I have two problems given in my textbook that the book unfortunately does not give a good amount of information on. I have the answers in the back of the book, but I need to know how to do this. So I hope someone can explain and show the work for the following problems.
Calculate the pH of the following solutions:
1.) 5.00g of HBr in 100 ml of aqueous solution
2.) 1.50g of NaOH in 50 ml of aqueous solution
Please show me the work and explain how to do these! The answers should be
1.) 0.209
2.) 13.875
1. 5g HBr = ? mole
molecular weight: H= 1, Br= 79.904
total molecular mass = 80.904
we know that
mass= mole * molar mass
5g/ 80.904= mole
mole = .o62
there are 0.062 moles in 100 ml or 0.1L = 0.62M
in HBr, there are 0.62 M H+ and 0.62 M Br
pH = -log[H+] = -log [0.62] = .2
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