Question

In: Chemistry

Calculate the pH, pOH, [H3O+], and [OH-] of the following solutions: (a) 0.001 M HNO3, (b)...

Calculate the pH, pOH, [H3O+], and [OH-] of the following solutions:
(a) 0.001 M HNO3,
(b) 0.3 M Ca(OH)2;
(c) 3.0 M HNO3,
(d) 6.0 M NaOH,
(e) 0.05 M HBr

Solutions

Expert Solution

(a) 0.001 M HNO3

HNO3 is strong acid

                   HNO3 + H2O--------> H3O+   + NO3-

                   0.001M                     0.001M

                  [OH-] = Kw/[H3O+]

                              = 1*10-14/0.001 = 10-11 M

                     PH    = -log[H3O+]

                               = -log0.001 = 3
(b) 0.3 M Ca(OH)2

                         Ca(OH)2 ---------> Ca+2 + 2OH-

                          0.3M                                   2*0.3 = 0.6M

                           [OH-]   = 0.6M

                           [H3O+]   = Kw/[OH-]

                                          = 1*10-14/0.6   = 1.67*10-14 M

                                PH   = -log1.67*10-14   = 13.7772
(c) 3.0 M HNO3

                      HNO3 + H2O---------> H3O+ + NO3-

                        3M                3M

                    [H3O+]   = 3M

                    [OH-]   = Kw/[H3O+]

                                 = 1*10-14/3 = 3.4*10-15 M

                     PH   = -log[H3O+]

                              = -log3   = -0.4471
(d) 6.0 M NaOH,

              NaOH   -------> Na+ + OH-

                6M                            6M

               [OH-]    = 6M

              [H3O+]   = Kw/[OH-]

                             = 1*10-14 /6    = 1.7*10-15 M

                PH   = -log[H3O+]

                         = -log1.7*10-15

                         = 14.7695
(e) 0.05 M HBr

                     HBr ----------> H+ + Br-

                   0.05M             0.05M

                  [H+]   = 0.05M

                    [OH-]   = Kw/[H3O+]

                                 = 1*10-14 /0.05   = 2*10-12 M

                    PH = -log[H3O+]

                           = -log0.05 = 1.3010

queen_honey_blossom answered 1 year ago
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