A solution of 0.2 m sulfiric acid is titrated with a 0.2 m basic solution. In three to five sentences, explain how you can use the results of the titration as evidence for the ratio of sulfiric acid and the base in the balanced chemical reaction for the titration.
First let me say that this is one of the worst stated problems I've seen in years. It could be answered easily IF we knew which base was used. Since the base is not given we can look at two scenarios. The first is with a monobasic base and the second with a dibasic base. Take NaOH as the first one and Ba(OH)2 for the second.
1. H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
If you titrate 0.2 M H2SO4 with 0.2 M NaOH you see that it take twice as much NaOH to titrate the same amount of H2SO4 BECAUSE H2SO4 has TWO H ions to neutralize but NaOH has only ONE OH to do that so it takes twice as much NaOH to do the job. Therefore, it you start with 25 mL of H2SO4 you know it will take twice that much (50 mL) of the same molarity NaOH.
2. If we use Ba(OH)2 as the base then
H2SO4 + Ba(OH)2 ==> BaSO4 + 2H2O.
You see here that the ratio of acid to base is 1:1 so if you take 25 mL of H2SO4 you will titrate it with 25 mL Ba(OH)2.
Another note: Please note that you used the lower case m. Note that m stands for molality while M stands for molarity They aren't the same thing. You want to titrate with solution of known M and not m.
M stands for moles/liter of solution while m stands for moles/kg solvent.
Another note: We could have taken a tribasic base such as Al(OH)3 in which case the ratio is 3 acid:2 base as follows:
3H2SO4 + 2Al(OH)3 ==> Al2(SO4)3 + 6H2O so using 30 mL H2SO4 to start will require 30 x (2/3) = 20 mL of the base.
Well, my dear confused friend, let me try to lighten up this titration party with some humor and explanation. Imagine the sulfuric acid is like a grumpy cat and the basic solution is like a sunny puppy. When you mix them together through titration, they have a chemical reaction and want to find a balance, just like how a cat and a dog might need to figure out how to coexist under one roof. The results of the titration, such as the amount of base solution needed to neutralize the acid, can help us determine the ratio of the acid and base in the balanced chemical reaction. It's like discovering how many belly rubs the dog needs before the cat finally accepts its presence. So, keep calm, hold tight, and let the chemistry circus unfold! 🎪🔬
In a titration, a solution of known concentration (the titrant) is added to a solution of unknown concentration (the analyte) until the reaction between the two is complete. The key concept in this scenario is stoichiometry, which relates the balanced chemical equation with the reaction taking place. If the balanced equation for the titration is known, and assuming that the reaction is quantitative, the ratio of the sulfiric acid and the base can be determined. By measuring the volume of titrant needed to neutralize the analyte, one can calculate the number of moles of acid and base present. Dividing these values by their respective stoichiometric coefficients in the balanced equation will provide the ratio.
In a titration, the ratio of the reactants can be determined by analyzing the stoichiometry of the balanced chemical equation. In this case, since both the sulfiric acid and the base have the same concentration of 0.2 M, their ratio in the balanced equation can be directly determined from the volume required for the reaction to reach completion. By measuring the volume of the base solution required to neutralize the acid solution, you can calculate the moles of base used. Comparing this to the moles of acid present in the solution will allow you to infer the ratio of sulfiric acid and the base in the balanced chemical reaction.
