If the hydroxide ion concentration of an aqueous solution is 3.0 x 10-4, what is the [H+] in the solution? Is the solution acidic, basic, or neutral?

[H+] is  3.31 × 10^-11 M

Solution: Basic

Explanation:

In the question we are given;

Concentration of Hydroxide ion [OH-] as 3.0 × 10^-4 M

We are required to determine the [H+] and whether the solution is acidic, basic or neutral.

We know that;

pOH + pH = 14

and that;

pOH = - log [OH-]

Therefore;

pOH = - log ( 3.0 × 10^-4)

       = 3.52

But;

pH = 14 - pOH

Thus;

pH = 14 - 3.52

     = 10.48

But, we know that;

pH = - log[H+]

Therefore;

H+ = Antilog -pH

    = Antilog -10.48

    = 3.31 × 10^-11

Thus, the concentration of H+ ions [H+] is  3.31 × 10^-11 M

Also since the pH is 10.48, then the solution is basic

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.

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