FA 5 is a mixture containing two cations and two anions. Three of the ions are listed in the Qualitative analysis notes. (i) Carry out the following tests and record your observations in Table 3.1. (ii) Carry out the following tests using a 1 cm depth of FA 6 in a test-tube for each test. Record your observations in Table 3.2. (iii) FA 5 reacts with nitric acid to make FA 6 in Test 2 in Table 3.1. State a change you would see in one of the observations in Table 3.2 if hydrochloric acid had been used to prepare FA 6. ....................................................................................................................................... . ................................................................................................................................. (iv) Use your observations in (a)(i) and (a)(ii) to identify the formulae of three of the ions present in FA 5. Formulae of ions present are ..................... and ..................... and ..................... .

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_s24_qp_33 Year：2024 Question No：(a)

Answer:

Knowledge points:

7.1.1.1 understand what is meant by a reversible reaction

7.1.1.2 understand what is meant by dynamic equilibrium in terms of the rate of forward and reverse reactions being equal and the concentration of reactants and products remaining constant

7.1.1.3 understand the need for a closed system in order to establish dynamic equilibrium

7.1.10 describe and explain the conditions used in the Haber process and the Contact process, as examples of the importance of an understanding of dynamic equilibrium in the chemical industry and the application of Le Chatelier’s principle

7.1.2 define Le Chatelier’s principle as: if a change is made to a system at dynamic equilibrium, the position of equilibrium moves to minimise this change

7.1.3 use Le Chatelier’s principle to deduce qualitatively (from appropriate information) the effects of changes in temperature, concentration, pressure or presence of a catalyst on a system at equilibrium

7.1.4 deduce expressions for equilibrium constants in terms of concentrations,

7.1.5 use the terms mole fraction and partial pressure

7.1.6 deduce expressions for equilibrium constants in terms of partial pressures,

7.1.7 use the expressions to carry out calculations (such calculations will not require the solving of quadratic equations)

7.1.8 calculate the quantities present at equilibrium, given appropriate data

7.1.9 state whether changes in temperature, concentration or pressure or the presence of a catalyst affect the value of the equilibrium constant for a reaction

Answer:

Knowledge points:

Solution:

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