A chemist prepares a solution of silver(II) oxide by measuring out 0.0013 of silver(II) oxide into a 100 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in of the chemist's silver(II) oxide solution. Be sure your answer has the correct number of significant digits.

1.3x10⁻⁸ mol/L

Explanation:

0.0013μmol, Calculate concentration in mol/L

To obtain concentration in mol/L we need to convert the μmoles to moles and mL to liters:

Moles silver(II) oxide:

0.0013μmol × (1mol / 1x10⁶μmol) = 1.3x10⁻⁹ moles

Liters solution:

100mL * (1L / 1000mL) = 0.1L

That means concentration in mol/L is:

1.3x10⁻⁹ moles / 0.1L =

the answer is 1 i believe

it is stable as it is in group 0 which have full outer shells of electrons