Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (b) 44.0 mL of 0.100 M Na2SO4 with 25.0 mL of 0.150 M KCl
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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 74a
(a) How many milliliters of a stock solution of 6.0 M HNO3 would you have to use to prepare 110 mL of 0.500 M HNO3?
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 (M). Understanding molarity is crucial for diluting solutions and performing calculations involving concentrations, as it allows chemists to relate the amount of solute to the volume of solution.
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Molarity Concept
Dilution Equation
The dilution equation, often expressed as M1V1 = M2V2, relates the molarity and volume of a concentrated solution (M1 and V1) to the molarity and volume of the diluted solution (M2 and V2). This equation is essential for calculating how to prepare a desired concentration from a stock solution, ensuring accurate and precise solution preparation.
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00:58Dilution Equation
Volume Conversion
Volume conversion is the process of changing units of volume, such as from liters to milliliters. In this context, understanding how to convert between these units is important for accurately measuring and mixing solutions, as the dilution equation requires consistent units to yield correct results.
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Related Practice
Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl2 solution. Assume that the volumes are additive.
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Textbook Question
(b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500 L, what will be the concentration of the final solution?
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Textbook Question
(b) If you dilute 10.0 mL of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?
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Textbook Question
medical lab is testing a new anticancer drug on cancer cells. The drug stock solution concentration is 1.5 * 10-9 M, and 1.00 mL of this solution will be delivered to a dish containing 2.0 * 105 cancer cells in 5.00 mL of aqueous fluid. What is the ratio of drug molecules to the number of cancer cells in the dish?
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Textbook Question
Calicheamicin gamma-1, C55H74IN3O21S4, is one of the most potent antibiotics known: one molecule kills one bacterial cell. Describe how you would (carefully!) prepare 25.00 mL of an aqueous calicheamicin gamma-1 solution that could kill 1.0 * 108 bacteria, starting from a 5.00 * 10-9M stock solution of the antibiotic.
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