Question

Calculate: concentration is measured by molarity (m), or moles per liter. brackets are also used to symbolize molarity. for example, if 0.6 moles of hno3 are dissolved in a liter of water, you would say [hno3] = 0.6 m. because hno3 is a strong acid, it dissociates almost completely in water. that means the concentration of h+ is very nearly equal to that of hno3. what is [h+] if [hno3] is 0.01 m? _it is also 0.01________ the ph of a solution is equal to the negative log of h+ concentration: ph = –log[h+] what is the ph of this solution? (use the "log" button on your calculator.) _________ what is the ph of a 0.6 m hno3 solution? _________

Answer 1

 As HNO₃ completely dissociates to H⁺ ions, concentration of H⁺ ions is equal to concentration of HNO₃.
As  [HNO₃] is 0.01 m , [H⁺] = 0.01 m

ph can be calculated using the following equation,
pH = - log [H⁺]
For the solution of 0.01 m, pH is 
pH = - log 0.01
pH = 2
when  [HNO₃] is 0.01 m , pH = 2

when  [HNO₃] is 0.6 m, [H⁺] = 0.6 m
Therefore,
pH = -log 0.6
pH of solution is 0.22

Answer 2

The pH of $\rm \bold { [HNO_3]}$  at 0.01 M conentration is 2 while at 0.6 M the pH will be 0.22.

The $\rm \bold { HNO_3}$ is strong acid hence it completely dissociate in the water.

Hence,

$\rm \bold { [HNO_3]}$  = 0.01 M,  $\rm \bold { [H^+]}$ will also be 0.01 M

From pH formula,

$\rm \bold {pH = - log [H^+]}$

pH = 2

when $\rm \bold { [HNO_3]}$  is 0.6 M,  $\rm \bold { [H^+]}$ will be 0.6 M

pH = -log 0.6

pH of solution is 0.22

Hence, we can conclude that the pH of $\rm \bold { [HNO_3]}$  at 0.01 M conentration is 2 while at 0.6 M the pH will be 0.22.

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