A tanker truck carrying 2.01×10 3 kg of concentrated sulfuric acid solution tips
ID: 951364 • Letter: A
Question
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? Express your answer with the appropriate units.
A 35.00 mL sample of an unknown H3PO4solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.28 mLof NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3PO4(aq)+3NaOH(aq)3H2O(l)+Na3PO4(aq)
Explanation / Answer
mass of H2SO4 = 2.01 x 10^3 x 95% = 1909.5 kg
moles of H2SO4 = 1909.5 x 19^3 / 98 = 19484.7 moles
H2SO4 + Na2CO3 ----------------> Na2SO4 + H2O + CO2
moles of H2SO4 = moles of Na2CO3
moles of Na2CO3 = mass / molar mass
19484.7 = mass / 106
mass of Na2CO3 = 2.06 x 10^6 g
= 2.06 x 10^3 kg
2)
H3PO4(aq)+3NaOH(aq)3H2O(l)+Na3PO4(aq)
H3PO4 volume = 35 mL
NaOH concentration = 0.1 M
volume of NaOH = 26.28 mL
from relation
M1 V1 / n1 = M2 V2 / n2
M1 x 35 / 1 = 0.1 x 26.28 / 3
M1 = 0.025 M
concentration of H3PO4 = 0.025 M
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