Class 10 Chemistry Chapter 2 Important Question

• Here are the detailed class 10 chemistry chapter 2 important questions with answers to help you prepare for your exams.
• Important Multiple Choice Questions of Chapter Number 10: Acid Bases and Salts of Chemistry class 10th Urdu Medium.
• Important Short Questions of Chapter Number 10: Acid Bases and Salts of Chemistry class 10th Urdu Medium.
• Uses of Bases: Sodium hydroxide, is used for manufacturing of soap.
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• Calcium hydroxide, is used for manufacturing of bleaching powder, softening of hard water and neutralizing acidic, soil and lakes due to acid rain.
• Potassium hydroxide, is used in alkaline batteries.
• Magnesium hydroxide, is used as a base to neutralize acidity in the stomach. It is also used for the treatment of bee’s stings.
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• Aluminium hydroxide, is used as foaming agent in fire extinguishers.
• Ammonium hydroxide, is used to remove grease stains from clothes.
• pH SCALE: Concentration of hydrogen ion [H+] in pure water is the basis for the pH scale. Water is a weak electrolyte because it ionizes very slightly into ions in a process called auto-ionization or self-ionization;
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• As it is difficult to deal with such small figures having negative exponents, so it is convenient to convert these figures into a positive figure using a numerical system. It is taking the common (base-10) logarithm of the figure and multiplying it with -1. ‘p’ before a symbol means’ negative logarithm of the symbol. So ‘p’ before H means negative logarithm of [H+]. Therefore, pH is the negative logarithm of molar concentration of the hydrogen ions.
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• Since the pH scale is logarithmic, a solution of pH 1 has 10 times higher concentration of [H+] than that of a solution of pH 2; 100 times than that of a solution of pH 3 and so on. Hence, low pH value means strong acid while high pH value means a strong base and vice versa. Conclusion
• pH of a neutral solution is always 7.
• Acidic solutions have pH less than 7.
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• Basic solutions have pH value greater than 7.
• pH and pOH values range from 0 to 14.
• Uses of pH: It is used to determine acidic or basic nature of a solution.
• It is used to produce medicines, culture at a microbiological particular concentration of H+ ion.
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• It is used to prepare solutions of required concentrations necessary for certain biological reactions.
• Indicators: Indicators are the organic compounds. They have different colours in acidic and alkaline solutions. Litmus is a common indicator. It is red in acidic solutions and blue in alkaline solutions. Each indicator has a specific colour in acidic medium which changes at a specific pH to another colour in basic medium. For example, phenolphthalein is colourless in strongly acidic solution and red in strongly alkaline solution. It changes colour at a pH of about 9. This means phenolphthalein is colourless in a solution with pH less than 9. If the pH is above 9, phenolphthalein is red.
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• Measuring pH of a Solution: Universal Indicator: Some indicators are used as mixtures. The mixture indicator gives different colours at different pH values. Hence, it is used to measure the pH of a solution. Such a mixed indicator is called Universal Indicator or simply pH indicator.
• What is the difference between Arrhenius base and Bronsted-Lowry base?
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• What do you mean by neutralization reaction according to Arrhenius acid-base concept?
• Prove that water is an amphoteric specie.
• How can you justify that NH3 is Bronsted-Lowry base but not Arrhenius base?
• State and explain the neutralization reaction according to Lewis concept.
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• Define and give the characteristics of a Lewis acid.
• Why BF3 behaves as a Lewis acid? 
• Which types of salts produce SO2 gas on reacting with acids?
• Give the uses of sulphuric acid.
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• Name the gas liberated when alkalies react with ammonium salts.
• Write down the colours of the precipitates formed by reaction of aqueous caustic soda with solutions of: copper, zinc and ferric salts.
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• Name an alkali used in alkaline batteries.