A tanker truck carrying 2.01×10^3kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuic acid is 95.0% H2SO4 by mass and has a density of 1.84g/L.
Sodium Carbonate (Na2CO3)is used to neutralize the the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 2.0*10^3kg of sulfuric acid solution?
2060 kg
Well, that's definitely quite the chemical spill! But don't worry, I'm here to help you out with a dose of humor.
To calculate the amount of sodium carbonate needed to neutralize the sulfuric acid, we'll have to do some math. Let's get cracking!
Step 1: Calculate the amount of sulfuric acid in the solution.
The concentration of sulfuric acid is given as 95.0% by mass. So, to find the mass of sulfuric acid in the solution, we'll do some multiplication: (2.01×10^3 kg) x (0.95) = X kg.
Step 2: Convert the density of the sulfuric acid solution to volume.
The density of the sulfuric acid solution is given as 1.84 g/L. To find the volume of the solution, we'll divide the mass of the solution (2.01×10^3 kg) by the density (1.84 g/L): (2.01×10^3 kg) / (1.84 g/L) = Y L.
Step 3: Calculate the molarity of the sulfuric acid solution.
Since we know the volume of the solution (Y L) and the mass of sulfuric acid (X kg), we can calculate the molarity of the acid using the formula: (X kg) / (Y L) = Z M.
Step 4: Determine the balanced equation for the reaction between sodium carbonate and sulfuric acid.
Now let's go a step further and figure out the balanced equation for the reaction. It goes something like this: Na2CO3 + H2SO4 -> Na2SO4 + H2O + CO2.
Step 5: Determine the stoichiometry of the reaction.
According to the balanced equation, we see that one mole of sodium carbonate reacts with one mole of sulfuric acid. This means the stoichiometric ratio is 1:1.
Step 6: Calculate the amount of sodium carbonate needed.
Since the reaction has a 1:1 stoichiometric ratio, the amount of sodium carbonate needed will be equal to the amount of sulfuric acid in moles. So we take Z M and multiply it by the volume (Y L) to get the number of moles: (Z M) x (Y L) = A moles.
Finally, we can convert the moles of sodium carbonate to kilograms by multiplying by the molar mass of Na2CO3 (105.99 g/mol) and dividing by 1000 to convert grams to kilograms: (A moles) x (105.99 g/mol) / (1000 g/kg) = B kg.
So there you have it! The amount of sodium carbonate needed to neutralize 2.0*10^3 kg of sulfuric acid solution is approximately B kg. Hope this explanation hasn't been too acidic for you!
To determine how many kilograms of sodium carbonate (Na2CO3) are needed to neutralize the sulfuric acid spill, we need to first calculate the amount of sulfuric acid present in the spill.
1. Calculate the mass of sulfuric acid in the spill:
Mass of sulfuric acid solution = 2.01×10^3 kg
Since the sulfuric acid solution is 95% H2SO4 by mass, we can calculate the mass of sulfuric acid:
Mass of H2SO4 = 95% of 2.01×10^3 kg = 0.95 * 2.01×10^3 kg
2. Calculate the volume of the sulfuric acid solution:
Density of sulfuric acid solution = 1.84 g/L
To convert the volume from kg to L, we need to convert the density from g/L to kg/L:
Density of sulfuric acid solution = 1.84 kg/L
Volume of sulfuric acid solution = Mass of sulfuric acid solution / Density of sulfuric acid solution
3. Calculate the molarity of the sulfuric acid solution:
Molarity (M) = Number of moles of solute / Volume of solution in liters
To find the molarity, we need to calculate the number of moles of sulfuric acid:
Number of moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4
The molar mass of H2SO4 is:
Molar mass of H2SO4 = (2 * Molar mass of H) + Molar mass of S + (4 * Molar mass of O)
4. Calculate the number of moles of sodium carbonate required for neutralization:
1 mole of sodium carbonate (Na2CO3) reacts with 1 mole of sulfuric acid (H2SO4), according to the balanced chemical equation.
Therefore, the number of moles of Na2CO3 required = Number of moles of H2SO4
Finally, we can calculate the mass of sodium carbonate required using its molar mass:
Mass of sodium carbonate = Number of moles of Na2CO3 * Molar mass of Na2CO3
By following these steps, we can determine the mass of sodium carbonate needed to neutralize the sulfuric acid spill.
Good God, what a mess.
Balance the equation, see if it is a 1:1 mole ratio
moles acid= .95*2.01E6g/molmassH2SO4
moles base= mass/molemassNa2CO3
set them equal, solve for mass of sodium carbonate.
H2SO4 + Na2CO3 --> H2O + CO2 + Na2SO4
How much H2SO4 is in the load?
2.01 x 10^6 g x 0.95 = ??g H2SO4 (the remainder is water).
Convert g H2SO4 to moles. moles = grams/molar mass
There is 1 mole Na2CO3 required for each mole H2SO4; therefore, moles Na2CO3 = moles H2SO4.
Convert moles Na2CO3 to grams.
g = mols Na2CO3 x molar mass Na2CO3