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(a)
Interpretation:
The difference between a strong electrolyte and a strong acid needs to be explained.
Concept introduction:
A strong acid is a compound or solute completely dissociates or ionizes in solution to give proton. The concentration of proton increases instantly by addition of acid in solution.
Strong electrolyte involves the compounds such as NaCl, KCl which dissociates completely to give the corresponding ions present in it.
Due to the 100 % dissociation, they are known as good conductor of electricity. Strong acids, strong bases and ionic compounds are good example of strong electrolyte.
(b)
Interpretation:
The difference between oxidizing agent and reducing agent needs to be explained.
Concept introduction:
A
A reactant that loses electron/s gets positive charge on it and undergoes oxidation. While reactant that accepts electron/s gets negative charge on it and undergo reduction.
The reactant or species getting reduced in the reaction by accepting the electron helps in the oxidation of other reactant and thus act as oxidizing agent.
The reactant or species getting oxidized in the reaction by releasing the electron helps in the reduction of the other reactant and thus act as reducing agent.
(c)
Interpretation:
The difference between precipitation reaction and neutralization reaction needs to be explained.
Concept introduction:
Neutralization reactions generally involve the
Precipitation reaction generally involves the precipitation of the reactants present in the reaction. Formation of precipitates takes place on the reaction between the electrolytes in the reaction.
(d)
Interpretation:
The difference between half reaction and overall reaction needs to be explained.
Concept introduction:
A redox reaction is the reaction consists of reactant in which one reactant gets oxidized and other gets reduced.
A reactant that loses electron/s gets positive charge on it and undergoes oxidation. While reactant that accepts electron/s gets negative charge on it, undergo reduction.
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Chapter 5 Solutions
EBK GENERAL CHEMISTRY
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- distinguish between ions, electrolytes, and free radicals;andarrow_forwardXO4- (aq) + Z3+ (aq)=X2+ (aq) + ZO22+ (aq) Where: X = Metal #1 and Z = Metal #2 (a) the initial oxidation numbers of each atom on both sides of the equation. (b) separate oxidation and reduction 1/2-reactions. (c) the balancing of electrons, atoms, and charge in both 1/2-reactions. (d) combining of balanced half-reactions, cancelling species if necessary, to form a balanced redox reaction in acidic solution. (e) modification of the balanced reaction in acidic solution to a balanced reaction in basic solution.arrow_forward1) Give oxidation numbers for the underlined element in each of the folle molecules or ions. (a) C4H§O4: (b) Fe3O4: (c) VO2*: (d)SnBr4: (e) PH4: (f) Ce2(SO4)3:arrow_forward
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