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Chapter 2: Problem 24

A stock solution of 12.0 M sulfuric acid is made available. What is the best procedure to make up 100.0 mL of 4.0 M sulfuric acid using the stock solution and water prior to mixing? (A) Add 33.3 mL of water to the flask, and then add 66.7 mL of 12.0 M acid. (B) Add 33.3 mL of 12.0 M acid to the flask, and then dilute it with 66.7 mL of water. (C) Add 67.7 mL of 12.0 M acid to the flask, and then dilute it with 33.3 mL of water. (D) Add 67.7 mL of water to the flask, and then add 33.3 mL of 12.0 M acid.

Short Answer

Expert verified
The best procedure to make up 100.0 mL of 4.0 M sulfuric acid using the stock solution and water is in fact (B) Add 33.3 mL of 12.0 M acid to the flask, and then dilute it with 66.7 mL of water.

Step by step solution

01

Identify the initial conditions

The starting molarity (\(M1\)) of the sulfuric acid is 12.0 M, and the final desired molarity (\(M2\)) is 4.0 M. We need to find the required volume of the 12.0 M solution to achieve 100.0 ml of 4.0 M solution.
02

Use the dilution formula

Using the dilution formula \(M1V1 = M2V2\), we substitute the known values to calculate the needed volume of the 12.0 M solution (\(V1\)). Therefore, \(V1 = M2V2 / M1 = 4.0 M * 100.0 mL / 12.0 M = 33.3 mL\).
03

Determine the volume of water

To achieve a final volume of 100 mL, the volume of water to be added should be the final volume (\(V2\)) minus the volume of the acid used (\(V1\)). Thus, volume of water = \(100.0 mL - 33.3 mL = 66.7 mL\).
04

Match to options

The results correspond to option (B): 'Add 33.3 mL of 12.0 M acid to the flask, and then dilute it with 66.7 mL of water'. This is therefore the best procedure to achieve the desired concentration.

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Most popular questions from this chapter

\(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\) 2.0 mol of \(\mathrm{CO}(g)\) and 2.0 mol of \(\mathrm{O}_{2}(g)\) are pumped into a rigid, evacuated \(4.0-\mathrm{L}\) container, where they react to form \(\mathrm{CO}_{2}(g) .\) Which of the following values does NOT represent a potential set of concentrations for each gas at a given point during the reaction? (A) 0.5 0.5 0 (B) 0 0.25 0.5 (C) 0.25 0.25 0.5 (D) 0.25 0.38 0.25

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The enthalpy values for several reactions are as follows: (I) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) \(\quad \Delta H=-131 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (II) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 3 \mathrm{H}_{2}(g)+\mathrm{CO}(g)\) \(\quad \Delta H=206 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (III) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) \(\quad \Delta H=-41 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (IV) \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) \(\quad \Delta H=-890 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) In which of the reactions does the amount of energy released by the formation of bonds in the products exceed the amount of energy necessary to break the bonds of the reactants by the greatest amount? (A) Reaction I (B) Reaction II (C) Reaction III (D) Reaction IV
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