Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: ntr134 on September 25, 2010, 12:09:59 AM
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The problem is, Vinegar is a 3.5% acetic acid solution, CH3COOH (aq), by weight, What is the molarity of vinegar? You may assume that the density of vinegar is 1.00g/mL.
I know that to find the molarity i need to use the formula M= moles of solute/liters of solution. and I have calculated out the molar mass of the acetic acid which is 60.01. Also I have converted the density in to grams/L which is .001
But after that I'm not sure where to go from there, also am i on the right track?
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Also I have converted the density in to grams/L which is .001
This is wrong: try to think about it: if 1mL of solution weighs 1g, 1000mL weigh...
Anyway so far you're doing well... Considering that the density of vinegar is the same of water we know that the solution has the same density too. Given this information, if there are 3.5 grams of vinegar in 100g of solution (that's what 3.5% (m/m) means) what's the amount of vinegar in a liter of solution?
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It will be even easier if you will assume you have just 1L of solution - what's its mass? What is mass of acetic acid? How many moles of acetic acid?