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Solution Manual For Laboratory Manual for General, Organic, and Biological Chemistry, 3rd Edition

Solution Manual For Laboratory Manual for General, Organic, and Biological Chemistry, 3rd Edition bridges the gap between textbook theory and practical application.

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    Pre - Lab Study Questions 1 1 . What are the standard units of length, mass, volume, and temperature in the metric system? Length – meter M ass – gram V olume – liter T emperature – degrees Celsius (Kelvin) 2 . Why is the metric (SI) system called a decimal system of measurement? The ‘deci’ prefix means 10 . M easurements in the metric system are based on factors of 10. 3 . What is the purpose of using prefixes in the metric system? Prefixes are attached to the standard unit to provide larger and smaller measurements 4 . Fill in the blank lines below with the unit name, abbreviation, and property measured. Unit Name Abbreviation Property Measured liter L volume centimeter cm length kilometer km length milligram mg mass 5 . Identify each of the following as a measured number or an exact number: 5 books Exact (counted) 9.25 L Measured 0.035 kg Measured 100 cm in 1 m Exact (definition) 12 beakers Exact (counted) 59.067 g Measured 1000 mL  1 L Exact (definition) 8.03 mL Measured Date Name Section Team Instructor

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    A. Measuring Length 1. What units are represented by the numbers marked on the meterstick? centimeters What do the small lines marked on the meterstick represent ? millimeters Complete the following statements: There are 100 centimeters (cm) in 1 meter (m). There are 1,000 millimeters (mm) in 1 meter (m). There are 10 millimeters (mm) in 1 centimeter (cm). Item 2. Length 3. Estimated Digit 4. Number of Significant Figures Width of little fingernail 0.82 cm 0.02 2 Distance around wrist 21.45 cm 0.05 4 Length of your shoe 26.34 cm 0.04 4 5. Length of line Your measurement 13.74 cm Other students’ values 13.72 cm 13.77 cm How does your value of the line length compare to those of other students? My line is 0.02 cm longer than one, yet 0.03 cm shorter than the other . Questions and Problems Q1 What digits in the measurements for the line by other students are the same as yours and which are different? Their tens, units , and tenths are the same while their hundredths differ. Date Name Section Team Instructor REPORT SHEET Chemistry and Measurement LAB 1

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    B. Measuring Volume Volume of a liquid ( include units for every measurement ) Cylinder 1 Cylinder 2 Cylinder 3 1. Volume (mL) 25.6 mL 482 mL 780. mL Volume of a solid by displacement 2. Initial volume of water 20.0 mL 3. Volume of water and submerged solid 24.5 mL 4. Volume of solid ( 3  2 ) 4.5 mL C. Measuring Mass Item 1. Mass 4. Number of Significant Figures 1. Beaker 145.651 g 6 Stopper 6.534 g 4 Evaporating dish 52.168 g 5 2. Unknown # 0.567 g 3 3. Actual mass of unknown 0.565 g 3 Questions and Problems Q 2 State the number of significant figures in each of the following measurements: 4.5 m 2 204.52 g 5 0.0004 L 1 625.000 mm 6 805 lb 3 34.80 km 4 Q 3 Indicate the estimated digit in each of the following measurements: 1.5 cm 0.5 4500 mi 500 0.0782 in. 0.0002 42.50 g 0.00 48.231 g 0.001 8.07 lb 0.07

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    Pre - Lab Study Questions 2 1 . What are the rules for rounding off numbers? Look at the number immediately following the digit to be rounded. If the number is five or greater, round the digit up; if the number is less than five, leave the digit as is. 2 . How do you determine the number of significant figures for an answer obtained by multiplication or division? The final answer has the same number of significant figures as the measured number with the fewest significant figures. 3 . How do you determine the number of decimal places for an answer obtained by addition or subtraction? The final answer has the same decimal place as the measured number with the fewest decimal places. 4 . What is an equality and how is it used to write a conversion factor? An equality is the same measurement expressed in two different units; they are equal to each other. A conversion factor is written by placing one of the units in the numerator and the other in the denominator. 5. Write the equality and conversions factors for the relationship between miles and hours for a car traveling at 55 mi/h. Equality: Date Name Section Team Instructor

