Problem: Determine the pH of each solution.a solution that is 1.07% HCl by mass (Assume a density of 1.01  g / mL for the solution.)

FREE Expert Solution

We're asked to determine the pH of a solution that is 1.07% HCl by mass.


Recall that the pH of a solution is given by:


pH=-log H+

Take note that:         [H+] = [H3O+]


Since HCl is a strong acid, it will completely dissociate into ions in solution as follows:


HCl(aq)   H+(aq) + Cl(aq)


This means that:  [HCl] = [H+]

**Brackets, [] indicate concentration in molarity


We first need to determine the molarity of HCl.  


Recall that molarity (M) is given by:         

       

Molarity = mol soluteL solution


Since we’re given the mass percent (% by mass) and the density of HCl solution, we can find the number of moles of HCl and the volume of the solution


Recall that mass percent is given by:


mass percent =mass solutemass solution×100


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Problem Details

Determine the pH of each solution.

a solution that is 1.07% HCl by mass (Assume a density of 1.01  g / mL for the solution.)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.

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Based on our data, we think this problem is relevant for Professor Rabson's class at AMARILLO.