Due Date: 3/16/07 Assignment #7 Chemistry 106 Chapter 9: Applying Your Knowledge 4. (a) H + ion donor – acids are H + ion donors because they have the ability to release a H + ion in a water solution (b) H + ion acceptor – bases are H + ion acceptors because are able to accept H + ions from acids (c) Hydronium ion – a hydrated proton H 3 O + (d) Hydroxide ion – OH-ions – bases have higher concentrations of hydroxide ions than of hydronium ions 12. pH is defined as the negative logarithm of the hydronium ion concentration. pH = -log [H 3 O + ] 16. (a) HBr( aq ) + Ca(OH) 2 ( aq ) → CaBr( aq ) + H 2 O( l ) (b) HNO 3 ( aq ) + Al(OH) 3 ( aq ) → AlNO 3 ( aq ) + H 2 O( l ) 18. A solution with a pH of 10 is more basic than a solution with a pH of 2 because solutions increase in acidity as they go from pH 7 to pH 0 and they increase in basicity as they go from pH 7 to pH 14. A solution with a pH of 10 has a higher concentration of hydroxide ions than hydronium ions. 24. If an acid is added, it will react with the basic component of the buffer (in this case,
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This homework help was uploaded on 02/20/2009 for the course CHEM 106 taught by Professor Houston,p during the Spring '08 term at Cornell.