Can you imagine the taste of food without salt? Food without salt is tasteless, and it becomes difficult for us to eat. Just like this, we encounter Acids, Bases, and salts in our daily life, like the stain of turmeric on a white cloth. If soap is spilled on that stain, then the color of the yellow stain is converted into reddish-brown. Acids, Bases, and Salts are essential in nature as well as in industry. These acids, bases and salts ncert solutions explain the chemical nature of Acids, Bases, and Salts, and how they react with elements like metals and non-metals and with each other. It also explains some astonishing phenomena like a change of color of litmus papers, from red to blue when bases are present, and blue to red when acids are present, and no change in color if the substance is neutral.
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These solutions offer a systematic and structured approach for the exercise questions to prepare well for your exams by providing comprehensive and detailed solutions. NCERT Solutions for Class 10 also serve as a valuable resource for students to enhance their performance in board exams and establish a strong foundation for various competitive exams like JEE and NEET.
Students can download the class 10 science chapter 2 acids, bases and salts question answer in pdf format for free. These solutions of NCERT are designed to help you understand the fundamental concepts and solve textbook questions with ease.
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These class 10 science chapter 2 acids, bases and salts solutions provide clear and stepwise answers to all the questions asked within the chapter. These NCERT Solutions for Class 10 Science help students understand key concepts thoroughly and build a strong foundation for solving related problems in exams.
Answer:
Litmus is a common indicator that is used to identify acid and base. The colour of litmus paper turns to blue indicates that the chemical is a base. If there is no change in colour, then the chemical is either acidic or neutral.
First marks the three test tubes as A, B, and C.
Now,
(i) First of all, put the red litmus paper in each test tube one by one. The test tube in which red litmus paper will turn blue indicates the solution of that test tube is basic/Alkaline in nature.
(ii) Now remaining two are either acidic or neutral. Now mix a drop of the basic solution with a drop of each of the remaining two solutions separately and then the nature of the drops of the mixtures is checked. If the colour of the red litmus turns blue, then the second solution is neutral and if there is no change in colour, then the second solution is acidic. This is because acidic and basic solutions neutralize each other.
Question.1 Why should curd and sour substances not be kept in brass and copper vessels?
Answer:
Curd and sour substances not be kept in brass and copper vessels because curd and other sour substances contain acids.
Therefore, when they are kept in brass and copper vessels, the metal reacts with the acid to liberate hydrogen gas and harmful products, thereby may spoil the food.
Answer:
Hydrogen gas is usually liberated when an acid reacts with a metal.
When zinc granules react with dilute sulphuric acid, then the bubbles of the soap solution are formed. These soap bubbles contain hydrogen gas and a zinc sulphate solution is formed.
$\mathrm{Zn}+2 \mathrm{H}_2 \mathrm{SO}_4 \Rightarrow \mathrm{Zn}\left(\mathrm{SO}_4\right)_2+2 \mathrm{H}_2$
The evolved hydrogen gas can be tested by taking a burning candle near a soap solution containing hydrogen gas. If the candle burns with a pop sound, it confirms the evolution of hydrogen gas.
Answer:
During the chemical reaction, the evolved gas extinguishes a burning candle which means the gas is carbon dioxide.
Since, one of the compounds formed during this reaction is calcium chloride and carbon dioxide is formed when dilute hydrochloric acid reacts with a metal carbonate (or metal hydrogen carbonate) producing effervescence it means the metal compound is calcium carbonate (It cannot be calcium hydrogen carbonate because calcium hydrogen carbonate is found only in solution, it is also unstable to exist as a solid). Hence, the compound A is calcium carbonate.
The chemical reaction is written as follows:
$\mathrm{CaCO}_3+2 \mathrm{HCl}_{(a q)} \rightarrow \mathrm{CaCl}_{2(a q)}+\mathrm{CO}_{2(g)}+\mathrm{H}_2 \mathrm{O}_{(l)}$
Answer:
Acids form hydrogen ions [ $H^{+}(\mathrm{aq})$ ions] in its aqueous solution which is responsible for their acidic characters. HCl and $\mathrm{HNO}_3$ form hydrogen ions in aqueous solution hence, they show acidic characters in aqueous solution.
The reaction of HCL is as follows:
$
\begin{aligned}
& \mathrm{HCl}_{(a q)} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-} \\
& \mathrm{H}^{+}+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{H}_3 \mathrm{O}^{+}
\end{aligned}
$
While solutions of compounds like alcohol and glucose do not form hydrogen ions in the solution, hence, they do not show acidic character.
