Problem: In a 0.20 M solution, a weak acid is 3.0% dissociated.(a) Calculate the [H3O+], pH, [OH−], and pOH of the solution.

🤓 Based on our data, we think this question is relevant for Professor Ison's class at NCSU.

FREE Expert Solution

Recall that the percent ionization is given by:


% ionization=[H3O+][HA]initial×100


pH=-log[H3O+]


pH+pOH=14


[OH-]=10-pOH


solve for [H3O+]:


3.0%=[H3O+]0.20×100

[H3O+]=0.20×3.0100

[H3O+] = 0.006 M


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Problem Details

In a 0.20 M solution, a weak acid is 3.0% dissociated.

(a) Calculate the [H3O+], pH, [OH], and pOH of the solution.

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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 Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ison's class at NCSU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.