This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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1: A solution conducts electricity if the bulb glows brightly, dimly, or not at all when electrodes are dipped in it and connected to a battery and bulb. If the bulb glows, the solution conducts electricity. 2a: Aqueous HCl is a strong acid that completely ionizes in water to produce a large number of free H+ and Cl- ions. HCl_(aq) -> H+_(aq) + Cl-_(aq) These mobile ions carry electric current, so the bulb glows brightly. Aqueous HCl conducts due to complete ionization into H+ and Cl- ions. 2b: Solid lead(II) bromide is an ionic compound, but the Pb^2+ and Br- ions are held fixed in the crystal lattice and cannot move. No free mobile ions are present to carry electric current. Solid PbBr2 does not conduct as ions are immobile in the lattice. 2c: Glucose solution contains neutral glucose molecules that do not ionize or dissociate into ions in water. No free ions are present to conduct electricity. Glucose solution does not conduct as it is a non-electrolyte (no ions). 2d: Dilute sulphuric acid is a strong acid (dibasic) that ionizes stepwise to produce H+ and HSO4- (and further SO4^2-) ions. H2SO4_(aq) -> H+_(aq) + HSO4-_(aq) HSO4-_(aq) <=> H+_(aq) + SO4^2-_(aq) Mobile ions carry current, so the bulb glows. Dilute H2SO4 conducts due to ionization into H+, HSO4-, and SO4^2- ions.