Question.2 Why does an aqueous solution of acid conduct electricity?
Answer:
Acids dissociate in aqueous solutions to form ions. Like hydrogen ions ( $H^{+}$) or hydronium ions ( $\mathrm{H}_3 \mathrm{O}^{+}$) and the presence of these ions in an aqueous solution of acid are responsible for conducting electricity.
Question.3 Why does dry HCl gas not change the colour of the dry litmus paper?
Answer:
The colour of litmus paper changes only in the presence of ions like hydrogen ( $\mathrm{H}^{+}$) or hydronium ( $\mathrm{H}_3 \mathrm{O}^{+}$) ions. Dry HCl does not contain ( $\mathrm{H}^{+}$) or ( $\mathrm{H}_3 \mathrm{O}^{+}$) ions. It can produce these ions only in the form of an aqueous solution.
Hence, because of that dry HCl gas does not change the colour of dry litmus paper.
Answer:
The process of dissolving an acid in water is highly exothermic in which a large amount of heat is evolved. It is always recommended that acid should slowly be added to water because evolved heat is easily absorbed by a large amount of water.
If it is done the other way, then it is possible that because of the large amount of heat generated, the mixture splashes out and causes burns.
Question.5 How is the concentration of hydronium ions (H3O+) affected when a solution of an acid is diluted?
Answer:
When the solution of an acid is diluted, the concentration of hydronium ions $\left(\mathrm{H}_3 \mathrm{O}^{+}\right)$per unit volume decreases.
That means, the strength of the acid decreases.
Answer:
The concentration of hydroxide ions $\left(\mathrm{OH}^{-}\right)$ would increase when excess base is dissolved in a solution of sodium hydroxide .
Answer:
The pH value of less than 7 indicates an acidic solution while greater than 7 indicates a basic solution. The pH value of a neutral solution is 7. And the acidic solution has more hydrogen ion concentration.
Therefore, solution A with pH = 6 is acidic and has more hydrogen ion concentration than solution B with pH = 8 which is basic.
Question.2 What effect does the concentration of H + (aq) ions have on the nature of the solution?
Answer:
Concentration of $H^{+}(\mathrm{aq})$ can have a varied effect on the nature of the solution. When we increase the concentration of $H^{+}$ions in the solution, the solution becomes more acidic, while when we decrease the concentration of $H^{+}$ions in the solution, the basicity of the solution increases.
Question.3 Do basic solutions also have H + (aq) ions? If yes, then why are these basic?
Answer:
Yes, the basic solution also has $\mathrm{H}+(\mathrm{aq})$ ions. However, they are basic because the concentration of hydrogen ions in them is less as compared to the concentration of hydroxide ions $\left[\mathrm{OH}^{-}\right.$ions $]$that makes the solution basic.
Answer:
Quicklime, slaked lime and chalk are basic in nature. When they react with acids, the neutralization reaction takes place.
Therefore, If the soil is acidic and improper for cultivation, then to increase the basicity of soil, the farmer would treat the soil with quicklime or slaked lime or chalk.
Question.1 What is the common name of the compound $\mathrm{CaOCl}_2$ ?
Answer:
The common name of the compound $\mathrm{CaOCl}_2$ is bleaching powder.
Question.2 Name the substance which on treatment with chlorine yields bleaching powder .
Answer:
Calcium hydroxide $\left[\mathrm{Ca}(\mathrm{OH})_2\right]$ on treatment with chlorine yields bleaching powder.
Question.3 Name the sodium compound which is used for softening hard water.
Answer:
Washing soda $\left(\mathrm{Na}_2 \mathrm{CO}_3 \cdot 10 \mathrm{H}_2 0\right)$ is used for softening hard water.
Answer:
When a solution of sodium hydrogen carbonate (sodium hydrogen carbonate) is heated, it undergoes decomposition reaction to form sodium carbonate and water, and carbon dioxide gas is liberated.
The equation of the reaction involved is:
$2 \mathrm{NaHCO}_3 \xrightarrow{\text { heat }} \mathrm{Na}_2 \mathrm{CO}_3+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2$
Question.5 Write an equation to show the reaction between the Plaster of Paris and water .
