Calculate the concentrations of H₃O⁺ and the pH of each acidic solution. Since HCl is a monoprotic acid, the H₃O⁺ concentration is equivalent to the HCl molarity.

I don't have any numbers though. It's a Late Nite Lab. I can look for numbers in the data window if needed, but really all I have is the color of the solutions.

So basically what I am asking for is the procedure for how I would come about finding the pH level and concentrations. Does that make sense..? Thanks!

Question

Calculate the concentrations of H₃O⁺ and the pH of each acidic solution. Since HCl is a monoprotic acid, the H₃O⁺ concentration is equivalent to the HCl molarity.

I don't have any numbers though. It's a Late Nite Lab. I can look for numbers in the data window if needed, but really all I have is the color of the solutions.

So basically what I am asking for is the procedure for how I would come about finding the pH level and concentrations. Does that make sense..? Thanks!

goformit100 · Answer

use the IONIC BALANCING METHOD for solving it

anonymous · Answer

I am not sure what that is? I haven't learned that..

anonymous · Answer

A solution that contains H₃O⁺ ions is considered to be acidic and a solution that contains OH⁻ ions is considered to be basic. The pH is a logarithmic measurement scale used to describe the acidity of a solution, and it is calculated from the equation: 

     pH= -log [H₃O⁺]

For example, a solution that is 1M in H₃O⁺ has a pH of 0, while a solution that is .001M in H₃O⁺ has a pH of 3. A pOH scale is defined in the similar way, based on the OH⁻ concentration. The equation to calculate pOH is: 

     pOH= -log [OH⁻]

Pure water exhibits autoionization of the H₂O molecules into H₃O⁺ and OH⁻ ions at a concentration that is equivalent to a pH of 7. Therefore, for any aqueous solution the sum of the values pH + pOH is always 14.

pH indicators are organic acids that change color depending on the acidity (pH) of the solution. They are selected for their intense colors even when only a few drops are added to a solution. These indicators have a particular pH range over which they make a transition from one color to another (and some indicators have multiple ranges).

In this experiment you will investigate different indicators with solutions of varying pH. Solutions of HCl and NaOH will be diluted with water to obtain a range of pH values.

Your job is to identify the pH range for which each given pH indicator is most effective.

You will be asked to set up sets of test tubes containing dilute acid or base at various concentrations in order to test the pH indicators. A sample of what you are looking for as well as a convenient way to arrange the sets of test tube on the workbench is shown in the following link: 
m-cresol sample

That is the background given to me if that helps?

goformit100 · Answer

you can refer to J.D.Lee book

anonymous · Answer

Not to sound silly, but is that online..? And thanks for your help!

goformit100 · Answer

that book is online......

anonymous · Answer

Okay. Thanks!