Nielsen Bhaskar/PC/1713K/A 2/05 1CHM1041 Answer to Exercise set # 7 Ionic Equilibria I 1. By choosing the proper temperatures, both (normally a solid) and (normally a gas) are liquids. But liquid is a good conductor of electricity and liquid is not. Why is this? On the other hand, a water solution of either substance at room temperature is a good conductor. Explain why. NaC1HC1NaC1HC1NaC1is an ionic solid at room temperature and incapable of conducting electricity as a solid. Mobile ions are required for the conduction of electric current, and the ions of solid are locked in the crystal lattice. As a liquid at higher temperatures (molten state), the ions become mobile and the conduction of current is possible. Hydrogen chloride, is a polar covalent molecule and cannot conduct electric current as a solid, pure liquid, or gas. In water solution, however, both and produce 100% ions and both conduct current. NaC1HC1,NaC1HC1100% ()()()2H Os+1-1aqNaC1Na+C1aq⎯⎯⎯→()()()23+1-12gaH OHC1+ H OH OC1⎯⎯⎯→+qaq100% 2. Calculate the concentration of each of the ions in the following solutions of strong electrolytes: (a) 0.0090 M HBr()()2H O+11agHBrHBrag−⎯⎯⎯→+100% 0.0090 M 0.0090 M (b) 240.0102 M Li SO100% ( )()()22H O4s+1-24agagLi SOSO2 Li+⎯⎯⎯→0.0090 M0.0102 M(c) ()()246320.0033 MA1 H OSO⎡⎤⎣⎦()()( )()()2H O2+3-22463 s6 ag2AH OSO2 AH O+ 3 SO⎡⎤⎯⎯⎯→⎣⎦AA40.0066 M 0.0099 M
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