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Unformatted text preview: &+¡¢£ :RUNVKHHW ¤ £¢ TXHVWLRQV LQYROYLQJ VLPSOH ZDWHU HTXLOEULD DQG WKH DSSUR[LPDWLRQV WKDW PDNH WKHP VLPSOH¥ 1. The only water equilibrium for which we make no approximations is the case of pure water (amazing how simple something is when you don’t add anything to it.) What is the most common approximation made when we add acids or bases to water? 2. For each of the compounds and concentrations shown below, tell what kind of compound it is (strong acid, weak acid, strong base, weak base, salt) and write down the equation you would use to solve the problem. compound type equation 0.2 M HClO 4 0.1 M NH 4 Cl HgI 2 0.03 M Ba(OH) 2 0.2 M CH 3 NH 2 0.2 M lithium acetate 0.1 M lactic acid AgI 3-11. For the next eight problems, find either the pH or the molar solubility of the compound for the compounds in Table 2. Assume a simple equilibrium in each case. You will note that the total time and uncertainty involved in solving these eight problems will probably be less than the time and doubt involved in completing table 2. This should be a heads up to you that the biggest reason people struggle in this section of material is that they don’t know what kind of problem they are working—and we haven’t even started dumping multiple compounds into solution!! 3. What is the pH of 0.2 M HClO 4 ? 4. What is the pH of 0.1 M NH 4 Cl? The pK b of NH 3 is 4.75. 5. What is the molar solubility of HgI 2 ? The K sp of HgI 2 is 3 x 10-29 . 6. What is the pH of 0.03 M Ba(OH) 2 ? (Hint, there are 2 OH- dumped into solution for each Ba(OH) 2 .) 7. What is the pH of...
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ws6302 - & ¡¢£:RUNVKHHW ¤ £¢ TXHVWLRQV LQYROYLQJ...

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