Question

Sodium carbonate (Na2CO3) is used to neutralize the sulfuric
acid spill. How many kilograms of sodium carbonate must be added to
neutralize 4.03×10^{3} kg of sulfuric acid solution?

Answer #1

H2SO4 + Na2CO3 -------------------> Na2SO4 + CO2 + H2O

1 mol of Na2CO3 is required ------------ to neutralise 1 mol of H2SO4 spilt.

mass of H2SO4 = 4.03 x 10^3 kg = 4.03 x 10^6 g

BUT it is only 95% H2SO4,

so mass H2SO4 = 95/100 x (4.03x10^6) g

= 3.8285x10^6 g

moles H2SO4 = mass / molar mass

= 3.829x10^6 g / 98.1 g/mol

= 3.903 x10^4 moles

So you will need 3.904 x 10^4 moles of Na2CO3 to neutralise it.

moles = mass / molar mass

mass of Na2CO3 = 3.903 x 10^4 moles x 106

= 4.14 x 10^6 g of Na2CO3

= 4.14 x 10^3 kg

**mass of Na2CO3 = 4136.8 kg**

**= 4.14 x 10^3 kg**

Sodium carbonate (Na2CO3) is used to neutralize the sulfuric
acid spill. How many kilograms of sodium carbonate must be added to
neutralize 3.02×103 kg of sulfuric acid solution?

A tanker truck carrying 6.05×103 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.
Part A
Sodium carbonate (Na2CO3) is used to neutralize the sulfuric
acid spill. How many kilograms of sodium carbonate must be added to
neutralize 6.05×103 kg of sulfuric acid solution?
Express your answer with the appropriate units.

A tanker truck carrying 6.05×103 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 (Na2O3 ) is used to neutralize the sulfuric acid
spill. How many kilograms of sodium carbonate must be added to
neutralize 6.05×103 kg of sulfuric acid solution?

1)Write the balanced reaction for the reaction of sodium
carbonate with sulfuric acid with phase descriptors. 2)Write the
balanced reaction for the reaction of sodium bicarbonate with
sulfuric acid with phase descriptors. 3)What solid product
will be isolated from both reactions? 4)What is the molar mass of
this solid product? 5)What is the molar mass of sodium bicarbonate?
and 6)What is the molar mass of sodium carbonate? 7)Why would the
evaporation step be performed in the fume hood?
1 &...

Hydrochloric acid (HCl) reacts with sodium carbonate (Na2CO3),
forming sodium chloride (NaCl), water (H2O), and carbon dioxide
(CO2). This equation is balanced as written:
2HCl(aq)+Na2CO3(aq)→2NaCl(aq)+H2O(l)+CO2(g)
A 327-mL sample of unknown HCl solution reacts completely with
Na2CO3 to form 18.1 g CO2. What was the concentration of the HCl
solution?

What volume of 0.250m nitric acid is required to neutralize 4.8mL
of 0.150m sodium carbonate?

Sodium carbonate nuetralizes H2SO4 as shown below in
the reaction:
Na2CO3 (s) + H2SO4 (aq) -->Na2SO4 (aq) + H2O (l)
+CO2 (g)
How many grams of sodium carbonate are required to
nuetralize 455ml of 5.4% ( W/V) solution of H2SO4?

How many lbs/day of pure sodium hydroxide are required to
neutralize an industrial waste with an acidity equivalent to 20
lbs/day of sulfuric acid? H2SO4 + NaOH = H2O + Na2SO4 (unbalanced
equation)

What is the molarity of a sulfuric acid solution if 60.00 mL of
H2SO4 is required to neutralize 0.420 g of sodium hydrogen
carbonate (84.01
g/mol)?
H2SO4(aq) + 2 NaHCO3(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g)

1. TITRATION PROBLEM:
Oxalic acid is a diprotic acid. Calculate the percent of oxalic
acid (H2C2O4) in a solid given that a 0.7984 gram sample of that
solid required 37.98 mL of 0.2283 M NaOH for neutralization. Show
your work!
2. TITRATION PROBLEM:
Some sulfuric acid is spilled on a lab bench. You can neutralize
the acid by sprinkling sodium bicarbonate on it and then mopping up
the resultant solution.
2 NaHCO3(s) + H2SO4(aq) --> Na2SO4(aq) + 2 CO2(g) +...

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