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**Making Molar Solutions**

From Solids

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**What are molar solutions?**

A molar solution is one that expresses “concentration” in moles per volume Usually the units are in mol/L mol/L can be abbreviated as M or [ ] Molar solutions are prepared using: a balance to weigh moles (as grams) a volumetric flask to measure litres L refers to entire volume, not water! Because the units are mol/L, we can use the equation M = n/L Alternatively, we can use the factor label method

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**Calculations with molar solutions**

Q: How many moles of NaCl are required to make 7.5 L of a 0.10 M solution? M=n/L, n = 0.10 M x 7.5 L = 0.75 mol # mol NaCl = 7.5 L x 0.10 mol NaCl 1 L = 0.75 mol But in the lab we weigh grams not moles, so … Q: How many grams of NaCl are required to make 7.5 L of a 0.10 M solution? # g NaCl = 7.5 L x 0.10 mol NaCl 1 L x g NaCl 1 mol NaCl =43.83 g Read pages 288 – Do Q

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# g NaOH = 3.00 L x mol NaOH 1 L x g NaOH 1 mol NaOH =15.0 g # g NaCl = 5.0 L x 0.56 mol NaCl 1 L x g NaCl 1 mol NaCl = 164 g 355 ppm = 355 mg/L or g/L # g CO2 = 1.00 L x g CO2 1 L =.355 g 0.355 g CO2 x 1 mol CO2 44.0 g CO2 = 8.07 x 10–3 mol 1L = 8.07 x 10–3 mol/L a) 235 g 3000 mL x 100% =7.83 % W/V b) mol/L = 4.02 mol / 3.00 L = 1.34 mol/L

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**Practice making molar solutions**

Calculate # of grams required to make 100 mL of a 0.10 M solution of NaOH (see above). Get volumetric flask, plastic bottle, 100 mL beaker, eyedropper. Rinse all with tap water. Fill a beaker with distilled water. Pour mL of H2O from beaker into flask. Weigh NaOH. Add it to flask. Do step 5 quickly. Mix (by swirling) until the NaOH is dissolved. Add distilled H2O to just below the colored line. Add distilled H2O to the line using eyedropper. Place solution in a bottle. Place label (tape) on bottle (name, date, chemical, molarity). Place bottle at front. Rinse & return equipment.

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**More Practice Questions**

For more lessons, visit How many grams of nitric acid are present in 1.0 L of a 1.0 M HNO3 solution? 2. Calculate the number of grams needed to produce 1.00 L of these solutions: a) 1.00 M KNO3 b) 1.85 M H2SO c) 0.67 M KClO3 3. Calculate the # of grams needed to produce each: a) 0.20 L of 1.5 M KCl b) L of M HCl c) 0.20 L of 0.09 mol/L AgNO3 d) 250 mL of 3.1 mol/L BaCl2 4. Give the molarity of a solution containing 10 g of each solute in 2.5 L of solution: a)H2SO4 b)Ca(OH)2 63 g 101 g 181 g 82 g a) 22 g b) 1.75 g c) 3 g d) 0.16 kg 5. Describe how 100 mL of a 0.10 mol/L NaOH solution would be made. a) mol/L b) mol/L

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Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry Properties of Solutions.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry Properties of Solutions.

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