Problem: 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

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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:

pH=-log H3O+

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

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Problem Details

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

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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 Chibba & Davis' class at McMaster University.