Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: MegaBabyRawr on April 21, 2016, 10:11:59 PM
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So currently, I am doing titration labs in my chemistry class, but i need some help understanding it. This is what I think it is:
A base can neutralize (is neutralize the right word, what i mean is bring to the end point) an acid. 1mL of the .5M base can neutralize the 1mL of the .5M acid. (This is just an example) If you add 500mL of the acid and 5000mL of water together, then add 500mL of the base, it should still neutralize completely right?
The dilution would not affect the base and acid bringing each other to the endpoint right?
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A base can neutralize (is neutralize the right word, what i mean is bring to the end point) an acid.
Yes. It is more accurate to say 'alkali' instead of 'base' - alkalis are soluble bases.
1mL of the .5M base can neutralize the 1mL of the .5M acid. If you add 500mL of the acid and 5000mL of water together, then add 500mL of the base, it should still neutralize completely right?
Not really. Have you heard about dibasic acid or tribasic acid?
The dilution would not affect the base and acid bringing each other to the endpoint right?
What do you mean by 'would not affect'? The general ionic equation for neutralisation reaction (H+ + OH- :rarrow: H2O) is the same for any bases and acids of any concentrations. However, dilution does affect the volume of acid/base required to reach the end point.
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A base can neutralize (is neutralize the right word, what i mean is bring to the end point) an acid.
Yes. It is more accurate to say 'alkali' instead of 'base' - alkalis are soluble bases.
1mL of the .5M base can neutralize the 1mL of the .5M acid. If you add 500mL of the acid and 5000mL of water together, then add 500mL of the base, it should still neutralize completely right?
Not really. Have you heard about dibasic acid or tribasic acid?
The dilution would not affect the base and acid bringing each other to the endpoint right?
What do you mean by 'would not affect'? The general ionic equation for neutralisation reaction (H+ + OH- :rarrow: H2O) is the same for any bases and acids of any concentrations. However, dilution does affect the volume of acid/base required to reach the end point.
Sorry what that was just to be an example of a reaction. In my lab, we added acid to the base until it changed colour (end point). What I am wondering is, does it matter how diluted the base is (how much extra water was added). Will it affect the reaction?
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The reaction is not affected.
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1mL of the .5M base can neutralize the 1mL of the .5M acid. (This is just an example)
Why not just state "reaction proceeds according to the stoichiometry of the neutralization reaction"? You know how to write and balance the reaction equation between an acid and a base, don't you? Sure, you can use formula as often given, but it just makes you forgot the basics.
What I am wondering is, does it matter how diluted the base is (how much extra water was added). Will it affect the reaction?
In general - no. In practice using too diluted titrant is impractical and can be source of additional problems. See http://www.titrations.info/titrant-and-sample-volume