A railroad tank car derails and spills 36 tons of concentrated sulfuric acid. The acid is 98.0 mass% H 2 SO 4 and has a density of 1.836 g/mL. (b) How many kilograms of sodium carbonate are needed to completely neutralize the acid?

Welcome back everyone in a laboratory. A student accidentally spills 300 g of glacial acetic acid which is 99.5% acetic acid by mass, calculate the mass and grams of sodium bicarbonate required to neutralize the spill. Let's recall that sodium bicarbonate is represented by the formula N a H C 03. Where we would recognize that it's considered a weak base. Whereas our acetic acid we want to recognize is a weak acid. So reacting the two, we would have acetic acid, CH three C 02 H reacting with sodium bicarbonate, N A H C 03 to produce on our product side are conjugate base of our weak acid which is going to be sodium acetate. So that would be CH three C 02 N. A. And this is the salt of our conjugate base. We would also form carbon dioxide and water as our products. Since our acid is going to be donating a proton to form a bond with the hydrogen and oxygen atom in our sodium bicarbonate. So now that we have this reaction, let's make sure everything is balanced. And looking at all of our atoms on both sides of our equation are react inside and our product side, we can confirm that all of our atoms are actually balanced when you count them out. So we're just going to put a check mark for the fact that this equation is balanced as is with no needed additional coefficients. So what we're going to do now is take note of our mass of our acetic acid. So according to the prompt. So for our mass of ch three c 02 H we have a mass of 300 g and were given the percent by mass of acetic acid as 99.5% which we're going to interpret as decimal being 0.995. And so multiplying these two values, this gives us our massive acetic acid being 298. g. Now we want to make note of our molar mass of acetic acid from our periodic table, Where we will see that for every atom in acetic acid, we have a molar mass of 60.05 g per mole. We also want to make note of our molar mass of sodium bicarbonate from the periodic table of n a h c 03. And we would see that sodium bicarbonate corresponds to the molar mass of 84.1 g per mole. So now we're going to get into stock geometry to figure out our final answer which is our mass of sodium bicarbonate and grams required to neutralize the acetic acid spill. So beginning with what we know, we're going to begin with that mass, we calculated of 298.5 g of our acetic acid, ch three c 02 H. We're going to go from grams of acetic acid, two moles of acetic acid. By utilizing our molar mass, which we noted down is 60.5 g for one mole of acetic acid, allowing us to cancel out grams of acetic acid so far. And sorry, this is grams over here. So now we're at moles of acetic acid. We want our final answer to end up with sodium bicarbonate. So just to make more room here and let's fix this just to make more room. Our next conversion factor is to use our bounced equation to go from moles of acetic acid, two moles of sodium bicarbonate. Based on our balanced equation, we see we have a molar ratio where we have a coefficient of one in front of sodium bicarbonate and a coefficient of one in front of our acetic acid. So we have a 1-1 molar ratio which allows us to go from moles of acetic acid to now moles of sodium bicarbonate. Where we need to end up with our mass and grams of sodium bicarbonate. So continuing the calculation below, we're going to utilize that molar mass of our sodium bicarbonate. Where we see that we have from going from moles of sodium bicarbonate in the denominator. So it can cancel out two g of sodium bicarbonate. We have an equivalent of 84.01 g for one mole of sodium bicarbonate. Because our moles of sodium bicarbonate are aligned diagonally. We can cancel them out. And for our final unit, we're left with grams of sodium bicarbonate, which is going to give us our final answer of our Weak base, needed to neutralize our weak acid acetic acid of 417.6 g of sodium bicarbonate needed. So this is needed to neutralize the spill, and this would be our final answer to complete this example. So I hope this was helpful if you have any questions, leave them down below and I'll see everyone in the next practice video.

Ch.17 - Applications of Aqueous Equilibria

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McMurry 8th Edition

Ch.17 - Applications of Aqueous Equilibria

Problem 153b

Chapter 17, Problem 153b

A railroad tank car derails and spills 36 tons of concentrated sulfuric acid. The acid is 98.0 mass% H₂SO₄ and has a density of 1.836 g/mL. (b) How many kilograms of sodium carbonate are needed to completely neutralize the acid?

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Determine the mass of pure \( \text{H}_2\text{SO}_4 \) in the spill by multiplying the total mass of the acid by the mass percentage of \( \text{H}_2\text{SO}_4 \) (98.0%).

