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Solution is a homogeneous mixture of two or more compounds. We experience different types of solutions in our daily lives like sugar dissolved in water, salt dissolved in water, and air which is a homogeneous mixture of gases. Every mixture is not a solution for example, oil dissolved in water is a mixture but not a solution because it is not a homogeneous mixture. So, for a mixture to be a solution one thing is necessary which is mixture must be homogeneous. A homogeneous mixture is one where the composition of the mixture is uniform throughout.
In this chapter, students are going to study different types of solutions, their properties, and how their concentration is expressed. This chapter helps students understand why some substances dissolve and others remain undissolved, and why sugar dissolves easily in hot water as compared to cold water. NCERT solutions designed by subject experts provide easy-to-understand and comprehensive explanations of every question NCERT solutions for class 12 helps students to develop analytical and problem-solving abilities. Solutions for every question are given below and students can scroll down to get detailed answers of the given questions.
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NCERT Exemplar Class 12 Chemistry solutions Chapter 1 |
NCERT notes Class 12 Chemistry Chapter 1 Solution |
Answer:
We know that solute and solvent forms solution.
So mass percentage of benzene (solute) :-
=
Similarly mass percentage of CCl4 :-
Question 1.2 Calculate the mole fraction of benzene in solution containing
Answer :
For calculating mole fraction, we need moles of both the compounds.
It is given that benzene is
So if we consider 100g of solution then 30g is benzene and 70g is CCl4 .
Moles of CCl
Similarly moles of benzene :
(Molar mass of benzene
So mole fraction of benzene is given :
Question 1.3(a) Calculate the molarity of each of the following solutions:
Answer :
For finding molarity we need the moles of solute and volume of solution.
So moles of solute :
Since molar mass of
Now,
Question 1.3(b) Calculate the molarity of each of the following solutions:
Answer :
By conservation of moles we can write :
M1V1 = M2V2
Given that M1= 0.5 M and V1 = 30 ml ; V2 = 500 ml
Question 1.4 Calculate the mass of urea
Answer :
Let us assume that the mass of urea required be x g.
So moles of urea will be :
Molality
we get x = 37
Thus mass of urea required = 37 g.
Question 1.5 Calculate
(a) molality
(b) molarity and
(c) mole fraction
of KI if the density of
Answer :
If we assume our solution is 100 g. Then according to question, 20 g KI is present and 80 g is water.
So moles of KI :
(a) Molality :-
Molality
(b) Molarity :-
Volume
Molarity
(c) Mol fraction = Moles of water :-
So, mol fraction of KI :-
Page- 9
Answer :
For finding Henry's constant we need to know about the mole fraction of H2S.
Solubility of H2S in water is given to be 0.195 m .
i.e., 0.195 moles in 1 Kg of water.
So
At STP conditions, pressure = 1 atm or 0.987 bar
Equation is :
So we get :
Question 1.7 Henry’s law constant for
Answer :
We know that ,
Pressure of CO2= 2.5 atm
We know that :
So, Pressure of CO2 =
By Henry Law we get,
Taking density of soda water = 1 g/ml
We get mass of water = 500 g.
So, Moles of water :
Also,
So, moles of CO2= 0.042 mol
Using relation of mole and given mass, we get
Mass of CO2 = 1.848 g.
Page-15
Answer :
Let the composition of liquid A (mole fraction) be x A .
So mole fraction of B will be x B = 1 - x A .
Given that,
Using Raoult’s law ,
Putting values of p total and vapour pressure of pure liquids in the above equation, we get :
600 = 450.x A + 700.(1 - x A )
or 600 - 700 = 450x A - 700x A
or x A = 0.4
and x B = 0.6
Now pressure in vapour phase :
= 450(0.4) = 180 mm of Hg
= 700(0.6) = 420 mm of Hg
And mole fraction of liquid B = 0.70
Page - 23
Question 1.9 Vapour pressure of pure water at
Answer :
Given that vapour pressure of pure water,
Moles of water :
Moles of urea :
Let the vapour pressure of water be Pw.
By Raoult's law, we get :
or
or p w = 23.4 mm of Hg.
Relative lowering :- Hence, the vapour pressure(v.P) of water in the solution = 23.4 mm of Hg
and its relative lowering = 0.0173.
Question 1.10 Boiling point of water at
Answer :
Here we will use the formula :
Elevation in temperature = 100 - 99.63 = 0.37
K b = 0.52 ;
Putting all values in above formula, we get :
Thus 121.67 g of sucrose needs to be added.
