1.Write the molecular equation and the net ionic equation for the reaction of H2SO4 with NaOH.
2. Exactly 25.00 mL of 0.1522 M H2SO4 were needed to titrate 45.25 mL of NaOH according to the balanced equation in the problem above. Calculate the moles of NaOH needed for the reaction. Calculate the molarity of the NaOH solution.
3. One group of students made an error by using HCl instead of H2SO4 to titrate an unknown solution of NaOH. Would this error change the calculated molarity of the NaOH solution? Explain your answer.
4. Calculate the grams of Na2CO3 needed to react with 25.0 mL of 0.220 M HCl solution if one mole of Na2CO3 reacts with 2 moles of HCl.
5. What volume of 0.10 M NaOH is required to titrate 12 mL of vinegar that contains 5% by weight of acetic acid. They density of the vinegar is 1.00 g/mL.
There are multiple questions here . i am allowed to answer only 1 at a time. I will answer 1st 2 question for you.Please ask other as different question.
2NaOH (aq) + H2SO4 (aq) --> Na2SO4 (aq) + 2 H2O (l)
H+ (aq) + OH- (aq) ---> H2O (l)
number of moles of H2SO4 = M*V = 0.1522 M * 0.025 L =3.805*10^-3 mol
From equation above:
number of moles of NaoH required = 2* number of moles of H2SO4
= 2* 3.805*10^-3
= 7.61*10^-3 mol
Answer: 7.61*10^-3 mol
Molarity of NaOH = number of moles/ volume
= 7.61*10^-3 mol / 0.04525 L
= 0.168 M
Answer: 0.168 M
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