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

oh it is true if thats what you are asking

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.