Convert the mass of \( \text{H}_2\text{SO}_4 \) from tons to grams, knowing that 1 ton is equal to 907,185 grams.

Calculate the number of moles of \( \text{H}_2\text{SO}_4 \) using its molar mass (98.08 g/mol).

Write the balanced chemical equation for the neutralization reaction: \( \text{H}_2\text{SO}_4 + \text{Na}_2\text{CO}_3 \rightarrow \text{Na}_2\text{SO}_4 + \text{H}_2\text{O} + \text{CO}_2 \).

Use stoichiometry to determine the moles of \( \text{Na}_2\text{CO}_3 \) required, then convert this to mass in kilograms using the molar mass of \( \text{Na}_2\text{CO}_3 \) (105.99 g/mol).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to form water and a salt. In this case, sulfuric acid (H2SO4) will react with sodium carbonate (Na2CO3) to produce sodium sulfate (Na2SO4), water (H2O), and carbon dioxide (CO2). Understanding this reaction is crucial for determining the stoichiometry involved in neutralizing the acid.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. For the neutralization of sulfuric acid with sodium carbonate, the balanced equation helps to determine the molar ratios needed to find out how much sodium carbonate is required to neutralize a given amount of sulfuric acid.

Concentration and Density

Concentration refers to the amount of solute in a given volume of solution, while density is the mass per unit volume of a substance. In this problem, the concentration of sulfuric acid is given in mass percent, and its density is provided, which allows for the conversion of mass to volume and vice versa, essential for calculating the amount of sodium carbonate needed for neutralization.

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Textbook Question

In qualitative analysis, Ca2+ and Ba2+ are seperated from Na+, K+, Mg2+ by adding aqueous (NH4)2CO3 to a solution that also contains aqueous NH3 (Figure 17.18). Assume that the concentrations after mixing are 0.080 M (NH4)2CO3 and 0.16 M NH3. (a) List all the Bronsted-Lowry acids and bases present initially, and identify the principal reaction.

Textbook Question

A railroad tank car derails and spills 36 tons of concentrated sulfuric acid. The acid is 98.0 mass% H₂SO₄ and has a density of 1.836 g/mL. (a) What is the molarity of the acid?

Textbook Question

Some progressive hair coloring products marketed to men, such as Grecian Formula 16, contain lead acetate Pb(CH3CO2)2. As the coloring solution is rubbed on the hhair, the Pb2+ ions react with the sulfur atoms in hair proteins to give lead(II) sulfide (PbS), which is black. A typical coloring solution contains 0.3 mass% Pb(CH3CO2)2, and about 2 mL of the solution is used per application. (b) Suppose the hair is washed with shampoo and water that has pH = 5.50. How many washings would be required to remove 50% of the black color? Assume that 3 gal of water is used per washing and that the water becomes saturated with PbS. (c) Does the calculated number of washings look reason-able, given that frequent application of the coloring solution is recommended? What process(es) in addition to dissolution might contribute to the loss of color?

Textbook Question

Some progressive hair coloring products marketed to men, such as Grecian Formula 16, contain lead acetate Pb(CH₃CO₂)₂. As the coloring solution is rubbed on the hair, the Pb²⁺ ions react with the sulfur atoms in hair proteins to give lead(II) sulfide (PbS), which is black. A typical coloring solution contains 0.3 mass% Pb(CH₃CO₂)₂, and about 2 mL of the solution is used per application. (a) Assuming that 30% of the Pb(CH₃CO₂)₂ is converted to PbS, how many milligrams of PbS are formed per application of the coloring solution?

Textbook Question

Neutralization reactions involving either a strong acid or a strong base go essentially to completion, and therefore we must take such neutralizations into account before calculating concentrations in mixtures of acids and bases. Consider a mixture of 3.28 g of Na3PO4 and 300.0 mL of 0.180 M HCl. Write balanced net ionic equations for the neutralization reactions and calculate the pH of the solution.

A railroad tank car derails and spills 36 tons of concentrated sulfuric acid. The acid is 98.0 mass% H2SO4 and has a density of 1.836 g/mL. (b) How many kilograms of sodium carbonate are needed to completely neutralize the acid?

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Key Concepts

Neutralization Reaction

Stoichiometry

Concentration and Density

A railroad tank car derails and spills 36 tons of concentrated sulfuric acid. The acid is 98.0 mass% H₂SO₄ and has a density of 1.836 g/mL. (b) How many kilograms of sodium carbonate are needed to completely neutralize the acid?