Chemistry Help Please

Question

Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate whether the solutions are acidic, basic or neutral. Report your answers to 3 sig figs.

a) [H+] = 8.93 ×10−12×10-12 M pH =  pOH = 

     Acidic, basic, or neutral? 

b) [H+] = 4.68 ×10−10×10-10 M pH =  pOH = 

     Acidic, basic, or neutral?  

c) [OH−] = 5.05 ×10−13×10-13 M pOH =  pH = 

     Acidic, basic, or neutral? S

d) [OH−] = 4.98 ×10−6×10-6 M pOH =  pH = 

     Acidic, basic, or neutral? 

Answer 1

Here's what you need to know:

pH + pOH = 14

pH = -log [H⁺]

pOH = -log [OH^-]

acid = pH < 7

basic = pH > 7

neutral = pH 7

a). [H+] = 8.93x10^-12 M

pH = -log 8.93x10^-12

pH = 11.0

pOH = 14 - pH = 14 - 11.0 = 3.00

solution is basic (pH > 7)

b). Do it the same as for (a)

c). [OH^-] = 5.05x10^-13 M

pOH = -log 5.05x10^-13

pOH = 12.3

pH = 14 - pOH = 14 - 12.3 = 1.7

solution is acid (pH < 7)

d). Do it the same as for (c)