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Chapter 15: Problem 58

Calculate the \(\mathrm{pH}\) of a 0.0316 \(\mathrm{M}\) solution of the strong base RbOH.

Short Answer

Expert verified
The pH of a 0.0316 M solution of the strong base RbOH is approximately 12.5.

Step by step solution

01

Properties of strong bases

RbOH is a strong base. This means that it dissociates completely in an aqueous solution, yielding hydroxide ions (OH-) and Rb+ ions. Hence, the concentration of OH- is the same as that of RbOH, which is 0.0316 M in this case.
02

Calculate the pOH first

To find the pH of this base solution, it will be useful to first calculate the pOH. The pOH is calculated as the negative logarithm of the concentration of OH- in the solution. So, use the formula pOH = -log [OH-]. Plugging in the given concentration, the pOH becomes -log(0.0316).
03

Evaluate the numerical value

Using a calculator, -log(0.0316) equals approximately 1.50. So, the pOH of this solution is 1.50.
04

Calculate the pH

Then, one can use the relationship between pH and pOH in water, which is pH = 14 - pOH. Substituting the calculated value pOH = 1.50 into the equation, the resulting pH value is 14 - 1.50 = 12.5.

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