What is the pH of a solution that has a hydronium ion concentration of #1.00 times 10^-4 M#?

1 Answer

Answer:

pH = 4

Explanation:

To calculate the pH of a solution, use the equation

#pH = -log[H_3O^+]#

Since we are given the hydronium ion (#H_3O^+#) concentration of the solution, we can plug this value into the formula.

#pH = -log[1.00 xx 10^-4 M]#
#pH = 4#

The pH of this solution is 4.

Added notes:
#pH = pH_3O^+# because hydrogen ions attach to water molecules for form hydronium ions.

Some other key things to remember for pH calculations include:

pH + pOH = 14

pH = -log[#H^+#]
pOH = -log[#OH^-#]

#[H^+] = 10^(-pH)#
#[OH^-] = 10^(-pOH) #

The video below explains how to use all this information so that you can complete these types of calculations.

Hope this helps!