We are asked to calculate the pH of the solution with 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl.
The pH of a compound determines its acidity.
▪ pH stands for the negative logarithmic function of hydronium ion concentration
▪ can be calculated using the following equation:
Strong acids are considered strong electrolytes. They completely dissociate into ions when dissolved in water.
• Strong binary acids – paired with a highly electronegative atom
Strong binary acids are: HCl, HBr, and HI
• Strong oxyacids (or oxoacids) - have 2 or more oxygens than hydrogens
Oxyacids → possess H+ ion, connected to nonmetal and oxygen
Common strong oxyacids are: HNO3, HClO3, HClO4, H2SO4
Exceptions to the rule are: Oxalic acid (H2C2O4) and Iodic acid (HIO3)
▪ both have 2 more O than H but are weak acids because carbon and iodine have low electronegativity
Determine the pH of each solution.
a solution that is 4.7×10−2 M in HClO4 and 5.1×10−2 M in HCl
Frequently Asked Questions
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 Chibba & Davis' class at McMaster University.