What would be the poh of an hno3 solution if the [h+] = 3.26 x 10-6 moles/liter?

We are given with a compound, Nitric Acid (HNO3) solution,characterized as a strong acid. We are tasked to solve for it's corresponding mass pOH given [H+] = 3.26 x 10-6 moles/liter. Note that

14=pH+pOH

First we need to convert [H+] to pH by

pH=-log[H+]

pH=-log[3.26x10-6]

pH=5.49

Thus,

14=5.49+pOH

pOH=14-5.49=8.51

Therefore, the pOH of Nitric acid solution having a [H+] = 3.26 x 10-6 moles/liter is 8.51

can you attach a picture of the lettuce? : )

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml