8.7 Making Molar Solutions

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Making Molar Solutions

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Presentation transcript:

8.7 Making Molar Solutions From Liquids(More accurately, from stock solutions)

Making molar solutions from liquids Not all compounds are in a solid form Acids are purchased as liquids (“stock solutions”). Yet, we still need a way to make molar solutions of these compounds. The Procedure is similar: Use pipette to measure moles (via volume) Use volumetric flask to measure volume

C1V1 = C2V2 Now we use the equation C1V1 = C2V2 1 is starting (concentrated conditions) 2 is ending (dilute conditions) C1 = concentration of starting “stock” solution V1 = initial volume taken C2 = concentration of final “dilute” solution V2 = final volume

Reading a pipette Identify each volume to two decimal places (values tell you how much you have expelled) 4.48 - 4.50 4.86 - 4.87 5.00

Practice using a pipette Always keep pipette vertical To rinse: take up water, remove green filler, rotate pipette, replace filler, expel water If filler can not take up or expel enough liquid, remove, place finger over pipette, turn knob, replace filler. Take up water to 0 mark. Measure 3.2 mL into 10 mL cylinder. (one per person) If drop is hanging off, touch to cylinder Repeat with 1.7 mL and 5.1 mL __________________________________ If done correctly you should get 10 mL in graduated cylinder

The Dilution Formula C1V1 = C2V2 E.g. if we have 1.0 L of 3.0 M HCl, what is M if we dilute acid to 6.0 L?

Why does the formula work? Because we are equating mol to mol: V1 = 1 L C1 = 3 M V2 = 6 L C2 = 0.5 M C1V1 = 3 mol C2V2 = 3 mol

Practice problems Example 1: –What volume of 0.50 M HCl can be prepared from 1.0 L of 12.0 M HCl?

Example 2: Combining molar solutions 1.0 L of a 3.0 M HCl solution is added to 0.50 L of a 2.0 M HCl solution. What is the final concentration of HCl? (hint: first calculate total number of moles and total number of L)

Practice making molar solutions Calculate # of mL of 1.0 M HCl required to make 100. mL of a 0.1 M solution of HCl Get volumetric flask, pipette, plastic bottle, 100 mL beaker, 50 mL beaker, eyedropper. Rinse all with tap water. Dry 50 mL beaker Place about 20 mL of 1 M HCl in 50 mL beaker Rinse pipette, with small amount of acid Fill flask about 1/4 full with distilled water Add correct amount of acid with pipette. Mix. Add water to line (use eyedropper at the end).

Practice Questions 1. How many mL of a 14 M stock solution must be used to make 250 mL of a 1.75 M solution? 2. You have 200 mL of 6.0 M HF. What concentration results if this is diluted to a total volume of 1 L? 3. 100 mL of 6.0 M CuSO4 must be diluted to what final volume so that the resulting solution is 1.5 M? 4. What concentration results from mixing 400 mL of 2.0 M HCl with 600 mL of 3.0 M HCl?

5. What is the concentration of NaCl when 3 L of 0 5. What is the concentration of NaCl when 3 L of 0.5 M NaCl are mixed with 2 L of 0.2 M NaCl? 6. What is the concentration of NaCl when 3 L of 0.5 M NaCl are mixed with 2 L of water? 7. Water is added to 4 L of 6 M antifreeze until it is 1.5 M. What is the total volume of the new solution? 8. There are 3 L of 0.2 M HF. 1.7 L of this is poured out, what is the concentration of the remaining HF?