Answer:
The chemical equation for the reaction of Plaster of Paris and water can be represented as $\mathrm{CaSO}_4 \cdot \frac{1}{2} \mathrm{H}_2 \mathrm{O}+1 \frac{1}{2} \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{CaSO}_4 \cdot 2 \mathrm{H}_2 \mathrm{O}$
These acids, bases and salts class 10 question answer offer detailed and accurate explanations for all the end-of-chapter questions. These NCERT solutions assist students in revising important concepts, practising application-based questions, and enhancing their overall problem-solving skills.
Question.1 A solution turns red litmus blue, its pH is likely to be
(a) 1
(b) 4
(c) 5
(d) 10
Answer:
(d) As we have lean bases turn red litmus blue. The basic solution has a pH value of more than 7. Since the solution turns red litmus blue, therefore its pH is likely to be > 7 i.e. 10.
(a) NaCl
(b) HCl
(c) LiCl
(d) KCl
Answer:
(b) The solution contains HCI reacts with crushed egg-shells to give a gas that turns lime-water milky.
(a) 4 mL
(b) 8 mL
(c) 12 mL
(d) 16 mL
Answer:
It is given that
10 ml of NaOH neutralizes 8 ml Solution of HCl $\therefore 1 \mathrm{ml}$ of NaOH neutralizes $=\frac{8}{10}$
$=\frac{4}{5} \mathrm{ml}$ Solution of HCl
Therefore, 20 ml of NaOH will neutralise $=\frac{4}{5} \times 20=16 \mathrm{ml}$ solution of HCL
Therefore, 16 ml of HCl solution will be required to neutralize the 20 ml of NaOH.
The correct answer is (d)
Question.4 Which one of the following types of medicines are used for treating indigestion?
(a) Antibiotic
(b) Analgesic
(c) Antacid
(d) Antiseptic
Answer:
(c) The antacid is used for treating indigestion.
Question.5 Write word equations and then balanced equations for the reaction taking place when –
(a) dilute sulphuric acid reacts with zinc granules.
(b) dilute hydrochloric acid reacts with magnesium ribbon.
(c) dilute sulphuric acid reacts with aluminum powder.
(d) dilute hydrochloric acid reacts with iron filings.
Answer:
Balanced equations are:-
(a) $\mathrm{H}_2 \mathrm{SO}_{4(a q)}+\mathrm{Zn}_{(s)} \rightarrow \mathrm{ZnSO}_{4(a q)}+\mathrm{H}_{2(g)}$
(b) $2 \mathrm{HCl}_{(a q)}+\mathrm{Mg}_{(s)} \rightarrow \mathrm{MgCl}_{2(a q)}+\mathrm{H}_{2(g)}$
(c) $3 \mathrm{H}_2 \mathrm{SO}_{4(a q)}+2 \mathrm{Al}_{(s)} \rightarrow \mathrm{Al}_2\left(\mathrm{SO}_4\right)_{3(a q)}+3 \mathrm{H}_{2(g)}$
(d) $6 \mathrm{HCl}_{(a q)}+2 \mathrm{Fe}_{(s)} \rightarrow 2 \mathrm{FeCl}_{3(a q)}+3 \mathrm{H}_{2(g)}$
Answer:
Take the solution of dilute hydrochloric solution and glucose. Two nails are fitted on a cork and are kept it in a 100 mL beaker. The nails are then connected to the two terminals of a 6-volt battery through a bulb and a switch. Dilute HCl is poured in the beaker and current is switched on. Now, the same experiment is performed with a glucose solution and an alcohol solution.
We will observe that the bulb glows in the HCl solution and does not glow in the glucose solution.
Because: HCl dissociate into H+ (aq) and Cl-(aq) ions. These ions conduct electricity in the solution resulting in the glowing of the bulb. On the other hand, the glucose solution does not dissociate into ions. Therefore, it does not conduct electricity.
Conclusion:
From this activity, it can be concluded that all acids contain hydrogen but not all compounds containing hydrogen are acids. That is why, though compounds like alcohols and glucose contain hydrogen, they are not categorized as acids.
Question.7 Why does distilled water not conduct electricity, whereas rainwater does?
Answer:
Distilled water is a pure form of water that does not contain ions. Therefore, it does not conduct electricity. Rainwater on the other hand, being an impure form of water, contains many ionic compounds such as acids and therefore it conducts electricity.
Question.8 Why do acids not show acidic behaviour in the absence of water?
