Lab 5_Density_ A characteristic Property (1)

4. Your lab instructor directs you to use 12.5 grams of the cyclohexanol to start the synthesis. If the density of cyclohexanol is 0.9624 grams/cm³, what volume of cyclohexanol should you measure out in your 25-mL graduated cylinder? Show the calculation completely, giving close attention to the use of units and significant figures.

In a similar experiment, a pair of students was asked to measure out 10.00 mL of water using a 25-mL buret. The data they collected is shown in the table below: Trial Student 1 Student 2 1 9.98 mL 9.97 mL 2 10.00 mL 9.99 mL 3 9.99 mL 10.01 mL Which of the following statements best describes the set of data collected by each student? Student 1 both accurate and precise Student 2 only accurate [ Choose] only accurate both accurate and precise only precise

Measurement and Matter Adding or subtracting and multiplying or dividing measurements 1/3 B A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: The label on the graduated cylinder says: empty weight: 7.2 g . She put some solid sodium hydroxide into the graduated cylinder and weighed it. With the sodium hydroxide added, the cylinder weighed 63.517 g. . She added water to the graduated cylinder and dissolved the sodium hydroxide completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 91.0 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. g-mL G

Solution 1 is diluted by combining 6 mL of Solution 1 with 64 mL of Solution 2. What is the dilution of solution 1?   Report your answer in standard decimal notation rounded to two decimal places. For example, 4 mL added to 16 mL would be a 0.20 dilution. Include trailing zeros if necessary so your answer has two decimal places.

Measurement and Matter Adding or subtracting and multiplying or dividing measurements 0/3 B A chemistry student must write down in her lab notebook the concentration of a solution of potassium chloride. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: The label on the graduated cylinder says: empty weight: 1.500 g She put some solid potassium chloride into the graduated cylinder and weighed it. With the potassium chloride added, the cylinder weighed 40.22 g. She added water to the graduated cylinder and dissolved the potassium chloride completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 172.08 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. A Om g·mL -1 □×1 x10 x 5

Imagine you collected a master batch (undiluted) wastewater sample as shown in the illustration below. The total mass of lead (Pb) found in 300 mL of a two-fold diluted master sample was 1.65 µg Calculate the amount of Pb in the master batch sample of the wastewater in ppb. Enter numerical values rounded to one significant figure without units. O Volume of solution: 1 L Mass of solution: 1.1 kg

In the lab you weigh 12.54 g of NaCl to make a stock solution of 5.12 M. To further dilute the solution to 100.0 mL of 0.125 M, how much of the stock solution do you need? Give your answer in mL. Use correct number of significant figures.

A given analytical test was performed five times. The results of the analysis are represented by the following values: 6.738, 6.738, 6.737, 6.739, and 6.738%. Would you say that these results are precise? Can you say that they are accurate? Explain both answers.

Part B Gather all of your pennies dated before 1982. Then follow the steps to complete the table. Include units as necessary. Record the number of pennies dated before 1982. Weigh (as a group) the pennies dated before 1982. Record the total mass. If you’re unfamiliar with using an electronic balance, watch this video before continuing. Calculate and record the average mass of a single penny. If you need help with the calculation, visit the averaging data section of the math review. number of pennies: 8 combined mass of the pennies (g): 49.2 average mass of a penny (g): 5.525 Part C Now gather all of your pennies dated after 1982. Complete the table for the post-1982 pennies using the same steps from part B. number of pennies: 9 combined mass of the pennies (g): 51.7 average mass of a penny (g): 5.744 Part D In parts B and C, you measured the average mass of each group of pennies. Now you’ll measure their volume. (For this part, assume that the pennies dated before and after…

Part B Gather all of your pennies dated before 1982. Then follow the steps to complete the table. Include units as necessary. Record the number of pennies dated before 1982. Weigh (as a group) the pennies dated before 1982. Record the total mass. If you’re unfamiliar with using an electronic balance, watch this video before continuing. Calculate and record the average mass of a single penny. If you need help with the calculation, visit the averaging data section of the math review. number of pennies: 8 combined mass of the pennies (g): 49.2 average mass of a penny (g): 5.525 Part C Now gather all of your pennies dated after 1982. Complete the table for the post-1982 pennies using the same steps from part B. number of pennies: 9 combined mass of the pennies (g): 51.7 average mass of a penny (g): 5.744 Part D In parts B and C, you measured the average mass of each group of pennies. Now you’ll measure their volume. (For this part, assume that the pennies dated before and after…

What were the main results found in this experiment? Include both quantitative results (i.e. important calculated values, including percent error) and qualitative results (i.e. important properties that were investigated).

