GMontenaro M3 Lab 1 Exploring Density

1. ASSERTION: The solubility of gases in water follows the order O2 < N2 < SO2 < CO2 < NH3. REASON: For appreciable solubility, the solute-solvent interactions should outweigh the solute-solute and     solvent-solvent interactions. a. Assertion and reason both are correct statements and reason is the correct explanation for assertion. b. Assertion and reason both are correct statements but reason is not the correct explanation for assertion. c. Assertion is a correct statement but reason is a wrong statement. d. Assertion is a wrong statement but reason is a correct statement. 2. ASSERTION: The solubility of all gases in water decreases with the rise in temperature. REASON: The dissolution of gases in water is an endothermic process. a. Assertion and reason both are correct statements and reason is the correct explanation for assertion. b. Assertion and reason both are correct statements but reason is not the correct explanation for assertion. c. Assertion is a correct…

Standardization of a sodium hydroxide (NaOH) solution against potassium hydrogen phthalate (KHP) yielded the following results: Mass of KHP, g Volume of NaOH, mL 0.7987 38.29 0.8365 38.96 0.8104 38.51 0.8039 38.29 MM KHP: 204.22 MM NaOH: 40.00 a. Calculate the mean molar concentration of sodium hydroxide. (First, compute the concentration of NAOH in each titration then compute for its mean/average value.) b. Calculate the standard deviation. Please provide solutions for your answers. If you have used your calculator for calculating for mean and standard deviation, you can just provide the formula with the values indicated.

A hollow square metal tube has a measurement of 2.42 in for each side and a weight of 53.71 g. The volume of empty space inside the tube was measured to be 0.93 in³. If the density of the metal used in constructing the tube is 11.81 g/mL, calculate the length of the tube in inches. Note: 1 in = 2.54 cm, 1 cm3 = 1 mL %3D Show your solutions in the next item Round your answer to 2 decimal places.

Note: The explanation of this work would be we did a work on the process of preparing diverse solution sets and regarding that these are the following sets of questions.  PART: 2 What happens to the solution's concentration when you add more solute to the same volume of solvent? How to raise the concentration of an aqueous solution? When is the ppm concentration applied? What do you conclude from this lab? Was your hypothesis confirmed or not? Explain your answer.

A 5.04 g sample of a solid containing Ni is dissolved in 20.0 mL water. A 5.00 mL aliquot of this solution is diluted to 100.0 mL and analyzed in the lab. The analyzed solution was determined to contain 5.53 ppm Ni. Determine the molar concentration of Ni in the 20.0 mL solution. concentration: M Determine the mass, in grams, of Ni in the original sample. mass: g Determine the weight percent of Ni in the sample. weight percent: % * TOOLS x10

PERCENT BY MASS Percent by Mass percent by mass = mass of solute x 100 mass of solution Percent by mass equals the mass of the solute divided by the mass of the whole salution, multiplied by 100. TRY THIS: A label on a bottle of cough syrup contains 25 mg dextromethorphan (DTN) dissolved in a solution weighing 1000.0 mg. Given the product above, choose the best percent by mass below and explain your answer with your work shown. a. 2.5% 1 b. 40% I c. 0.025% d. 2.4%

A traditional way of determining the concentration of alcohol in alcoholic beverages is by measuring thedensity of the solution, since these two characteristics of the solution (density and % alcohol) arerelated. This is a convenient determination method because it is low cost and can be done quickly. Thisis why customs officials sometimes use density measurements to classify alcoholic beverages and spirits.In the stockroom, you will find a variety of reagents including two alcoholic beverages. Design andperform an experiment to classify each of the two alcoholic beverages into one of the following fivecategories of alcohol strength (based on % v/v) defined by the Canadian importation laws:1. Less than 0.5% by volume2. 0.5% - 1.2%3. 1.2% - 7.0%4. 7.0% - 22.9%5. More than 22.9% by volume   Pre-Lab Questions1. Perform the following calculations and report the answer to the appropriate number of significantfigures:(a) An alcohol solution was prepared by adding enough water to 35. 0 mL of…

A certain liquid X has a normal freezing point of -1.20 °C and a freezing point depression constant -1 K₁=5.73 °C kg-mol . A solution is prepared by dissolving some ammonium sulfate ((NH4), SO4) in 750. g of X. This solution freezes at -6.4 °C. Calculate the mass of (NH4) SO4 that was dissolved. Round your answer to 2 significant digits. g x10 X Ś

A pool contains 4500 gallons of 1.4% chlorine solution, which means that 1 4% of the liquid in the pool is actially chlorine: the rest is water. The goal is to find how many gallons of chlorine would need to be added to increase the concentration in the pool to 3%. Round your answer to the nearest gallon. ___ gallons would need to be added to increase the concentration in the pool to 3%

When (8.09x10^1) g of a non-electrolyte is dissolved in (5.9500x10^2) g of a solvent (with Kp = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the molar mass (in g/mol) of the non- electrolyte solute? 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.