Answer:
Acids do not show acidic behaviour in the absence of water because acids form hydrogen ions [H + (aq) ions] in its aqueous solution which are responsible for their acidic characters and the dissociation of hydrogen ions from an acid occurs in the presence of water only.
Therefore in the absence of water, acids do not produce hydrogen ions and hence do not show acidic behaviour.
Question.9 (a) Five solutions A, B, C, D, and E, when tested with universal indicator, showed pH as 4,1,11,7 and 9, respectively. Which solution is
Answer:
Solution with pH equal to 7 is a neutral solution. Therefore, a neutral solution is D
Question.9 (b) Five solutions A, B, C, D, and E, when tested with universal indicator, showed pH as 4,1,11,7 and 9, respectively. Which solution is
Answer:
The solution with the highest pH is strongly alkaline. Therefore, a strongly alkaline solution is C with a pH equal to 11
Question.9 (c) Five solutions A, B, C, D, and E, when tested with universal indicator, showed pH as 4,1,11,7 and 9, respectively. Which solution is
Answer:
The solution with the lowest pH value is strongly acidic. Therefore, a strongly acidic solution is B with pH equal to 1
Question.9 (d) Five solutions A, B, C, D, and E, when tested with universal indicator, showed pH as 4,1,11,7 and 9, respectively. Which solution is
Answer:
A solution with a pH less than 7 but close to 7 is weakly acidic. Therefore, the weakly acidic solution is A with a pH equal to 4
Question.9 (e) Five solutions A, B, C, D, and E, when tested with universal indicator, showed pH as 4,1,11,7 and 9, respectively. Which solution is
e) Weakly alkaline?
Answer:
The solution with a pH greater than 7 but close to 7 is weakly alkaline. Therefore, a weakly alkaline solution is E with pH equal to 9
Answer:
When an acid reacts with magnesium metal, hydrogen gas is produced which causes fizzing. Stronger acids having a greater number of hydrogen ions in it. Hence, fizzing will occur strongly in test tube A, in which hydrochloric acid (HCI) is added.
This is because HCI is a stronger acid as compared to $\left(\mathrm{CH}_3 \mathrm{COOH}\right)$ and therefore, during the chemical reaction with magnesium metal, HCl will produce more hydrogen gas due to which fizzing will be more vigorous in test-tube A.
Question.11 Fresh milk has a pH of 6. How do you think the pH will change as it turns into curd? Explain your answer.
Answer:
The pH of fresh milk is 6.
As milk turns into curd, lactic acid is formed due to which it becomes more acidic. Therefore, the pH of milk will decrease.
Question.12 (a) A milkman adds a very small amount of baking soda to fresh milk.
(a) Why does he shift the pH of the fresh milk from 6 to slightly alkaline?
Answer:
Fresh milk is slightly acidic in nature, The milkman shifts the pH of the fresh milk from 6 to slightly alkaline by adding little baking soda.
Because this will prevent the milk from getting sour due to lactic acid formation.
Question.12 (b) A milkman adds a very small amount of baking soda to fresh milk.
(b) Why does this milk take a long time to set as curd?
Answer:
Since this milk is slightly basic than usual milk, the lactic acid, formed during curdling, needs to first neutralize the alkali present in the milk.
Therefore, it takes a longer time for the curd to set.
Question 13 The plaster of Paris should be stored in a moisture-proof container. Explain why?
Answer:
Plaster of Paris should be stored in a moisture-proof container because it absorbs moisture (or water) to form a hard substance called gypsum which makes Plaster of Paris useless.
$\mathrm{CaSO}_4 \cdot \frac{1}{2} \mathrm{H}_2 \mathrm{O}+1 \frac{1}{2} \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{CaSO}_4 \cdot 2 \mathrm{H}_2 \mathrm{O}$
Question 14 What is a neutralization reaction? Give two examples.
Answer:
A reaction in which an acid and base react with each other to give a salt and water is known as neutralization reaction. That is: Acid + Base → Salt + Water
For example:
(i) Sodium hydroxide (NaOH) reacts with hydrochloric acid (HCl) to form sodium chloride (NaCl) and water:
$
\mathrm{NaOH}+\mathrm{HCl} \rightarrow \mathrm{NaCl}+\mathrm{H}_2 \mathrm{O}
$
(ii) Magnesium hydroxide reacts with hydrochloric acid to form magnesium chloride and water:
$
\mathrm{Mg}(\mathrm{OH})_2+2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2+2 \mathrm{H}_2 \mathrm{O}
$
Question 15 Give two important uses of washing soda and baking soda.