Question 1.11 Calculate the mass of ascorbic acid (Vitamin C,
Answer :
Elevation in melting point = 1.5 degree celsius.
Here we will use the following equation :
Putting given values in the above equation :
Thus 5.08 ascorbic acid is needed for required condition.
Question 1.12 Calculate the osmotic pressure in pascals exerted by a solution prepared by dissolving
Answer :
We know that :
We are given with :-
Volume, V = 0.45 L
Thus osmotic pressure :
Question.1.1 Define the term solution. How many types of solutions are formed? Write briefly about each type with an example.
Answer :
A solution is a homogeneous mixture of two or more non-reacting substances. It has two components :- solute and solvent.
Types of solutions are given below :-
Question 1.2 Give an example of a solid solution in which the solute is a gas.
Answer:
Solution of hydrogen in palladium is such an example in which the solute is a gas and the solvent is a solid.
Question 1.3(i) Define the following terms:
Mole fraction
Answer :
Mole fraction is defined as the ratio of a number of moles of a component to and total number of moles in all components.
i.e.,
Question 1.3(ii) Define the following terms:
Molality
Answer :
It is defined as the number of moles of solute dissolved per kg (1000g) of solvent
i.e.,
It is independent of temperature.
Question 1.3(iii) Define the following terms:
Molarity
Answer :
Molarity is defined as a number of moles of solute dissolved per litre(or 1000 mL) of solution.
i.e.,
It depends on temperature because volume is dependent on temperature.
Question 1.3(iv) Define the following terms:
Mass percentage.
Answer :
Mass percentage is defined as the percentage ratio of mass of one component to the total mass of all the components.
i.e.,
Answer :
According to given question, in 100 g of solution 68 g is nitric acid and rest is water.
So moles of 68 g HNO3:-
= 1.08
Density of solution is given to be 1.504.
So volume of 100 g solution becomes :-
= 66.49\ mL
Thus, molarity of nitric acid is :
Molarity
= 16.24 M
Answer :
According to question,
Molar mass of glucose (C6H12O6) =
So moles of glucose are :
Mole fraction :-
Molarity :- Volume of 100 g solution :
Question 1.6 How many mL of
Answer :
Total amount of mixture of Na2CO3 and NaHCO3= 1 g.
Let the amount of Na2CO3 be x g.
So the amount of NaHCO3 will be equal to (1 - x) g.
Now it is given that it is an equimolar mixture.
So, Moles of Na2CO3= Moles of NaHCO3
or
or x = 0.558 g
So
and
It is clear that for 1 mol of Na2CO3 2 mol of HCl is required, similarly for 1 mol of NaHCO3 1 mol of HCl is required.
So number of moles required of HCl = 2(0.00526) + 0.0053 = 0.01578 mol
It is given that molarity of HCl is 0.1 which means 0.1 mol of HCl in 1 L of solution.
Thus required volume :
Answer :
According to question we have 2 solute,
Solute 1. :
Solute 2. :
So total amount of solute = 75 + 160 = 235 g.
Thus mass percentage of solute is :
and mass percentage of water
Answer :
For finding molality we need to find the moles of ethylene glycol.
Moles of ethylene glycol :
We know that :
Now for molarity :-
Total mass of solution = 200 + 222.6 = 422.6 g
Volume of solution
So molarity :-
express this in percent by mass
Answer :
We know that 15 ppm means 15 parts per million.
Required percent by mass :
Question 1.9(ii) A sample of drinking water was found to be severely contaminated with chloroform
determine the molality of chloroform in the water sample.
Answer :
Moles of chloroform :
Mass of water is
So molality will be :
Question 1.10 What role does the molecular interaction play in a solution of alcohol and water?
Answer :
Both alcohol and water individually have strong hydrogen bonds as their force of attraction. When we mix alcohol with water they form solution due to the formation of hydrogen bonds but they are weaker as compared to hydrogen bonds of pure water or pure alcohol.
Thus this solution shows a positive deviation from the ideal behaviour.
Question 1.11 Why do gases always tend to be less soluble in liquids as the temperature is raised?
Answer:
It is known that dissolution of gas in a liquid is an exothermic process. So, by Le Chatelier principle we know that equilibrium shifts backwards as we increase temperature in case of exothermic process. Thus gases always tend to be less soluble in liquids as the temperature is raised.
Question 1.12 State Henry’s law and mention some important applications.
