What is the ph of a solution containing the strong base ba(oh)2 at a concentration of 0.064 mol/l?

The pH of a solution is a measure used to evaluate the acidity of a solution. It is related to the hydronium ion concentration in the solution. It is expressed as pH = -log [H+]. Also, it is related to pOH by the equation 14 = pH + pOH. It is stated that the substance given in the problem is a strong base which means that it completely dissociates into ions. It dissociates as follows:

Ba(OH)2 = Ba^2+ + 2OH-

To determine the pH of the solution, we need to determine the OH- concentration. Then, find pOH. We do as follows:

[OH-] = 0.0064 mol Ba(OH)2 / L ( 2 mol OH- / 1 mol Ba(OH)2 ) = 0.0128 mol OH- / L

pOH = -log (0.0128) = 1.8928
pH = 14 - 1.8928 = 12.1072

All the given elements belong to the second period of the periodic table

Explanation:

Let's locate the elements with the given atomic numbers:

Z = 3, this corresponds to lithium (Li);Z = 4, this corresponds to beryllium (Be);Z = 5, this corresponds to boron (B);Z = 6, this corresponds to carbon (C);Z = 7, this corresponds to nitrogen (N);Z = 8, this corresponds to oxygen, (O);Z = 9, this corresponds to fluorine, (F).

Now notice that each of these 9 elements can be found in the same row of the periodic table. This is period 2. We may then summarize that all of these elements belong to the same period, period number 2.