Answer:
Uses of Washing Soda:
(i) It is used for removing the permanent hardness of the water.
(ii) It is used in glass, soap, and paper industries.
Uses of Baking Soda:
(i) It is used in soda-acid fire extinguishers.
(ii) It is used in making baking powder. Baking powder is a mixture of baking soda and a mild edible acid called tartaric acid. When baking powder is heated
Or mixed in water, it releases CO2 that makes cakes or bread fluffy.
Some important practice questions related to the class 10 science chapter 2 acids, bases and salts solutions are given below. These questions have a high probability of being asked in future board exams.
Question 1. What are acids and bases? Give two examples of each?
Answer:
Acids: These substances release $\mathrm{H}^{+}$ ions in aqueous solutions.
Examples: HCl, $\mathrm{H}_2 \mathrm{SO}_4$.
Bases: These substances release $\mathrm{OH}^{-}$ ions in aqueous solutions.
Examples: NaOH, $\mathrm{Ca}(\mathrm{OH})_2$.
Question 2. Why is it important to maintain the pH of soil?
Answer:
Plants need a specific pH range to grow. If the soil is too acidic or basic, nutrients become unavailable, and plant growth is affected. So, maintaining the pH ensures proper nutrient absorption and fruther growth of the plant.
Question 3. What is the pH range of acidic, Basic, and neutral solution?
Answer:
The pH range of acidic, Basic, and neutral solution:
Acidic solution: pH less than 7.
Basic solution: pH greater than 7.
Neutral solution: pH equal to 7.
Question 4: A white shirt has a yellow stain of curry. When soap is rubbed on this shirt during washing, the yellow stain turns reddish-brown. On rinsing the shirt with plenty of water, the reddish-brown stain turns yellow again. Name the natural indicator present in curry stain
(1) Baking soda
(2) Common salt
(3) Citric acid
(4) Turmeric
Answer:
The yellow stain contains turmeric and as turmeric is natural indicator it turns into red colour when soap is rubbed because soap is basic. When the shirt is rinsed off the soap also gets rinsed off and hence again the colour turns to yellow.
Hence, the answer is the option (4).
Question 5: Acids not show acidic behavior in the absence of water because
(1) Dissociation of hydrogen ions occurs in water only
(2) They release OH- ions in absence water
(3) Acids release heat after addition to water
(4) None of the above
Answer:
Acids do not show acidic behaviour in the absence of water because the dissociation of hydrogen ions from an acid occurs in the presence of water only. It is the hydrogen ions that are responsible for the acidic behaviour.
Hence, the answer is the option (1).
Question 6: A student adds dilute HCl to a compound and observes brisk effervescence. The gas evolved turns lime water milky. Which of the following compounds was most likely used?
(1) NaCl
(2) $\mathrm{Na}_2 \mathrm{CO}_3$
(3) $\mathrm{MgCl}_2$
(4) $\mathrm{CuSO}_4$
Carbonates react with acids to form $\mathrm{CO}_2$ gas, which turns lime water milky due to the formation of CaCO
$\mathrm{Na}_2 \mathrm{CO}_3+2 \mathrm{HCl} \rightarrow 2 \mathrm{NaCl}+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2$
Hence, the correct answer is option (2).
Question 7: Acidic foods can be identified by which taste?
(1) Salty
(2) Sour
(3) bitter
(4) Sweet
Answer:
Acid is sour in taste, hence acidic foods are also sour in taste.
Hence, the answer is the option (2).
Question 8: Which of the following are the correct products from the reaction between magnesium hydroxide and sulfuric acid?
(1) Magnesium sulfate + water
(2) Magnesium sulfate + hydrogen chloride
(3) Magnesium sulfate + hydrogen
(4) none of the above
Answer:
Only Salt and water are the two products formed when an acid reacts with an alkali.
Hence, the answer is the option (1).
To solve acids, bases and salts class 10 question answer it is important to follow a systematic approach. It is recommended to strategies your study plan to solve the questions of this chapter. The following are the points that will help you build a good approach. The following are some points that can help you build a good strategy.
