What is the pH of a 0.0001 M solution of HNO3? pOH?

Answer 1

#pH=-log_(10)H_3O^+#;

in water #pOH=14-pH#

#log_10{0.0001}# #=# #log_10(10^-4)=-4#, by definition of the log function. Thus #pH# #=# #4#, and, necessarily, #pOH=10#.

Note that you should understand #log# functions. When I write #log_aB=c#, I specify that #a^c=B#; thus #log_(10)100=2,log_(10)1000=3#, and #log_(10)10^(-1)=-1#. What are #log_(10)1,000,000#, and #log_(10)10^-6#?

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Answer 2

Ellie Andrews

To find the pH and pOH of a solution of HNO3, we need to consider that HNO3 is a strong acid and completely dissociates in water.

Given that the concentration of HNO3 is 0.0001 M, this is also the concentration of H+ ions in the solution.

pH: pH = -log[H+] = -log(0.0001) = -log(1 x 10^-4) = 4
pOH: pOH = -log[OH-] = -log(1 x 10^-14 / [H+]) = -log(1 x 10^-14 / 0.0001) = -log(1 x 10^-10) = 10

Therefore, the pH of the solution is 4 and the pOH is 10.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.