Question

The pH of solution A is 2.4​, while the pH of solution B is 9.4.

​(a) What are their​ hydrogen-ion concentrations?
​(b) How many times greater is the​ hydrogen-ion concentration of solution A than that of solution​ B?
​(c) By how many orders of magnitude do the concentrations​ differ?

Answer 1

Given:

The pH of solution A = 2.4

The pH of solution B = 9.4.

Solution:

The hydrogen ion concentration is the amount of hydrogen ions present in the given solution usually expressed in terms of moles pere litre .

(A) hydrogen-ion concentrations of the solution.

`H^+= 10^(-pH)`

Now,

The hydrogen ion concentration of the solution A

`H^+= 10^(-2.4)`

`H^+= 3.981* 10^(-3)`

Similarly

hydrogen ion concentration of the solution B

`H^+= 10^(-9.4)`

`H^+= 3.981* 10^(-10)`

​(b) The hydrogen ion concentration of solution A
`3.981* 10^(-3)` is and the solution B is
`3.981* 10^(-10)`

so we can conclude that the hydrogen ion concentration of solution A is
`10^ 7` times greater than solution B

(c) The solutions A and Solution B differ by 7 order of magnitude