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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 82b
Chapter 4, Problem 82b

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

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1
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).
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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.
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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.
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Related Practice
Textbook Question

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

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Textbook Question

(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution?

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Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+?

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Textbook Question

(d) If 45.3 mL of a 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?

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Textbook Question

(c) If 25.8 mL of an AgNO3 solution is needed to precipitate all the Cl- ions in a 785-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?