Describe the trend in the solubility of the hydroxides of magnesium, calcium and strontium. ....................................................................................................................................... . ....................................................................................................................................... . ....................................................................................................................................... . ....................................................................................................................................... . ....................................................................................................................................... . ....................................................................................................................................... . (ii) Suggest the variation in pH of saturated solutions of the hydroxides of magnesium, calcium and strontium. Explain your answer. ....................................................................................................................................... . ....................................................................................................................................... . .................................................................................................................................

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_s24_qp_43 Year：2024 Question No：1(a)

Answer:

Knowledge points:

25.1.1 understand and use the terms conjugate acid and conjugate base

25.1.10.1 understand and use the common ion effect to explain the different solubility of a compound in a solution containing a common ion

25.1.10.2 perform calculations using values and concentration of a common ion

25.1.2 define conjugate acid–base pairs, identifying such pairs in reactions

25.1.3 define mathematically the terms pH, use them in calculations and the equation will not be tested)

25.1.4.1 strong acids

25.1.4.2 strong alkalis

25.1.4.3 weak acids

25.1.5.1 define a buffer solution

25.1.5.2 explain how a buffer solution can be made

25.1.5.3 explain how buffer solutions control pH; use chemical equations in these explanations

25.1.5.4 describe and explain the uses of buffer solutions, including the role of in controlling pH in blood

25.1.6 calculate the pH of buffer solutions, given appropriate data

25.1.7 understand and use the term solubility product

25.1.8 write an expression for

25.1.9 calculate from concentrations and vice versa

3.6.1.1 describe hydrogen bonding, limited to molecules containing N–H and O–H groups, including ammonia and water as simple examples

3.6.1.2.1 its relatively high melting and boiling points

3.6.1.2.2 its relatively high surface tension

3.6.1.2.3 the density of the solid ice compared with the liquid water

3.6.2 use the concept of electronegativity to explain bond polarity and dipole moments of molecules

3.6.3.1 describe van der Waals’ forces as the intermolecular forces between molecular entities other than those due to bond formation, and use the term van der Waals’ forces as a generic term to describe all intermolecular forces

3.6.3.2.1 instantaneous dipole – induced dipole (id-id) force, also called London dispersion forces

3.6.3.2.2 permanent dipole – permanent dipole (pd-pd) force, including hydrogen bonding

3.6.3.2.3 tdescribe hydrogen bonding and understand that hydrogen bonding is a special case of permanent dipole – permanent dipole force between molecules where hydrogen is bonded to a highly electronegative atom

3.6.4 stae that, in general, ionic, covalent and metallic bonding are stronger than intermolecular forces

Answer:

Knowledge points:

Solution:

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