1. First, start by memorizing and understanding the basic terms like Acids, bases and salts, Strong vs. weak acids/bases, Indicators, pH and its scale. Also learn what color changes each indicator shows with acids and bases. Students can also follow Class 10 Science Chapter 2 Acids, Bases And Salts notes to understand all these concepts better.
2. Make a quick table of important reactions such as:
3. The concept is easy yet important as it can help you solve many numerical type questions. Know how to use the pH scale (0 to 14)
Lower pH = more acidic; Higher pH = more basic
4. Study how common salt leads to the formation of baking soda, washing soda and bleaching powder
5. Read statements carefully and think logically. Also, interpret experiments like litmus paper in acid/base, pH of various solutions. Students must refer class 10 science chapter 2 acids, bases and salts solutions also solve exemplar problems and previous year board questions regularly.
Topics and subtopics covered in the NCERT Solutions for Class 10 Science Chapter 2 Acids, Bases and Salts are given below. A basic understanding of these topics helps students to solve complex problems easily.
2.1 Understanding the Chemical Properties of Acids and Bases
2.1.1 Acids and Bases in the Laboratory
2.1.2 How do Acids and Bases React with Metals?
2.1.3 How do Metal Carbonates and Metal Hydrogencarbonates React with Acids?
2.1.4 How do Acids and Bases React with each other?
2.1.5 Reaction of Metallic Oxides with Acids
2.1.6 Reaction of a Non-metallic Oxide with Base
2.2 What do All Acids and All Bases Have in Common
2.2.1 What Happens to an Acid or a Base in a Water Solution?
2.3 How Strong are Acid or Base Solutions?
2.3.1 Importance of pH in Everyday Life
2.4 More About Salts
2.4.1 Family of Salts
2.4.2 pH of Salts
2.4.3 Chemicals from Common Salt
2.4.4 Are the Crystals of Salts really Dry?
Important reactions from the NCERT Solutions for Class 10 Science Chapter 2 Acids, Bases and Salts are given below:
Important Reactions:
Acid + Metal $\rightarrow$ Salt + Hydrogen gas
Example: $2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Na}_2 \mathrm{ZnO}_2(\mathrm{~s})+\mathrm{H}_2(\mathrm{~g})$ (Sodium zincate)
Metal carbonate/Metal hydrogencarbonate + Acid $\rightarrow$ Salt $\boldsymbol{+}$ Carbon dioxide $\boldsymbol{+}$ Water
$\mathrm{NaOH}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Na}_2 \mathrm{ZnO}_2(\mathrm{~s})+\mathrm{H}_2(\mathrm{~g})($ Sodium zincate $)$
Base + Acid $\rightarrow$ Salt + Water
$\mathrm{NaOH}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\mathrm{l})$
Metal oxide + Acid $\rightarrow$ Salt + Water
When electricity is passed through an aqueous solution of sodium chloride (called brine), it decomposes to form sodium hydroxide. The process is called the chlor-alkali process because of the products formed– chlor for chlorine and alkali for sodium hydroxide.
$2 \mathrm{NaCl}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow 2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{Cl}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g})$
Bleaching Powder ($\mathrm{CaOCl}_2$) Formation:
$\mathrm{Ca}(\mathrm{OH})_2+\mathrm{Cl}_2 \rightarrow \mathrm{CaOCl}_2+\mathrm{H}_2 \mathrm{O}$
Baking Soda ($\mathrm{NaHCO}_3$3) Formation:
$\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2+\mathrm{NH}_3 \longrightarrow-\mathrm{NH} \mathrm{H}_4 \mathrm{Cl}$ (Ammonium chloride) $+\mathrm{NaHCO}_3$ (Sodium hydrogen carbonate)
Washing Soda ($\mathrm{Na}_2 \mathrm{CO}_3 \cdot 10 \mathrm{H}_2 \mathrm{C}$) Formation:
$\mathrm{Na}_2 \mathrm{CO}_3$ (sodium carbonate) $+10 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{Na}_2 \mathrm{CO}_3 \cdot 10 \mathrm{H}_2 \mathrm{O}$
Plaster of Paris:
$
\mathrm{CaSO}_4 \cdot \frac{1}{2} \mathrm{H}_2 \mathrm{O}
$
Preparation:
$
\underset{\text { Gypsum }}{\mathrm{CaSO}_4 \cdot 2 \mathrm{H}_2 \mathrm{O}} \xrightarrow{\text { Heat }} \underset{\text { Plaster of Paris }}{\mathrm{CaSO}_4} \cdot \frac{1}{2} \mathrm{H}_2 \mathrm{O}+1 \frac{1}{2} \mathrm{H}_2 \mathrm{O}
$
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These acids, bases and salts ncert solutions help students easily understand concepts. They explain important concepts and reactions in a simple way. These solutions also help students practice questions and prepare well for exams.
