Pure water has a hydrogen ion concentration of 1 × 10−7 m and a ph of 7. a student measures a basic solution and finds that it has a hydrogen ion (h+) concentration of 1 × 10−3. explain why the student must have made an error in her measurement.

Explanations:- Pure water is pH is 7 means it is neutral. If the solution is neutral then it must have equal concentrations of and .

So, if for the pure water, hydrogen ion concentration is then hydroxide ion concentration must also be .

The solution will be acidic if hydrogen ion concentration is greater than hydroxide ion concentration and the solution will be basic if hydroxide ion concentration is greater than hydrogen ion concentration.

For acidic solution, >

and for basic solution, >

A student measures a basic solution then the hydrogen ion concentration must be be less than but he find the hydrogen ion concentration of which is totally an error.

[tex]pH=-log1*10^-^3

pH = 3

A solution is neutral if its pH is 7, it is acidic if the pH is below 7 and basic if the pH is greater than 7.

Since the pH from the measured hydrogen ion concentration is 3 which is less than 7, the solution is acidic where as the student measured a basic solution. So, it's indicating an error in her measurements.

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.