OH-} \) |
| Litmus | Turn blue litmus red | Turn red litmus blue |
| Phenolphthalein | Colourless | Pink |
| Methyl orange | Red | Yellow |
| Examples | HCl, \( \ce{H2SO4} \), \( \ce{HNO3} \), \( \ce{CH3COOH} \) | NaOH, KOH, \( \ce{Ca(OH)2} \), \( \ce{NH4OH} \) |
A base that dissolves in water is called an alkali. Every alkali is a base, but not every base is an alkali.
Reactions of Acids and Bases
1. Acid with metal: salt and hydrogen. \( \ce{Zn + 2HCl -> ZnCl2 + H2} \). The hydrogen burns with a pop sound.
2. Acid with metal carbonate or bicarbonate: salt, water and carbon dioxide. \( \ce{Na2CO3 + 2HCl -> 2NaCl + H2O + CO2} \). Carbon dioxide turns lime water milky.
3. Acid with base (neutralisation): salt and water. \( \ce{NaOH + HCl -> NaCl + H2O} \).
4. Acid with metal oxide: salt and water. Base with non-metal oxide: salt and water. \( \ce{Ca(OH)2 + CO2 -> CaCO3 + H2O} \).
5. Zinc and aluminium also react with strong alkalis giving hydrogen. \( \ce{Zn + 2NaOH -> Na2ZnO2 + H2} \).
Strength and pH
1. Strong acids and bases ionise almost completely in water. Weak acids and bases ionise only a little. Strength is about ionisation, not concentration.
2. The pH scale runs from 0 to 14. pH below 7 is acidic, 7 is neutral and above 7 is basic. Lower pH means more hydrogen ions. At 25 degrees C, pH + pOH = 14.
3. Dilution: always add acid to water slowly with stirring, because mixing is highly exothermic.
4. Importance of pH: stomach acid is about pH 1.5 to 3, antacids are weak bases, tooth decay starts below pH 5.5, and plants grow best in soil of suitable pH.
5. Natural acids: citric in lemon, tartaric in tamarind, lactic in curd, oxalic in tomato, methanoic (formic) in ant and nettle stings, ethanoic in vinegar.
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Acids, Bases and Salts Concepts and Summary for Class 10 Chemistry
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