These solutions help students to understand the chemical properties and reactions of acids, bases, and salts.
Using these solutions they learn how to identify acids and bases using indicators and pH scale.
Preparation, uses, and importance of common salts in daily life can be explained easily with the help of class 10 science chapter 2 acids, bases and salts question answer.
Balancing of chemical equations involving acids, bases, and salts are discussed very well using these solutions.
The class 10 science acids, bases and salts question answer helps students understand the chemistry behind common substances used in daily life. Given below some points on why these solutions are important:
Besides NCERT Solutions for Class 10 Science Chapter 2 Acids, Bases and Salts, chapter-wise solutions for class 10 are given below:
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Frequently Asked Questions (FAQs)
NCERT Solutions for this chapter are a set of step by step answers to all in-text and exercise questions. They help students understand the concepts of acids, bases, and salts, learn their reactions and properties, and prepare effectively for exams.
Class 10 Science Chapter 2 Acids, Bases and Salts includes both in-text questions and exercise questions with answers. These cover definitions, properties, reactions, neutralisation, pH values, preparation, and uses of salts, and balancing chemical equations.
A solution is a base if it has a bitter taste, turns red litmus paper blue, and contains hydroxide ions. Bases usually feel slippery to touch, and their pH is greater than 7. Examples include sodium hydroxide and ammonia.
Indicators are substances that change the color depending on the pH of the solution. They are generally used to determine whether a solution is acidic, basic, or neutral. Common examples of indicators litmus paper, phenolphthalein, and methyl orange.
Acids and bases neutralize each other because an acid releases hydrogen ions and a base releases hydroxide ions in water. When they react, H⁺ and OH⁻ combine to form water, removing the acidic and basic properties. This reaction is called neutralisation, and it often produces a salt as well.
Acids and bases play a crucial role in everyday activities. For instance, acids are found in foods like citrus fruits, while bases can be found in cleaning agents. They are involved in processes like digestion, and their reactions are fundamental in various chemical processes in industries and laboratories.
A neutralization reaction occurs when an acid reacts with a base to produce salt and water. This process is crucial in many applications, such as treating acid burns with baking soda or the interaction between hydrochloric acid and sodium hydroxide, which forms sodium chloride and water.
Salts are formed from the neutralization of acids and bases and are vital in many biological processes. They regulate fluid balance, are essential for nerve function, and are key in agriculture for soil fertility.
pH measures how acidic or basic a solution is, on a scale from 0 to 14. It plays a crucial role in various aspects of daily life, such as in food, agriculture, and health.
Several factors influence the strength of acids and bases, including molecular structure, the degree of ionization in water, and the concentration of the solution. Strong acids and bases ionize completely, while weak acids and bases only partially ionize, resulting in lower concentrations of H⁺ or OH⁻ ions in solution.
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Check for
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https://school.careers360.com/boards/cbse/cbse-previous-year-question-papers-class-10
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If you have filled the wrong bubble on the ORM sheet in the CBSE Class 10 board but the roll number is correct, it is considered a minor error.
If your roll number is correct, your sheet may still be evaluated and you can check your marks using
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A block of mass 0.50 kg is moving with a speed of 2.00 ms-1 on a smooth surface. It strikes another mass of 1.00 kg and then they move together as a single body. The energy loss during the collision is
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An athlete in the olympic games covers a distance of 100 m in 10 s. His kinetic energy can be estimated to be in the range
| Option 1)
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Option 2)
|
| Option 3)
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Option 4)
|
A particle is projected at 600 to the horizontal with a kinetic energy . The kinetic energy at the highest point
| Option 1)
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Option 2)
|
| Option 3)
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Option 4)
|
In the reaction,
| Option 1)
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Option 2)
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| Option 3)
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Option 4)
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How many moles of magnesium phosphate, will contain 0.25 mole of oxygen atoms?
| Option 1)
0.02 |
Option 2)
3.125 × 10-2 |
| Option 3)
1.25 × 10-2 |
Option 4)
2.5 × 10-2 |
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