What is the ph of an aqueous solution with a hydrogen ion concentration of [h+]=9.3×10−5 m? b. what is the hydroxide ion concentration, [oh−] , in an aqueous solution with a hydrogen ion concentration of [h+]=9.3×10−5 m?

Okey so [H+] = 9.3×10¯5 is given. From given data we can derive the following

Equation for pH is;

pH = - log [H+]

= - log (9.3×10¯5)

= - log 9.3 + log 10¯5

= - (0.9684 + (-5)

= - (-4.0316)

= 4.0316

The pH = 4.0316

(b.)

By using the equation ;

14 = pH + pOH

pOH = 14 - 4.0316 (calculated from above)

pOH = 9.9684

Since pOH = 9.9684

pOH = - log [OH-]

9.9684 = - log [OH-]

[OH-] = antilog (-9.9684)

[OH-] = 1.075 ×10¯(10)

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.