Question

5. What is the pH of a solution with a OH concentration of 2.52 x 10'M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 6. What is the pH of a solution with a H2O* concentration of 2.7 x 10 M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 7. What is the pH of a solution with a OH concentration of 5.53 x 10-M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer

Answer 1

5.

We have

[OH^-] = 2.52 $\times$ 10^-9 M

We know that

pOH = -log[OH^-] and pH + pOH = 14 and pH = -log[H⁺]

So

pOH =-log[OH^-] = -log (2.52 $\times$ 10^-9 ) = 8.59

then pH = 14 - pOH = 14 - 8.59 = 5.41

pH = 5.41

WE know that

if pH is less than 7 then solution is acidic

if pH is equal 7 then solution is neutral

if pH is more than 7 then solution is basic

here pH is 5.41 which is less than 7 so solution is Acidic

Answer = pH = 5.41 , Solution is Acidic

6.

We have

[H₃O⁺] = 2.7 $\times$ 10^-5 M

We know that

pH = -log[H⁺] = -log[H₃O⁺]

So

pH =-log[H₃O⁺] = -log (2.7 $\times$ 10^-5 ) = 4.56

pH = 4.56

We know that

if pH is less than 7 then solution is acidic

if pH is equal 7 then solution is neutral

if pH is more than 7 then solution is basic

here pH is 4.56 which is less than 7 so solution is Acidic

Answer = pH = 4.56 , Solution is Acidic

7.

We have

[OH^-] = 5.53 $\times$ 10^-3 M

We know that

pOH = -log[OH^-] and pH + pOH = 14

So

pOH =-log[OH^-] = -log (5.53 $\times$ 10^-3 ) = 2.25

then pH = 14 - pOH = 14 - 2.25 = 11.75

pH = 11.75

We know that

if pH is less than 7 then solution is acidic

if pH is equal 7 then solution is neutral

if pH is more than 7 then solution is basic

here pH is 11.75 which is more than 7 so solution is Basic

Answer = pH = 11.75 , Solution is Basic