Answer :
According to Henry's law at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the solution or liquid.
i.e., p = kh.x, Here kh is Henry’s law constant.
Some of its applications are as follows:-
(a) We can increase the solubility of CO2 in soft drinks, the bottle is sealed under high pressure.
(b) To avoid bends (due to blockage of capillaries) and the toxic effects of high concentrations of nitrogen in the blood, the tanks used by scuba divers are filled with air diluted with helium (11.7% helium, 56.2% nitrogen and 32.1% oxygen).
(c) The partial pressure of oxygen is less at high altitudes than at ground level. This leads to low concentrations of oxygen in the blood and tissues, climbers. Due to low blood oxygen, climbers become weak and unable to think clearly, which are symptoms of a condition known as anoxia.
Answer :
Using Henry's Law we can write,
Putting value in this equation, we get :
So, the magnitude of k is
Now, we will again use the above equation for
So the required partial pressure is :-
or
Answer :
Positive and negative deviation: - A non-ideal solution is defined as a solution which does not obey Raoult’s law over the entire range of concentration i.e.,
Enthalpy relation to positive and negative deviation can be understood from the following example:-
Consider a solution made up of two components - A and B. In the pure state the intermolecular force of attraction between them are A-A and B-B. But when we mix the two, we get a binary solution with molecular interaction A-B.
If A-B interaction is weak than A-A and B-B then enthalpy of reaction will be positive thus reaction will tend to move in a backward direction. Hence molecules in binary solution will have a higher tendency to escape. Thus vapour pressure increases and shows positive deviation from the ideal behaviour.
Similarly, for negative deviation, A-B interaction is stronger than that of A-A and B-B.
Answer :
It is given that
Also the vapour of water at normal boiling point = 1.013 bar.
Using Raoult's law :
So we get :
Thus, the molar mass of non-volatile solute is 41.35 units.
Answer :
Vapour pressure of heptane =
and vapour pressure of octane =
Firstly, we will find moles of heptane and octane so that we can find the vapour pressure of each.
Molar mass of heptane = 7(12) + 16(1) = 100 unit.
and molar mass of octane = 8(12) + 18(1) = 114 unit.
So moles of heptane :
and moles of octane :
Mole fraction of heptane = 0.456 and mole fraction of octane = 0.544
Now we will find the partial vapour pressure:-
(i) of heptane :-
(ii) of octane :-
So total pressure of solution =
= 47.97 + 25.46 = 73.43 KPa
Question 1.17 The vapour pressure of water is
Answer :
It is asked the vapour pressure of a 1 molal solution, which means 1 mol of solute in 1000 g H 2 O.
Moles in 1000g of water = 55.55 mol. (Since the molecular weight of H 2 O is 18)
Mole fraction of solute :
Applying the equation :
or
or
Thus the vapour pressure of the solution is 12.083 KPa
Question 1.18 Calculate the mass of a non-volatile solute
Answer :
Let the initial vapour pressure of octane =
After adding solute to octane, the vapour pressure becomes :
Moles of octane :
Using Raoult's law we get :
or
or
Thus required mass of non-volatile solute = 10g.
the molar mass of the solute
Answer :
In this question, we will find the molar mass of the solute by using Raoult's law.
Let the molar mass of the solute be M.
Initially, we had 30 g of solute and 90 g of water.
Moles of water :
By Raoult's law we have:-
or
or
Now we have added 18 g of water more, so the equation becomes:
Moles of H2O :
Putting this in above equation we obtain:-
or
From equation (i) and (ii) we get
M = 23 u
So the molar mass of solute is 23 units.
vapour pressure of water at 298 K.
Answer :
In the previous part we have calculated the value of molar mass the Raoul's law equation.
We had :-
Putting M = 23 u in the above equation we get,
or
Thus vapour pressure of water = 3.53 kPa.
Answer :
It is given that the freezing point of pure water is 273.15 K.
So, elevation of freezing point = 273.15 - 271 = 2.15 K
Moles of cane sugar :
Molality :
We also know that -
or
Now we will use the above procedure for glucose.
Moles of glucose :
Thus molality :
So, we can find the elevation in freezing point:
Thus freezing point of glucose solution is 273.15 - 4.09 = 269.06 K.
Answer :
In this question we will use the formula :
Firstly for compound AB 2 :-
or
Similarly for compound AB 4 :-
If we assume atomic weight of element A to be x and of element B to be y, then we have :-
x + 2y = 110.87 ----------------- (i)
x + 4y = 196 ----------------- (ii)
Solving both the equations, we get :-
x = 25.59 ; y = 42.6
Hence atomic mass of element A is 25.59u and atomic mass of element B is 42.6u.
