An aqueous solution at 25 °C is 10.8% HNO3 by mass and has a density of 1.044 g/mL. What is the pH?
The solution is 10.8 % by mass which means 10.8 g of HNO3 is present in 100g of solution.
Thus 1000g of solution has 108 g of nitric acid
the solution has density of 1.044 g/mL
Volume of the solution = mass / density = 1000g/ 1.044g/mL= 957.85 mL
molar mass of HNO3 = 63 g/mL
MOlarity of solution = number of moles/ Volume in L
= [108/63]/ (957.85 /1000) = 1.789 M
pH is defined only for dilute solutions with molarity ranging from 1M(H+) acid to 1M base(OH-).
Thus pH is not defined for this solution.
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