Part 3: Calculate density of a metal an unknown metal. 1. Using the pictures below, record the displayed data in the data table in the report sheet. Make sure to include the right number of significant figures in the measurements and calculations. Mass measurement 7.1 g Volume of water measurement. There's only one measurement here – the larger image is for magnification only. -20 15 m Volume of water and metal measurement. There's only one measurement here – the larger image is for magnification only. 20 m 15

you combined 25 ml of milk with 30 ml of vinegar. After 10 minutes you observe the mixture again and the graduated cylinder now reads a total of 51.5 ml. How many ml have evaporated from the mixture?

O MEASUREMENT Adding or subtracting and multiplying or dividing measurements A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 1.5 g • She put some solid sodium hydroxide into the graduated cylinder and weighed it. With the sodium hydroxide added, the cylinder weighed 36.669 g. • She added water to the graduated cylinder and dissolved the sodium hydroxide completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 37.11 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. g mL Explanation -1 Check 99+ 0/5 VUDU © 2023 McGraw Hill LLC. All Rights…

Density of a Solid Material Water was poured into a 25-ml graduated cylinder (Figure A). Into it was placed a sample of solid material weighing 25.867 g, resulting in the rise of the water (Figure B). Determine the density of the liquid material. Report all quantitative data with the proper number of significant figures. Don't forget to write the units. ml ml. 25 25 20 20 15 15 10 Fill the table. Show your solutions. Weight of the solid material Precision of the graduated cylinder Volume of the water + solid material Volume of the water Volume of the solid material Density of the solid material

An analytical chemist weighs out 0.181 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0900M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 34.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. x10 mol

how can i plot this data for concentration with depth?

If you calculated from your titration that there was 13.75 mg of vitamin C in your fruit juice sample, calculate the concentration of vitamin C in mg/mL. (Concentration = mass/volume) Refer back to the first question on this report (or the procedure) for the volume of your fruit juice sample. Include the unit and two decimal places in your answer.   First question answer 20.00 mL

Jacquel Adding or subtracting and multiplying or dividing measurements A chemistry student must write down in her lab notebook the concentration of a solution of potassium chloride. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 4.200 g • She put some solid potassium chloride into the graduated cylinder and weighed it. With the potassium chloride added, the cylinder weighed 71.0 g. • She added water to the graduated cylinder and dissolved the potassium chloride completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 133.0 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. Ch 8 mL Explanation Check O2021 McGraw-Hill Education All Rights Reserved…

1.00 mL is taken from a stock solution of concentration 8.47 g/L and added to a 10.0 mL volumetric flask and diluted up to the calibration mark. What is the new concentration (in grams per liter)? Give your answer to three significant figures. g/L

4. The following data was collected from a solution that was prepared to allow a sample of plastic to neither float nor sink, but simply be suspended. What is the density of the Mass vs. Volume solution? Show units! 14 12 10 8. What is the density of the plastic sample? Show units! y = 1.2186x R² = 0.9945 4 6. 8 10 12 Volume (mL) 2. 64 Mass (g)

It is always important to label everything in the dispensary or the medicinal chemistry laboratory. One student made aspirin and the other student made paracetamol. Both students left their unlabelled samples near the balance. Give details of two techniques that you could use to distinguish between these samples

How many mL of (5.0300x10^0) M NANO3 would be needed in a dilution experiment to make (8.56x10^2) mL of (2.3400x10^0) M NANO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer

3. Plot the mass and volume data in your Data Table 1 to graphically determine the density of water using total mass (on the y-axis, in grams) vs. total volume (on the x- axis, in milliliters). You may elect to complete this graph by hand using the graph paper provided, or using a graphing program such as Microsoft Excel. Draw one "best fit" straight line through all your plotted points. Make sure to label both axes, and properly title the graph. Calculate slope of the line (Show actual calculations directly on graph, and clearly label the two points on the line used for your slope calculation) slope =______ The density of water as determined graphically is: _g/mL (Since the slope of the line indicates change in mass over change in volume, the slope of your line is the density of the water.)