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    REPORT SHEET Conversion Factors and Problem Solving LAB 2 A. Rounding Off Initial Number Student’s Rounded Value 1. Correct? (yes/no) 2. Corrected (if needed) 143.63212 144 Yes 532 800 533 Yes 0.008 583 45 0.009 No 0.00858 8 8.00 Yes B. Significant Figures in Calculations B.1 Multiplication and Division Perform the following multiplication and division calculations. Give a final answer with the correct number of significant figures: 0.1184 8.00 0.0345   0.0327 (42.4)(15.6) 1.265 523 (35.56)(1.45) (4.8)(0.56) 19 B.2 Addition and Subtraction Perform the following addition and subtraction calculations. Give a final answer with the correct number of decimal places. 13.45 mL 0.4552 mL  13.91 mL 145.5 m 86.58 m 1045 m   1277 m 245.625 g – 80.2 g 165.4 g 4.62 cm – 0.885 cm 3.74 cm Date Name Section Team Instructor

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    B. 3 A rea 1. Your measurements 3. Another student’s measurements Length 13.29 cm 13.27 cm Width 4.32 cm 4.33 cm Area ( 2. , 4. ) 57.4 cm 2 57.5 cm 2 Why could two students obtain different values for the calculated area of the same rectangle? Because each student will estimate the last digit of the measured numbers differently B.4 Volume of a Solid 1. Shape of the solid Rectangular solid (cuboid) Dimensions to measure Height, length , & width 2. Height 3.86 cm Length 1.41 cm Width 2.33 cm Diameter (if cylinder) n/a 3. Formula for volume of solid Volume of the solid 12.7 cm 3 ( Show calculations of volume, including the units. )

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    C. Equalities and Conversion Factors C.1 Metric — Metric Conversion Factors for Volume 1. Equality 1 L  1000 mL 2. Conversion factors C.2 Metric — U.S. System Conversion Factors for Volume 1. Number of milliliters in 1 qt 1 qt = 960 mL ( Experimental factor ) 2. True equality 1 qt = 946 mL 3. Conversion factors How does your experimental fac tor compare to the conversion factor 946 mL/1 qt.? My volume is 14 mL greater than the standard value. C.3 Metric — U.S. System Conversion Factors for Length 1. Vertical page length ( measured ) 11.00 in. Vertical page length ( measured ) 27.88 cm 2.  2.53 cm/1 in . ( Experimental factor ) 3. True equality 2.54 cm = 1 in 4. Conversion factors How does your experimental factor compare to the conversion factor 2.54 cm/1 in.? My length is 0.01 cm lower than the standard value. C.4 Metric — U.S. Syst em Conversion Factors for Mass 1. Name of commercial product Wheat Thins 2. Mass, in grams, stated on label 340 g Weight, in pounds or ounces, stated on label 12 oz 3. Weight in lb ( Convert oz to lb if needed. ) 4. = 453 g/1 lb ( Experimental factor ) 5. True equality 454 g  1 lb 6. Conversion factors

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    How does your experimental factor compare to the standard conversion factor of 454 g/lb? My mass is 1 g lower than the standard value. D. Problem Solving Using Conversion Factors Your metric height 1. Height (inches) 68.0 in. 2. Height in centimeters 173 cm ( Show your calculations ) 3. Height in meters 1.73 m ( Show your calculations ) Questions and Problems Q1 A pencil is 16.2 cm long. What is its length in inches? Q2 A person has a mass of 63.4 kg. What is that weight in pounds? Q3 A bottle of olive oil contains 1.4 qt of olive oil. What is that volume in milliliters? Q4 How many liters of plasma are present in 8.5 pt?

