Quiz+3s+120 by wanghonghx

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									Quiz 3A                                     Name________________________
10 points                                   Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14                pH + pOH = 14.00         KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                        pOH = -log[OH-]


1. Indicate if the following salts will be acidic, basic, or neutral in water.


         KCHO2                 Ca(CN)2                         NH4ClO3


2. Write the reaction, if any, that occurs when these ions are placed in water.

a) CN-


b) Br-


3. What is the pH of a 0.33M solution of nitrous acid, HNO2? Ka for HNO2 is 4.6 x 10-4.
Quiz 3B                                 Name________________________
10 points                               Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14             pH + pOH = 14.00      KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                     pOH = -log[OH-]


1. Give the products of these reactions below.

             Reactants                                  Products


       HCN      +        H2 O          


       C3H7NH3+     + H2 O              




2. What is the pH of a 0.25M solution of KClO? (Ka for HClO = 2.9 x 10-8)
Quiz 3C                                    Name________________________
10 points                                  Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14               pH + pOH = 14.00         KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                       pOH = -log[OH-]


1. Are the following salts acidic, basic, or neutral?


       C6H5NH3I                       KCHO2                          NaF




2. Write the reaction, if any, that occurs when these species are placed in water.

a) CH3CH2NH2


b) Ca2+



3. What is the pH of 0.30M H2CO3? Ka1 =          Ka2 =
Quiz 3D                                 Name________________________
10 points                               Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14             pH + pOH = 14.00       KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                     pOH = -log[OH-]


1. What is the pH of a solution that is 0.45M HF (Ka = 6.8 x 10-4) and 0.25M HI? What is the
% ionization of the HF in this solution?




2.   What is the pH of 0.85M sodium propionate, NaC3H5O2? Ka for HC3H5O2 = 1.3 x 10-5
Quiz 3E                                   Name________________________
10 points                                 Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14             pH + pOH = 14.00    KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                     pOH = -log[OH-]


1. Give the products of these reactions below.

             Reactants                                 Products


       CN-     +         H2O          


       C3H7NH2     + H2O               


2. What is the pH of 0.3M C6H5NH3I? Kb of C6H5NH2 = 3.9 x 10-10
Quiz 3F                                     Name________________________
10 points                                   Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14                pH + pOH = 14.00          KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                        pOH = -log[OH-]


1. Indicate if the following salts will be acidic, basic, or neutral in water.


         KCHO2                 CaCN                    NH4ClO3


2. Write the reaction, if any, that occurs when these ions are placed in water.

a) CN-


b) Br-


3. What is the pH of a 0.33M solution of nitrous acid, HNO2? Ka for HNO2 is 4.6 x 10-4.
Quiz 3G                                 Name________________________
10 points                               Maleckar / Chem 120 / Spring 2012
[H3O+][OH-] = 1 x 10-14             pH + pOH = 14.00       KaKb = Kw = 1 x 10-14
pH = -log[H3O+]                     pOH = -log[OH-]


1. What is the pH of a solution that is 0.45M HF (Ka = 6.8 x 10-4) and 0.25M HI? What is the
% ionization of the HF in this solution?




2.   What is the pH of 0.85M sodium propionate, NaC3H5O2? Ka for HC3H5O2 = 1.3 x 10-5

								
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