A student prepares a 1.2mM aqueous solution of crotonic acid C3H5CO2H. Calculate the fraction of crotonic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.

3. The following molarities were calculated from replicate standardizations of a NaOH solution: 0.502 8, 0.502 9, 0.502 3, 0.503 1, 0.502 6, 0.502 7, 0.503 4, and 0.502 5. Assuming no systematic errors, within what range are you 90% certain that the true mean value of the molarity falls?

KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.

Preparation of a standard solution of copper(II) sulfate pentahydrate 1. Weigh out accurately 9.99 g of copper(II) sulfate pentahydrate (CuSO4·5H2O) by taring using a clean and dry empty 250-ml beaker. 2. Add tap water to the beaker to reach the 50-mL mark on the side of the beaker. 3. Dissolve all the crystals of CuSO4·5H2O in the water using a clean glass rod for stirring. 4. Then using a glass funnel transfer all the blue solution to a 100-mL volumetric flask. Rinse the beaker with about 10 mL of water and transfer the solution to the volumetric flask. Repeat the rinsing of the beaker with another 10 mL of water and transfer the solution to the volumetric flask. This is called quantitative transfer of the solution. 5. Then add enough water to reach the calibration mark of the volumetric flask. (You will need to use a dropper to add the last few drops of water to ensure the meniscus is on the calibration mark). Close the volumetric flask with a stopper and mix the solution well (so…

A A student prepares a 0.52 M aqueous solution of 4-chlorobutanoic acid (C₂H CICO₂H). Calculate the fraction of 4- chlorobutanoic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. % ☐x X G

José performs an experiment to determine how much sugar can be dissolved in 250 milliliters (mL) of water at 25°C. He adds 50 grams (g) of sugar at a time to the water while stirring and observes the solution After adding sugar the eleventh tene (550 g), he notes that undissolved sugar has settled to the bottom of the container. He stops adding sugar and ends his experiment. In his lab write-up he concludes that the solubility of sugar in water at 25°C is 500 g per 250 ml. is his conclusion defensible, and why or why not? O No, because he did not add sugar enough times. Yes, because when he added more than 500 g it did not all dissolve. O No, because he does not know if any of the final portion of sugar dissolved. O Yes, because when he added the tenth portion (500 g) all of it dissolved.

What mass of cesium bromide must be added to 0.500 L of water d=1.00 to produce a 0.650 m solution? What are the mole fraction and the mass mL percent of CsBr? Be sure each of your answer entries has the correct number of significant figures. Part 1 of 3 Mass of cesium bromide = Part 2 of 3 Mole fraction= Part 3 of 3 Mass percent= % x10 g x10 X x10

A certain liquid X has a normal freezing point of 7.10°C and a freezing point depression constant =Kf3.27·°C·kgmol−1. A solution is prepared by dissolving some ammonium chloride (NH4Cl) in 700.g of X. This solution freezes at 6.4°C. Calculate the mass of NH4Cl that was dissolved. Round your answer to 1 significant digit.    __g

The density of a concentrated phosphoric acid solution is 1.514 g/mL solution at 20°C. It contains 141.6 g H3PO4 per 1.00E+2 mL of solution. Calculate the molar concentration of H3PO4 in this solution: Molar concentration = i M Calculate the number of grams of this solution required to hold 17.9 g H3PO4: Mass of the solution = i g Attempts: 0 of 15 used Submit Answer Save for Later étv N MacBook Air

Chemistry Tutorial O 2. (Based on Lime- soda process of water softening) QI. Calculate the amount of lime and soda required to soften 25,000 litres of water having following analysis: Ca(HCO, )2 4.86 ppm;Mg(HCO3)2 = 7.3 ppm;CaSO, 6.8 MgCl2 = 5.7 ppm; MgSO. = 9.0 ppm; SiO, = 3.5 ppm; NaCl = 5.85 ppm. (Ans. L = 490 g:S =490g) %3D

In the experiment of making salted eggs, a cleaned egg is immersed in a solution a lot of Nacl salt. Nacl in solution diffuses into the egg through the eggshelI, then towards the egg whites and yolks. Eggs can be considered perfectly spherical in shape with the radius in R and the thickness of the eggshell is T. The concentration of NaCl in the soaking solution is Caci,o and its value can be considered constant during the immersion process. Before being included in soaking solution, there is no Nacl in egg whites and egg yolks. Diffusion through eggshell can be ignored because it occurs very quickly. If the diffusivity coefficient of Nacl in egg white and egg yolk can be considered equal (DNaci), a. Use the component continuity equation table, so that the equation that is describe the profile of Nacl concentration in eggs (in the form of a differential equation along with the boundary conditions). b. Convert the equation obtained in point a into an equation of the form dimensionless…