(b) How many milliliters of 0.125 M H 2 SO 4 are needed to neutralize 0.200 g of NaOH?

Hey everyone. Our question here wants us to determine the volume of chronic acid used in this solution 1st. Let's go ahead and write out our reaction. So we have rubidium hydroxide and it reacts with chronic acid. Since we have an acid-based reaction, we end up with water plus rubidium chrome eight. Now, before we move on with our question, let's first balance out our reaction. As we can see in our product side, we have two of rubidium so we'll need to add a coefficient of two prior to rubidium hydroxide And since we adjusted our oxygen and hydrogen, we need to add a coefficient of two as well prior to our water. And now our reaction is completely balanced. Now starting off with our 0.424g of rubidium hydroxide, We're going to take the molar mass of rubidium hydroxide which is 102.475 g of rubidium hydroxide per one mole. And we'll go ahead and take our multiple ratios. And as we can see we have two moles of rubidium hydroxide per one mole of chronic acid. And since we want to end up in mill leaders of our chronic acid Will take the polarity of chronic acid which is 0.310 moles of chronic acid per one leader. And to convert this into middle leaders we know that one leader contains 10 to the 3rd mill leaders. And when we calculate this out and cancel out all our units, we end up with a value of 6.67 mill leaders of chronic acid and this is going to be our final answer. So I hope this made sense and let us know if you have any questions.

Ch.4 - Reactions in Aqueous Solution

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 82b

Chapter 4, Problem 82b

(b) How many milliliters of 0.125 M H₂SO₄ are needed to neutralize 0.200 g of NaOH?

Verified step by step guidance

Step 1: Write the balanced chemical equation for the neutralization reaction between sulfuric acid (H₂SO₄) and sodium hydroxide (NaOH). The balanced equation is: \[ \text{H}_2\text{SO}_4 + 2\text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O} \]

Step 2: Calculate the number of moles of NaOH. Use the formula: \[ \text{moles of NaOH} = \frac{\text{mass of NaOH (g)}}{\text{molar mass of NaOH (g/mol)}} \] The molar mass of NaOH is approximately 40.00 g/mol.

Step 3: Use the stoichiometry of the balanced equation to find the moles of H₂SO₄ needed. According to the equation, 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Therefore, \[ \text{moles of H}_2\text{SO}_4 = \frac{\text{moles of NaOH}}{2} \]

Step 4: Calculate the volume of 0.125 M H₂SO₄ solution required to provide the moles of H₂SO₄ calculated in Step 3. Use the formula: \[ \text{Volume (L)} = \frac{\text{moles of H}_2\text{SO}_4}{\text{Molarity of H}_2\text{SO}_4} \]

Step 5: Convert the volume from liters to milliliters by multiplying by 1000, since 1 L = 1000 mL.

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Key Concepts

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

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for stoichiometric calculations in chemistry, allowing us to relate the volume of a solution to the amount of substance it contains. In this question, the molarity of sulfuric acid (H2SO4) is given, which will be used to determine how much volume is needed to neutralize a specific mass of sodium hydroxide (NaOH).

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, sulfuric acid (H2SO4) will react with sodium hydroxide (NaOH) to form sodium sulfate (Na2SO4) and water. Understanding the stoichiometry of this reaction is essential to determine the exact amounts of reactants needed for complete neutralization.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to convert between grams, moles, and volumes of substances involved in a reaction. In this problem, stoichiometry will be used to relate the mass of NaOH to the moles of H2SO4 required for neutralization, ultimately leading to the calculation of the volume of the acid solution needed.