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Class 12 Chemistry · Chemistry Part I · Chapter 1
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Chemistry
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Physics, Chemistry, Maths + English
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Physics, Chemistry, Biology + English
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Accountancy, Business Studies, Economics + English
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Chemistry
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Chemistry
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Physics
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History
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Hindi Elective
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Mathematics
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Sociology
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Economics
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Home Science
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Urdu Elective
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Geography
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Accountancy
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English Core
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Political Science
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Business Studies
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Hindi Core
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Mathematics
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हिंदी (आधार)
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Accountancy
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اردو (اختیاری)
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Mathematics
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हिंदी (आधार)
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संस्कृतम् (केन्द्रिकम्)
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Physics
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हिंदी (ऐच्छिक)
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संस्कृत (ऐच्छिक)
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Physics
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हिंदी (ऐच्छिक)
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اردو (کور)
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Urdu Elective
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Computer Science
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Fine Art · Painting
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हिंदुस्तानी संगीत (गायन / वादन)
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Biology
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Informatics Practices
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Accountancy
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Biotechnology
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Accountancy
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सृजनात्मक लेखन और अनुवाद
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Business Studies
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हिंदुस्तानी संगीत (तबला / पखावज)
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Business Studies
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Economics
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Economics
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History
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History
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History
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Geography
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Geography
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Geography
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English Elective · Kaleidoscope
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Political Science
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Political Science
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Sociology
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Sociology
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Psychology
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English Core · Flamingo
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English Core · Vistas
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Home Science
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Home Science
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Summary
A solution is a homogeneous mixture of two or more components whose composition and properties are uniform throughout; the component in largest amount is the solvent. Concentration can be expressed as mass percentage, volume percentage, parts per million, mole fraction, molarity \(M\) (moles of solute per litre of solution) and molality \(m\) (moles per kg of solvent), of which mole fraction and molality are temperature independent. The solubility of a gas in a liquid is governed by Henry's law, \(p=K_H x\), the partial pressure of a gas over a solution being proportional to its mole fraction. For liquid-liquid solutions Raoult's law states that the partial vapour pressure of each volatile component is proportional to its mole fraction, \(p_A=p_A^{\circ}x_A\); ideal solutions obey it over the whole range while real solutions show positive or negative deviations. Properties that depend only on the number of solute particles and not their nature are colligative: relative lowering of vapour pressure, elevation of boiling point \(\Delta T_b=K_b m\), depression of freezing point \(\Delta T_f=K_f m\), and osmotic pressure \(\Pi=CRT\). These properties give molar masses of solutes; abnormal values arise when solutes associate or dissociate, accounted for by the van't Hoff factor \(i\).
Types of solutions and concentration unitsSolubility and Henry's lawVapour pressure and Raoult's lawIdeal and non-ideal solutionsColligative properties and molar massAbnormal molar mass and van't Hoff factor
Key terms
Mole fraction
Ratio of moles of one component to the total moles of all components; dimensionless and temperature independent.
Molality
Number of moles of solute per kilogram of solvent, \(m\); independent of temperature.
Henry's law
Partial pressure of a gas over a solution is proportional to its mole fraction, \(p=K_H x\).
Raoult's law
Partial vapour pressure of a volatile component equals its mole fraction times the pure-component vapour pressure, \(p_A=p_A^{\circ}x_A\).
Colligative property
A property that depends only on the number of solute particles, not their identity.
van't Hoff factor
Factor \(i\) that corrects colligative properties for dissociation or association of the solute.
Extra questions & answers
Try one from this chapter
Which of the following is a colligative property?