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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: prakashreddy on May 19, 2015, 12:00:24 AM

Title: Help with Concentration, Molarity of an acid/base neutralization
Post by: prakashreddy on May 19, 2015, 12:00:24 AM

Can you please help me with this question?

Tartaric acid (H2C4H4O6) is neutralized with 0.100M NaOH. A sample of 3.0 g of tartaric acid reacts with 45 ml of base. How concentrated is the base?

I calculated moles of NaOH by multiplying (45/1000)*0.1=0.0045 moles of NaOH.
I can also calculate moles of tartaric acid = 3 g x (1 mole of tartaric acid/150g)=0.02 moles of acid. I am stuck after this step…not sure if i am on the right track. Can someone please help? thank you so much!!

Title: Re: Help with Concentration, Molarity of an acid/base neutralization
Post by: Hunter2 on May 19, 2015, 02:40:52 AM

You calculated the moles of the acid. How much moles of NaOH correspond to the acid.
If you have this then you know the amount in 45 ml. Concentration is easy to calculate then.

Title: Re: Help with Concentration, Molarity of an acid/base neutralization
Post by: Borek on May 19, 2015, 02:48:03 AM

In general: start with the reaction equation.