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Common Dilutions
Hydrochloric Acid, HCl |
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(concentrated hydrochloric acid is 12 M) | |
CAUTION: Always add the acid to the water! |
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Quantity to add to make 1-L solution | |
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Sodium Hydroxide, NaOH |
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Molar mass of sodium hydroxide = 40.0 g·mol-1 | |
Quantity to add to make 1-L solution | |
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Sulfuric Acid, H2SO4 |
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CAUTION: Always add the acid to the water! | |
(concentrated sulfuric acid is 18 M) | |
Quantity to add to make 1-L solution | |
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Safety Precautions
Dilution of acids
- Always add acid to water (never add water to the acid)
Solution Preparation
Although there are several ways to measure solution concentration, molarity (M) is most commonly used. Molarity is measured as the number of moles of solute per liter of solution.
To prepare a 1M solution of a solute you would add 1 mole of the substance to a clean 1-L volumetric flask, partially filled with distilled or deionized water. Allow the solute to dissolve completely. Then add enough water to fill the flask to the mark on the flask.
To prepare a diluted solution, add the required volume of the concentrated solution to a volumetric flask (of the appropriate size), then fill to the mark on the flask
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Calculating Dilutions
To prepare a dilution, determine the volume and concentration (molarity) of solution that will be required. Use the following equation to determine how much of the concentrated solution will be required:
M1V1= M2V2
where
M1 and M2 are the concentrations of the original and diluted solutions and
V1 and V2 are the volumes of the original and diluted solutions
Example:
What volume of concentrated hydrochloric acid, 12.0 M, is required to prepare 500 mL of 0.150 M solution by dilution with water?
Solution:
In a dilution question there are 4 variables - M1, V1, M2 and V2. You will know three of these values and have to calculate the fourth.
M1 = 12.0 M M2= 0.150 M V1 = ? V2 = 500 mL Set up the formula, and rearrange to solve for the unknown, V1:
M1V1 =M2V2 12.0 × V1 =0.150 × 500 mL V1 = 0.150 × 500
12.0V1 =6.25 mL To make the required diluted solution, add 6.25 mL of concentrated hydrochloric acid to a 500 mL volumetric flask (or other volume measuring device). Fill to the mark on the flask with water.
Assorted Solution Recipes
Link to Lab Activity |
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Calcium hydroxide, Ca(OH)2 | ||||
saturated |
see Limewater | |||
Cobalt(II) chloride hexahydrate, CoCl2· 6H2O (acidified) |
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0.2 M |
2.6 g CoCl2· 6H2O to total solution volume of 100 mL. This produces the pink hydrated form of the equilibrium system. To form the blue chloro-complex side of this equilibrium, add concentrated 12M HCl (as much as 100 mL) until the solution turns blue. |
Equilibrium demonstrations | ||
Copper(II) nitrate, Cu(NO3)2 |
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0.5M |
93.8 g; add distilled water for a total volume of 1 L | Electrochemical Cells | ||
Copper(II) sulfate, CuSO4 |
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160 g; add distilled water for a total volume of 1 L | Electroplating | ||
Copper(II) sulfate, CuSO4 · 5H2O |
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0.1 M |
25.0 g ; add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
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250 g; add distilled water for a total volume of 1 L | Electroplating | ||
Iron(III) chloride, FeCl3 |
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0.1 M |
16 g FeCl3 in 50 mL 6M HCl. add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
Lead(II) nitrate, Pb(NO3)2 |
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0.5 M |
165.6 g; add distilled water for a total volume of 1 L | Electrochemical Cells | ||
Limewater, Ca(OH)2 |
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saturated |
1.5 g per liter of water. Stir or shake vigorously for a minute or two. Let stand overnight; filter off the clear solution and store. | |||
Limewater is often used to test for the presence of carbon dioxide. For example, have a student use a straw and blow into a solution of clear limewater. The solution will turn cloudy. The reactions:
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Potassium chloride, KCl |
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0.1 M |
7 g KCl; add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
Potassium chromate, K2CrO4 |
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0.1 M |
19 g K2CrO4, add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
Potassium dichromate, K2Cr2O7 |
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0.1 M |
29 g K2Cr2O7; add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
Potassium nitrate, KNO3 |
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0.5 M |
50.6 g; add distilled water for a total volume of 1 L | Electrochemical Cells | ||
Potassium thiocyanate, KSCN |
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0.1 M |
10 g KSCN; add distilled water for a total volume of 1 L | Le Châtelier's Principle | ||
Zinc nitrate, Zn(NO3)2 |
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0.5 M |
94.7 g; add distilled water for a total volume of 1 L | Electrochemical Cells | ||
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