Acids bases and salts class 10 mcq online test

Acids bases and salts is the 2st chapter of class 10th science syllabus and it is little bit harder as well as lengthy chapter as compared to other chapters of chemistry class 10th science syllabus. Acids have a sour taste and change the colour of blue litmus to red, while bases have a bitter taste and change the colour of red litmus to blue. In this segment, we’ll learn about acid and base reactions, how acids and bases balance out each other’s effects, and various other topics that we encounter in our daily lives. You can learn about the chemical properties of acids and bases, how acids and bases react with metals, how metal carbonates and metal hydrogen carbonates react with acids, how acids and bases react with each other, how metallic oxides react with acids, and how a non-metallic oxide reacts with a base, all of which are illustrated with appropriate illustrations and chemical reactions. 

CLASS 10 SCIENCE CHAPTER 2 – CHEMICAL REACTIONS AND EQUATIONS DETAILED ANALYSIS

Queries	Answer
DIFFICULTY LEVEL	Moderate to hard
EASIEST TOPIC	Concept of pH scale
HARDEST TOPIC	Preparation and uses of Sodium Hydroxide, Bleaching powder, Baking soda, Washing soda and Plaster of Paris
WEIGHTAGE	5 marks as per latest sample paper NOTE- it may vary between 5-8
TYPE OF QUESTIONS ASKED	2 questions of 1 marks 1 question of 3 marks Notes – This date is as per latest sample paper of 2023
NUMBER OF QUESTIONS IN EXAM	Approx 3-5 questions every year
IMPORTANCE OF CHAPTER	Will help in understanding Acids bases and salts
HANDWRITTEN NOTES OF THIS CHAPTER	Class 10 science handwritten notes pdf download
IMPORTANT TOPIC FOR EXAM	Basic definition, Preparation and uses of compounds given

IMPORTANT DEFINATIONS OF CHAPTER 2
Acids: Substances which turn blue litmus solution red are called acids. Acids are sour in taste
Bases: Substances which change red litmus solution blue are called bases. They are bitter in taste.
Mineral Acids: Acids which are obtained from minerals like sulphates, nitrates, chlorides etc. are called mineral acids, e.g., H2SO4( Sulphuric acid), HNO3(Nitric acid) and HCl(Hydrochloric acid).
Organic Acids: Acids which are obtained from plants and animals are called organic acids. e.g. citric acid, ascorbic acid, tartaric acid, lactic acid, acetic acid.
Hydronium Ions(H3O+): They are formed by reaction of H+ (from acid) and H2O. It is because H+ is unstable.
Strong Acids: Acids which dissociate into ions completely are called strong acids. E.g. H2SO4, HCl
Weak Acids: Acids which do not dissociate into ions completely are called weak acids E.g. Citric acid, acetic acid.
pH scale: A scale for measuring hydrogen ion concentration in a solution. The pH of a solution is defined as the negative logarithm of hydrogen ion concentration in moles per liter.  pH =-log [H+] pH =-log [H3O+] where [H+] or [H3O+] represents concentrations of hydrogen ions in solution. The pH of a neutral solution is 7  The pH of an acidic solution is < 7  The pH of a basic solution is> 7
Indicators – Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. Universal Indicator: A universal indicator is a mixture of indicators which shows a gradual but well-marked series of colour changes over a very wide range of change in concentration of H+ ion.
Chemical properties of acids Acids react with active metals to give salt and hydrogen gas. Acids react with metal carbonate and metals hydrogen carbonate to give salt, water and carbon dioxide. Acids react with bases to give salt and water. This reaction is called neutralization reaction. iv)Acids react with metals oxides to give salt and water.
Chemical properties of Bases Reaction with Metals – Certain metals such as Zinc, Aluminum and Tin react with alkali solutions on heating and hydrogen gas is evolved. Reaction with acids – Bases react with acids to form salt and water

EQUATIONS OF ACIDS,BASES AND SALTS
Acid + Metal à Salt + Hydrogen gas  H2SO4+Zn àZnSO4+H2
Base+ Metal àSalt + Hydrogen gas  2NaOH + Zn à Na2ZnO2 + H2
Base + Acid ——> Salt + Water NaOH (aq) +HCl (aq) àNaCl (aq) + H2O (l)
Acids give hydronium ions in water  HCl+H2Oà H3O++ Cl–
Bases generate OH– ions in water  NaOH(s)+H2O —->Na+(aq)+OH–(aq)
On heating, baking soda liberates CO2 2NaHCO3 + Heat ——-> Na2CO3 + H2O + CO2
On mixing plaster of Paris with water, gypsum is obtained   CaSO4.1/2H2O +1 ½ H2O à CaSO4 .2H2O

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