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    Pre - Lab Study Questions 3 1 . What property of oil makes it float on water? The oil’s lower density makes it float . 2 . Why would heating the gas in a hot air balloon make the balloon rise? Heat expands the gas volume causing h ot air to have a lower density than cold air . The balloon rises because of the low density hot air . 3 . What is the difference between density and specific gravity? Density has units of g/mL . S pecific gravity has no unit s because it is a ratio of a substance’s density to that of water and those units cancel out . 4. An object has a mass of 18.4 g and a volume of 11.2 mL. a. What is the density of the object? b. What is the specific gravity of the object? 1.64 c. Will the object sink or float in water? Sink 5. A 15.0 g - sample of a liquid has a density of 0.875 g/mL. a. What is the volume, in milliliters, of the liquid? Use conversion factors to calculate answer. b. What mass, in grams, of the liquid is in 34.6 mL of the liquid? Date Name Section Team Instructor

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    REPORT SHEET Density and Specific Gravity LAB 3 A. Density of Liquids A.1 Density of Water 1. Volume (mL) 20.2 mL 2. Mass of beaker 150.802 g 3. Mass of beaker + liquid 171.223 g 4. Mass of liquid 20.431 g 5. Density 1.01 g/mL ( Show calculations ) A.2 Density of an Unknown Liquid 1. Type of liquid sample Salt water Volume of liquid 20.3 mL 2. Mass of beaker 150.802 g 3. Mass of beaker + liquid 172.047 g 4. Mass of liquid 21.245 g 5. Density 1.05 g/mL ( Show calculations ) B. Specific Gravity 1. Specific gravity of water 1.01 2. Specific gravity of liquid sample 1.05 3. Specific gravity of water using a hydrometer 1.00 4. Specific gravity of liquid using a hydrometer 1.04 How do the calculated specific gravity of water and the liquid sample ( 1, 2 ) co m pare to the hydrometer readings ( 3, 4 ) for water and the liquid sample? The calculated values were both 0.01 units higher than the hydrometer rea d ings. Date Name Section Team Instructor

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    C. Density of Solids 1. Mass of the solid 24.641 g 2. Initial water level 19.9 mL 3. Final water level with solid 23.1 mL 4. Volume of solid ( 3  2 ) 3.2 mL 5. Density of the solid 7.7 g/mL ( Show calculations ) 6. Type of metal Iron D. Graphing Mass and Volume 1. Initial volume of water 22.7 mL 2. Initial mass of cylinder + water 43.850 g 3. Type of metal Brass Total Mass of Cylinder, Water, and Metal Pieces Total Volume of Water and Metal Pieces 4. 52.271 g 4. 23.7 mL 5. 63.363 g 5. 25.0 mL 6. 72.999 g 6. 2 5.9 mL 7. 89.951 g 7. 28.2 mL Calculations 8. Mass of Metal Pieces 9. Volume of Metal Pieces 10. Density (8/9) (4 – 2) 8.421 g (4 – 1) 1.0 mL 8.4 g/mL (5 – 2) 19.513 g (5 – 1) 2.3 mL 8.5 g/mL (6 – 2) 29.149 g (6 – 1) 3. 2 mL 8.3 g/mL (7 – 2) 46.101 g (7 – 1) 5.5 mL 8.4 g/mL

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    11. Drawing the Graph 1 2. Questions and Problems Q1 A metal object has a mass of 8.37 g. When it was placed in a graduated cy l inder containing 20.0 mL of water, the water level rose to 23.1 mL. What is the density and identity of the metal? (see Table 3.1) The metals is Al Q2 What is the mass of a solution that has a density of 0.775 g/mL and a volume of 50.0 mL? Q3 What is the volume of a solution that has a specific gravity of 1.2 and a mass of 185 g?

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    Q4 A pump delivers the following volume of a solution over 4 h. Volume (mL) Time (h) 0 0 50 1.0 100 2.0 125 2.5 150 3.0 200 4.0 Prepare a graph to represent the data.

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    Pre - Lab Study Questions 4 1 . What is the equation for converting a Fahrenheit temperature to a Celsius temperature? 2. What is meant by the term specific heat ? Specific heat is the amount of heat (cal or Joules) needed to raise the temperature of 1 .00 g of substance by 1 .00 ˚ C. 3. Why is a measured amount of water needed to determine the specific heat of a metal object? Since we use the cal gained by the water to find the cal lost by the metal, we need to know the mass of the water. 4. What are the units of specific heat? 5. How is the caloric value of a food sample determined? The food is put into a calorimeter sample chamber for a combustion reaction. The change in temperature is measured for a given mass of water in the calorimeter. Date Name Section Team Instructor

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