Answer:
1. [H⁺] = 1.58×10¯¹⁰ mol/L
2. pH = 9.8
3. pOH = 4.2
Step-by-step explanation:
We'll begin by calculating the pOH of the solution. This can be obtained as follow:
Concentration of Hydroxide ion [OH¯] = 5.8×10¯⁵ mol/L
pOH =?
pOH = –Log [OH¯]
pOH = –Log 5.8×10¯⁵
pOH = 4.2
Next, we shall determine the pH of the solution. This can be obtained as follow:
pOH = 4.2
pH =?
pH + pOH = 14
pH + 4.2 = 14
Collect like terms
pH = 14 – 4.2
pH = 9.8
Finally, we shall determine the concentration of Hydrogen ion [H⁺] in the solution. This can be obtained as follow:
pH = 9.8
Concentration of Hydrogen ion [H⁺] =?
pH = –Log [H⁺]
9.8 = –Log [H⁺]
Multiply through by –1
–9.8 = Log [H⁺]
Take the anti log of –9.8
[H⁺] = antilog (–9.8)
[H⁺] = 1.58×10¯¹⁰ mol/L
SUMMARY:
1. [H⁺] = 1.58×10¯¹⁰ mol/L
2. pH = 9.8
3. pOH = 4.2