Exset8 - Nielsen CHM1041 Exercise Set 8 Ionic Equilibria II...

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Nielsen Bhaskar/PC/1713J/A 2/05 1 CHM1041 Exercise Set 8 Ionic Equilibria II 1. Explain why water solutions of HCl and HClO 4 are practically equal in acid strength, even though HClO 4 is known to be a much stronger acid in certain other solvents. 2. Write the equations illustrating the dissolution of the following salts in water. Indicate which ions undergo hydrolysis, which do not, and write an equation describing each hydrolysis. State if the resulting solution is acidic, basic, or neutral. (a) Na 2 S (b) Cu(NO 3 ) 2 (c) CsBr (d) KF (e) NH 4 NO 3 (f) CH 3 NH 3 Cl (g) NH 4 S (h) Ca(NO 3 ) 2 (i) Ba(ClO) 2 (j) FeCl 3 3. Which has the greater OH –1 concentration, a 0.50 M solution of sodium acetate, NaO 2 CCH 3 , or a 0.50 M solution of sodium cyanide, NaCN? Calculate the OH –1 concentration for each solution. 4. Calculate the hydrogen ion concentration in 0.10 M NH 4 NO 3 . 5. (a) Based on relative values of K a and K b , explain why a water solution of KHSO 4 is acidic, whereas a water solution of KHCO 3 is basic. (b) Would a water solution of KH 2 PO 4 be acidic or basic? Why? Repeat for a water solution of K 2 HPO 4 . 6. What is the pH of a solution that has an H +1 ion concentration of 1.0 x 10 –5 mole/liter?
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This note was uploaded on 12/12/2011 for the course CHM 2041 taught by Professor Staff during the Fall '09 term at Santa Fe College.

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Exset8 - Nielsen CHM1041 Exercise Set 8 Ionic Equilibria II...

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