Topic: How do Strong Acids fully disassociate in water? (Read 2474 times)

akaEMILY · « **on:** March 21, 2012, 01:16:16 PM »

3. Determine the pH (to two decimal places) of the solution that is produced by mixing 98.9 mL of 6.56×10-4 M HNO3 with 9.27 mL of 4.46×10-3 M Na2O.

How does the chemical equation look? I don't know why, but I'm having difficulties with that. I know Na is a spectator ion and won't show in products.. once I balance that I'll know how to do the problem. I know HNO3 is a strong acid so the H proton will come off. But I have an extra O and it ruins my hydronium ion. A little hand and I'll be good!

HNO3 + Na2O + H2O -> ??

Borek · « **Reply #1 on:** March 21, 2012, 01:22:52 PM »

Ignore acid for a moment. What happens when you put the Na₂O in water?

akaEMILY · « **Reply #2 on:** March 21, 2012, 03:00:40 PM »

I get 2NaOH.

Borek · « **Reply #3 on:** March 21, 2012, 03:30:52 PM »

Good. Now add the acid to the equation.

Topic: How do Strong Acids fully disassociate in water? (Read 2474 times)

akaEMILY

How do Strong Acids fully disassociate in water?

Borek

Re: How do Strong Acids fully disassociate in water?

akaEMILY

Re: How do Strong Acids fully disassociate in water?

Borek

Re: How do Strong Acids fully disassociate in water?

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