Determine the ph of the following base solutions. (assume that all solutions are at 25°c and the ion-product constant of water, kw, is 1.01 ✕ 10−14.) (a) 1.39 ✕ 10−2 m naoh webassign will check your answer for the correct number of significant figures. (b) 0.0051 m al(oh)3 webassign will check your answer for the correct number of significant figures.

a) The pH of the solution is 12.13.

b) The pH of the solution is 12.17.

Explanation:

Ionic product of water =

Taking negative logarithm on both sides:

The pH is the negative logarithm of hydrogen ion concentration in solution.

The pOH is the negative logarithm of hydroxide ion concentration in solution.

a) of NaOH.

Concentration of hydroxide ions:

So,

pH=13.99-1.86=12.13

b) of NaOH.

Concentration of hydroxide ions:

So,

pH=13.99-1.82=12.17

elements

explanation:

yes the other ones are right just show me a pic of ur face cuz u look hot

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.