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You have a 4 L bottle of sulfuric acid solution. You take 50.0 mL of this H2SO4(aq) solution and titrate it to the endpoint with a 0.10 M NaOH solution. If the volume of NaOH solution needed is 60.0 mL, the concentration of the sulfuric acid (H2SO4) solution is:.

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Lelia Lubowitz
Lelia LubowitzLv2
7 Feb 2019
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Related questions

1-How many mL of a 7.4 M HCl solution would it take to make a 250 mL of a 1.5 M solution?

0.2

0

1233.33

0.4

50.68

2-What volume of 6.2 M NaOH is needed to completely titrate 0.9 L of 2.49 M sulfuric acid according to the equation:


H2SO4(aq)+2NaOH(aq)҆’Na2SO4(aq)+2H2O

4.48 L

0.18 L

13.89 L

722.9 L

0.72 L

a sample of sulfuric acid h2so4 with a volume of 10.4 ml is titrated with solution of naoh with a concentration of 1.17m the endpoint is reached after 22.2ml

1) A 24.00 Γ’ΒˆΒ’mL sample of an unknown HClO4 solution requires titration with 22.82 mL of 0.1900 M NaOH to reach the equivalence point.
What is the concentration of the unknown HClO4 solution? The neutralization reaction is:
HClO4(aq)+NaOH(aq)҆’H2O(l)+NaClO4(aq)

2) A 25.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.33 mL of NaOH solution is added.
What is the concentration of the unknown H3PO4 solution?

3) An acid solution is 0.100 M in HCl and 0.200 M in H2SO4.
What volume of a 0.140 M KOH solution would have to be added to 550.0 mL of the acidic solution to neutralize completely all of the acid?

4) A tanker truck carrying 2.01×103 kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuric acid solution is 95.0% H2SO4 by mass and has a density of 1.84 g/mL.
Sodium carbonate (Na2CO3) is used to neutralize the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 2.01×103 kg of sulfuric acid solution?

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