Answer :
According to given conditions we have same solution under same temperature. So we can write :
So, if we put all the given values in above equation, we get
or
Hence the required concentration is 0.061 M.
Question 1.23(i) Suggest the most important type of intermolecular attractive interaction in the following pairs.
n-hexane and n-octane
Answer :
Since both the compounds are alkanes so their mixture has van der Waal force of attraction between compounds.
Question 1.23(ii) Suggest the most important type of intermolecular attractive interaction in the following pairs.
Answer :
The binary mixture of these compounds has van der Waal force of attraction between them.
Question 1.23(iii) Suggest the most important type of intermolecular attractive interaction in the following pairs.
Answer :
The given compounds will have ion-dipole interaction between them.
Question 1.23(iv) Suggest the most important type of intermolecular attractive interaction in the following pairs.
Answer :
Methanol has -OH group and acetone has ketone group. So there will be hydrogen bonding between them.
Question 1.23(v) Suggest the most important type of intermolecular attractive interaction in the following pairs.
acetonitrile
Answer :
They will have dipole-dipole interaction since both are polar compounds.
Question 1.24 Based on solute-solvent interactions, arrange the following in order of increasing solubility in n-octane and explain.
Cyclohexane, KCl, CH3OH, CH3CN.
Answer :
The order will be : Cyclohexane > CH3CN > CH3OH > KCl
In this, we have used the fact that like dissolves like.
Since cyclohexane is an alkane so its solubility will be maximum.
Question 1.25(i) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
phenol
Answer :
We know the fact that like dissolves in like.
Since phenol is had both polar and non-polar group so it is partially soluble in water.
Question 1.25(ii) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
toluene
Answer :
Since toluene is a non-polar compound i.e., it doesn't have any polar group so it is insoluble in water. (because water is a polar compound)
Question 1.25(iii) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
formic acid
Answer :
Since the -OH group in formic acid (polar) can form H-bonds with water thus it is highly soluble in water.
Question 1.25(iv) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
ethylene glycol
Answer :
Ethylene glycol is an organic compound but is polar in nature. Also, it can form H-bonds with water molecules, thus it is highly soluble in water.
Question 1.25(v) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
chloroform
Answer :
Chloroform is a non-polar compound so it is insoluble in water.
Question 1.25(vi) Amongst the following compounds, identify which are insoluble, partially soluble and highly soluble in water?
pentanol
Answer :
Pentanol has both polar and non-polar groups so it is partially soluble in water.
Question .1.26 If the density of some lake water is
Answer :
We know that, Molality :
So, for moles of solute we have :
Thus, molality :
Molality of Na + ions is 4m.
Question 1.27 If the solubility product of
Answer :
We are given,
The dissociation equation of CuS is given by :-
So, the equation becomes :-
or
or
Thus maximum molarity of solution is
Question 1.28 Calculate the mass percentage of aspirin
Answer :
Total mass of solution = Mass of aspirin + Mass of acetonitrile = 6.5 + 450 = 456.5 g.
We know that :
So,
Thus the mass percentage of aspirin is
Answer :
We are given with molality of the solution, so we need to find the moles of Nalorphene.
Molar mass of nalorphene = 19(12) + 21(1) + 1(14) + 3(16) = 311u.
So moles of nalorphene :
Molality :
or
or
So the required weight of water is 3.2 g.
Question 1.30 Calculate the amount of benzoic acid
Answer :
Molar mass of benzoic acid = 7(12) + 6(1) + 2(16) = 122u.
We are given with the molarity of a solution.
or
or
So mass of benzoic acid :
Hence the required amount of benzoic acid is 4.575 g.
Answer :
We know that depression in the freezing point of water will depend upon the degree of ionisation.
The degree of ionisation will be highest in the case of trifluoroacetic acid as it is most acidic among all three.
The order of degree of ionisation on the basis if acidic nature will be:- Trifluoroacetic acid > Trichloroacetic acid > Acetic acid.
So the depression in freezing point will be reverse of the above order.
Question 1.32 Calculate the depression in the freezing point of water when
Answer :
Firstly we will find the Vant's Hoff factor the dissociation of given compound.
So we can write,
or
or
Putting values of K a and C in the last result, we get :
At equilibrium i = 1 - a + a + a = 1 + a = 1.0655
Now we need to find the moles of the given compound CH3 CH2CHClCOOH.
