Chapter 7 Solutions in addition to Colloids 7.5 Solution Preparation Molarity (M) Molarity

Chapter 7 Solutions in addition to Colloids 7.5 Solution Preparation Molarity (M) Molarity www.phwiki.com

Chapter 7 Solutions in addition to Colloids 7.5 Solution Preparation Molarity (M) Molarity

Duff, David, Music Director has reference to this Academic Journal, PHwiki organized this Journal Chapter 7 Solutions in addition to Colloids 7.5 Solution Preparation Molarity (M) Molarity (M) is a concentration term as long as solutions. gives the moles of solute in 1 L solution. moles of solute liter of solution Preparing a 1.0 Molar Solution A 1.00 M NaCl solution is prepared by weighing out 58.5 g NaCl (1.00 mole) in addition to adding water to make 1.00 liter of solution. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

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Calculation of Molarity What is the molarity of 0.500 L NaOH solution if it contains 6.00 g NaOH STEP 1 Given 6.00 g NaOH in 0.500 L solution Need molarity (mole/L) STEP 2 Plan g NaOH mole NaOH molarity Calculation of Molarity (cont.) STEP 3 Conversion factors 1 mole NaOH = 40.0 g 1 mole NaOH in addition to 40.0 g NaOH 40.0 g NaOH 1 mole NaOH STEP 4 Calculate molarity. 6.00 g NaOH x 1 mole NaOH = 0.150 mole 40.0 g NaOH 0.150 mole = 0.300 mole = 0.300 M NaOH 0.500 L 1 L Learning Check What is the molarity of 325 mL of a solution containing 46.8 g of NaHCO3 1) 0.557 M 2) 1.44 M 3) 1.71 M

Solution 3) 1.71 M 46.8 g NaHCO3 x 1 mole NaHCO3 = 0.557 mole NaHCO3 84.0 g NaHCO3 0.557 mole NaHCO3 = 1.71 M NaHCO3 0.325 L Learning Check What is the molarity of 225 mL of a KNO3 solution containing 34.8 g KNO3 1) 0.344 M 2) 1.53 M 3) 15.5 M Solution 2) 1.53 M 34.8 g KNO3 x 1 mole KNO3 = 0.344 mole KNO3 101.1 g KNO3 M = mole = 0.344 mole KNO3 = 1.53 M L 0.225 L In one setup: 34.8 g KNO3 x 1 mole KNO3 x 1 = 1.53 M 101.1 g KNO3 0.225 L

Molarity Conversion Factors The units of molarity are used as conversion factors in calculations with solutions. TABLE 7.8 Calculations Using Molarity How many grams of KCl are needed to prepare 125 mL of a 0.720 M KCl solution STEP 1 Given 125 mL (0.125 L) of 0.720 M KCl Need Grams of KCl STEP 2 Plan L KCl moles KCl g KCl Calculations Using Molarity STEP 3 Conversion factors 1 mole KCl = 74.6 g 1 mole KCl in addition to 74.6 g KCl 74.6 g KCl 1 mole KCl 1 L KCl = 0.720 mole KCl 1 L in addition to 0.720 mole KCl 0.720 mole KCl 1 L STEP 4 Calculate grams. 0.125 L x 0.720 mole KCl x 74.6 g KCl = 6.71 g KCl 1 L 1 mole KCl

Learning Check How many grams of AlCl3 are needed to prepare 125 mL of a 0.150 M solution 1) 20.0 g AlCl3 2) 16.7g AlCl3 3) 2.50 g AlCl3 Solution 3) 2.50 g AlCl3 0.125 L x 0.150 mole x 133.5 g = 2.50 g AlCl3 1 L 1 mole Learning Check How many milliliters of 2.00 M HNO3 contain 24.0 g HNO3 1) 12.0 mL 2) 83.3 mL 3) 190. mL

Solution 24.0 g HNO3 x 1 mole HNO3 x 1000 mL = 63.0 g HNO3 2.00 mole HNO3 Molarity factor inverted = 190. mL HNO3 Dilution In a dilution water is added. volume increases. concentration decreases. Mix The amount of solute in the concentrated solution = amount of solute in the diluted solution 3 containers of H2O 1 container orange juice concentrate +

Comparing Initial in addition to Diluted Solutions In the initial in addition to diluted solution, the moles of solute are the same. the concentrations in addition to volumes are related by the following equations: For percent concentration: C1V1 = C2V2 initial diluted For molarity: M1V1 = M2V2 initial diluted Dilution Calculations with Percent What volume of a 2.00% (m/v) HCl solution can be prepared by diluting 25.0 mL of 14.0% (m/v) HCl solution Prepare a table: C1= 14.0% (m/v) V1 = 25.0 mL C2= 2.00% (m/v) V2 = Solve dilution equation as long as unknown in addition to enter values: C1V1 = C2V2 V2 = V1C1 = (25.0 mL)(14.0%) = 175 mL C2 2.00% Learning Check What is the percent (% m/v) of a solution prepared by diluting 10.0 mL of 9.00% NaOH to 60.0 mL

Solution What is the percent (%m/v) of a solution prepared by diluting 10.0 mL of 9.00% NaOH to 60.0 mL Prepare a table: C1= 9.00 %(m/v) V1 = 10.0 mL C2= V2 = 60.0 mL Solve dilution equation as long as unknown in addition to enter values: C1V1 = C2V2 C2 = C1 V1 = (10.0 mL)(9.00%) = 1.50% (m/v) V2 60.0 mL Dilution Calculations with Molarity What is the molarity (M) of a solution prepared by diluting 0.180L of 0.600 M HNO3 to 0.540 L Prepare a table: M1= 0.600 M V1 = 0.180 L M2= V2 = 0.540 L Solve dilution equation as long as unknown in addition to enter values: M1V1 = M2V2 M2 = M1V1 = (0.600 M)(0.180 L) = 0.200 M V2 0.540 L Learning Check What is the final volume (mL) of 15.0 mL of a 1.80 M KOH diluted to give a 0.300 M solution 1) 27.0 mL 2) 60.0 mL 3) 90.0 mL

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Solution What is the final volume (mL) of 15.0 mL of a 1.80 M KOH diluted to give a 0.300 M solution Prepare a table: M1= 1.80 M V1 = 15.0 mL M2= 0.300 M V2 = Solve dilution equation as long as V2 in addition to enter values: M1V1 = M2V2 V2 = M1V1 = (1.80 M)(15.0 mL) = 90.0 mL M2 0.300 M

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