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Questions and Answers
What is the first step in the preparation of solutions?
Which of the following is the correct definition of molarity?
When diluting a solution, what relationship is maintained?
In preparing a 0.9% w/v NaCl solution, how much NaCl is needed for 500 mL?
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Which equation represents the dilution relationship correctly?
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What is the correct mass of NaOH needed to prepare 2 liters of a 0.5 M solution?
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How much NaCl is needed to prepare 800 mL of a 2 M solution?
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Using the dilution formula, what is the necessary volume of a 12.1 M HCl solution needed to prepare 100 mL of a 1.0 M solution?
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How many grams of Na2CO3 are needed to prepare 500 mL of a 0.1 M solution?
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For a 3500 mL solution of potassium permanganate at a concentration of 0.08 M, what mass is needed?
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Study Notes
Preparing Solutions
- Preparing solutions is a fundamental skill in chemistry involving the accurate measurement and mixing of solutes and solvents.
- A solution is a homogenous mixture of solute and solvent.
- The concentration of a solution is determined by the specific amount of solute in a specific amount of solution.
Steps for Preparing Solutions
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Calculations:
- Determine the desired concentration and volume of the solution.
- Calculate the amount of solute needed.
- Calculate the volume of solvent needed.
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Preparation:
- Weigh the solid or measure the liquid solute.
- Dissolve or mix the solute with the solvent.
Basic Concepts
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Molarity (M): Molarity is defined as the number of moles of solute per liter of solution.
- Formula: M = n ÷ V
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Percent Solutions:
- Mass percent: grams of solute per 100 grams of solution.
- Volume percent: milliliters of solute per 100 mL of solution.
- Mass/Volume percent (w/v%): grams of solute per 100 mL of solution.
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Dilution:
- The process of adding more solvent to a solution, increasing volume while keeping the number of moles of solute constant.
- Formula: M1V1 = M2V2
- M1, V1: Molarity and volume of the concentrated solution.
- M2, V2: Molarity and volume of the diluted solution.
Examples
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Preparing a 500 mL solution of NaCl 0.9% w/v:
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Calculation:
- Mass of solute = percent x volume of solution ÷ 100
- Mass of solute = 0.9 x 500 ÷ 100 = 4.5 grams
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Preparation:
- Weigh 4.5 grams of NaCl.
- Transfer to a 500 mL volumetric flask.
- Add water to dissolve and shake to promote dissolution.
- Add water until the volume reaches the mark on the flask.
- Close the flask and mix thoroughly.
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Calculation:
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Preparing 2 Liters of a solution of NaOH (0.5 M):
-
Calculation:
- Mass of NaOH = M x Mwt x Volume (L)
- Mass of NaOH = 0.5 x 40 x 2 = 40 grams
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Preparation:
- Weigh 40 g of NaOH.
- Transfer to a 2 L volumetric flask.
- Add water until the volume reaches 2 L.
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Calculation:
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Preparing 800 mL (0.8 L) of a 2 M sodium chloride (NaCl) solution:
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Calculation:
- Mass = M x Mwt x Volume (L) = 2 x 58.45 x 0.8 = 93.52 grams
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Preparation:
- Dissolve 93.52 g of NaCl in approximately 400 mL of water.
- Add more water until the final volume reaches 800 mL.
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Calculation:
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Preparing 100 mL (0.1 L) of a 1.0 M hydrochloric acid (HCl) from a concentrated solution (12.1 M):
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Calculation:
- V1 = M2V2/M1 = 1 x 0.1 / 12.1 = 0.00826 L = 8.26 mL
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Preparation:
- Add 8.26 mL of concentrated HCl to approximately 50 mL of water.
- Dilute to a final volume of 100 mL.
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Calculation:
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Preparing a standard solution of 500 mL of Na2CO3 (0.1 M):
- Calculation: Requires 5.3 grams in 500 mL solution.
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Preparing a 3500 mL solution of potassium permanganate (0.08 M):
- Calculation: Requires 44.24 grams in 3500 mL solution.
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Description
This quiz tests your understanding of preparing solutions in chemistry. It covers key concepts such as molarity, concentration calculations, and the steps involved in preparing both liquid and solid solutions. Enhance your skills in accurately mixing solutes and solvents.