So, moles =
Thus, molality of the solution :
Now we will use :
or
Answer :
Firstly we need to calculate molality in order to get vant's hoff factor.
So moles of CH2FCOOH :
We need to assume volume of solution to be nearly equal to 500 mL. (as 500 g water is present)
Now, we know that :
or
Now for dissociation constant :-
and,
Put values of C and a in the above equation, we get :
Question 1.34 Vapour pressure of water at
Answer :
Firstly we will find number of moles of both water and glucose.
Moles of glucose :
and moles of water :
Now,
or
or
Thus vapour pressure of water after glucose addition = 17.44 mm of Hg
Question 1.35 Henry’s law constant for the molality of methane in benzene at
Answer :
We know that :
We are given value of P and k, so C can be found.
Hence solubility of methane in benzene is
Answer :
For calculating partial vapour pressure we need to calculate mole fractions of components.
So number of moles of liquid A :
and moles of liquid B :
Mole fraction of A (x A ) :
and mole fraction of B (x B ) :
Now, P total = P A + P B
or
or
or
Thus vapour pressure in solution due to A =
Plot this data also on the same graph paper. Indicate whether it has positive deviation or negative deviation from the ideal solution.
Answer :
it has negative deviation from the ideal solution.
Answer :
Firstly, we will find the no. of moles of the given compounds.
No. of moles of benzene :
and the no. of moles of toluene :
Now we will find mol fraction of both:-
Mole fraction of benzene :-
and mole fraction of toluene :
Now,
P total = Pb + Pt
or
or
Hence mole fraction of benzene in vapour phase is given by :
Answer :
We have been given that the water is in equilibrium with air at a pressure of 10 atm or 7600 mm of Hg.
So the partial pressure of oxygen :
and partial pressure of nitrogen :
Now, by Henry's Law :
For oxygen :
For nitrogen :
Hence the mole fraction of nitrogen and oxygen in water is
Question 1.40 Determine the amount of
Answer :
We know that osmotic pressure :
or
We have been given the values of osmotic pressure, V, i and T.
So the value of w can be found.
Hence 3.42 g CaCl2 is required.
Answer :
Dissociation of K 2 SO 4 is as follows :-
Molecular weight of K 2 SO 4 = 2(39) + 1(32) + 4(16) = 174u.
Putting all the values :-
Question:
The freezing point depression of a 0.1 m aqueous solution of a monobasic weak acid HA is
Given :
(1).
(2).
(3).
(4).
Answer:
Hence, the correct answer is option (1).
Question: Which of the following binary mixture does not show the behaviour of minimum boiling azeotropes ?
(1)
(2)
(3)
(4)
Answer:
The solution showing positive deviation from Raoult's law will form a minimum boiling azeotrope. Phenol + Aniline shows negative deviation, so they will not form a minimum boiling azeotrope.
A binary mixture of
Hence, the correct answer is option (2).
Sometimes, problems related to Solutions seem difficult, but once we understand the basic formulas, it becomes very easy to solve all the questions related to Solutions.
We can follow the steps given below to solve the questions based on the Solutions:
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These steps can be followed while solving problems related to Solutions.
1.2 Expression Of Concentration Of Solution
1.3 Solubility
1.4 Vapour Pressure Of Liquid Solutions
1.5 Ideal and Non-ideal Solutions
1.6 Colligative Properties and Determination of Molar Mass
1.7 Abnormal Molar Masses
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Chapter 1, Solutions, primarily deals with the concept of solutions in chemistry. It explains the types of solutions, their properties, and the methods for expressing concentration, such as molarity, molality, and mass percentage. This chapter lays the foundational understanding of how solutes and solvents interact in a solution.
This chapter classifies solutions based on the states of matter of solute and solvent. The main types include:
Molarity is calculated using the formula:
Molarity (M) = moles of solute/liters of solution.
To find the moles of solute, you divide the mass of the solute in grams by its molar mass. Then, measure the volume of the solution in liters to determine the molarity.
Molarity (M) refers to the number of moles of solute per liter of solution, whereas molality (m) is the number of moles of solute per kilogram of solvent. The key difference lies in the denominator; molarity uses total volume of the solution, while molality considers only the mass of the solvent, making molality independent of temperature.
Concentration of a solution indicates how much solute is present in a given amount of solvent or solution. It can be expressed in various ways, such as molarity, molality, mass percentage, or parts per million (ppm). Understanding concentration is essential for preparing and using solutions in experiments.
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