Textbook Question
(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?
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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 82a
(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?
Verified step by step guidance1
Step 1: Write down the balanced chemical equation for the reaction. In this case, the reaction is between hydrochloric acid (HCl) and barium hydroxide (Ba(OH)2). The balanced equation is: 2HCl + Ba(OH)2 -> BaCl2 + 2H2O
Step 2: Calculate the moles of Ba(OH)2 in the solution using the formula: moles = volume (in liters) x molarity. In this case, the volume of Ba(OH)2 solution is 50.0 mL or 0.050 L and the molarity is 0.101 M.
Step 3: From the balanced chemical equation, we can see that the stoichiometric ratio between HCl and Ba(OH)2 is 2:1. This means that for every mole of Ba(OH)2, we need 2 moles of HCl to neutralize it. So, multiply the moles of Ba(OH)2 by 2 to get the moles of HCl needed.
Step 4: Now, calculate the volume of HCl solution needed using the formula: volume (in liters) = moles / molarity. In this case, the molarity of HCl is 0.120 M. Convert the volume from liters to milliliters by multiplying by 1000.
Step 5: The result is the volume of 0.120 M HCl needed to completely neutralize the 50.0 mL of 0.101 M Ba(OH)2 solution.
Verified Solution
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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 produce water and a salt. In this case, hydrochloric acid (HCl) reacts with barium hydroxide (Ba(OH)2). The balanced chemical equation helps determine the stoichiometric relationships between the reactants, which is essential for calculating the volumes needed for complete neutralization.
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Molarity (M)
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L). In this question, the molarity of HCl and Ba(OH)2 solutions is crucial for determining how much of each solution is required for the reaction, as it allows for the conversion between volume and the amount of substance.
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Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the proportions of substances consumed and produced. In this scenario, stoichiometry is used to relate the moles of HCl needed to neutralize the moles of Ba(OH)2 present in the solution, facilitating the calculation of the required volume of HCl.
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Related Practice
Textbook Question
(b) What volume of HCl is needed to neutralize 2.87 g of Mg(OH)2?
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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
(b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH?
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Textbook Question
(c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sample of Na2SO4, what is the molarity of the BaCl2 solution?
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Open Question
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 resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: 2 NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g). Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?