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Making Molar Solutions

Making Molar Solutions. From Solids. 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)

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Making Molar Solutions

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  1. Making Molar Solutions From Solids

  2. 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

  3. x 0.10 mol NaCl x 0.10 mol NaCl x 58.44 g NaCl 1 mol NaCl 1 L 1 L Calculations with molar solutions M=n/L, n = 0.10 M x 7.5 L = 0.75 mol Q: How many moles of NaCl are required to make 7.5 L of a 0.10 M solution? # mol NaCl = 7.5 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 =43.83 g Read pages 288 – 290. Do Q 19 - 22

  4. # g NaOH = x 0.125 mol NaOH x 40.00 g NaOH x 0.56 mol NaCl x 58.44 g NaCl x 0.355 g CO2 x 1 mol CO2 1 mol NaOH 44.0 g CO2 1 mol NaCl 1 L 1 L 1 L 3.00 L =15.0 g # g NaCl = 5.0 L = 164 g • 355 ppm = 355 mg/L or 0.355 g/L 1.00 L =.355 g # g CO2 = 0.355 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

  5. 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 20 - 30 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.

  6. For more lessons, visit www.chalkbored.com More Practice Questions 63 g 101 g • 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 H2SO4 c) 0.67 M KClO3 3. Calculate the # of grams needed to produce each: a) 0.20 L of 1.5 M KCl b) 0.160 L of 0.300 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)2 181 g 82 g a) 22 g b) 1.75 g c) 3 g d)0.16kg 5. Describe how 100 mL of a 0.10 mol/L NaOH solution would be made. a) 0.041 mol/L b) 0.054 mol/L

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