Post Lab 10

1. During the set-up of a distillation or a boiling point apparatus, the position of the bulb of the thermometer is crucial. Why is it so important to obtain accurate results?

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Match the units to the setup below for calculation of molarity X when dissolving a liquid X (X g)(density = D g X/mL X) in a liquid Y (Y mL)(density = D g Y/mL Y). All equations are set up so that the unit on the bottom cancels with the unit on the top to its immediate left. Be sure to match any unused answers to "Unused answer". X gx= 2._ = 7. _ 1.- 5._ X gX :+Y mL 6. mL X 1. 1. mol X/L 2. 2._ MW g X 3. 3. Dg X 4. 4._ 1000 mL 5. 5._ 6. 6._ 1 L 7. 7. 1000 L 8. Unused answer 1 mol X > > > > > > >

11 of 11 I Review | Constants Periodic Table Suppose that you want to find the equation for a line that passes through the two points (0,3) and (4, 9). What is the slope of this line? Express your answer numerically. > View Available Hint(s) Πνα ΑΣΦ ? m = Submit rt C Complete previous part(s) 9:41 PM 36%

- 1 A certain substance X has a normal freezing point of – 10.2 °C and a molal freezing point depression constant K,=4.75 °C·kg•mol *. A solution is prepared by dissolving some urea ((NH,) CO) in 500. g of X. This solution freezes at – 12.1 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits. g x10

3. A solution of 20.91 % by weight H,So, has a specific gravity of 1.150. What is the normality of this solution? Water is added to dilute this solution to a solution of 3.03% by weight H,SO, (SG= 1.020). What is the new normality of the resulting solution and how were they mixed? (Assume 100 ml of the original solution was used.)

A 25.0 ml aliquot of a well-shaken and filtered sample of river water is pipetted into an evaporating dish. The sample was heated to dryness. Determine the concentration of Total Dissolved Solids (TDS) in mg/L given the following data: Mass of evaporating dish = 25.5 g Mass of dried sample plus evaporating dish = 25.9729 g Note: Round off your answer to the nearest whole number.

C Fn A student mixes 1.0 mL of aqueous silver nitrate, AgNO3(aq), with 1.0 mL of aqueous potassium carbonate, K₂CO₂ (aq), in a clean 3 test tube. What will the student observe? Select the single best answer. O Bubbles will form within the liquid mixture. Jx F1 OA silver mirror will coat the interior of the test tube. O The mixture appears to be white and cloudy. Continue 61°F Partly cloudy O The mixture will remain colorless and transparent, but the test tube will feel hot. S O The mixture will remain colorless and transparent. F2 @ 2 F3 # 3 F4 $ LA 4 Search 8 1 F5 % 5 F6 < F7 & N 7 F8 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi M * O S F9 DELL prt sc F10 home F11 Submit Assignme X end F12 insert

1.    In your pharmacy you have a balance with a sensitive requirement of 7mg; 10,25,50 and 100ml graduated cylinder; and 1 oz apothecary and 4-ounce apothecary conical cylinder. What is the minimum measurable volume in ml using the graduated cylinder?a.    5b.    20c.    1d.    2

I don’t need an explanation, just an answer.

A solution is prepared by mixing 20.0 mL of 0.1 00M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of SCN^- in this solution? Give answer with correct amount of significant figures. 

A stock solution of analyte is made by dissolving 34.83 mg of copper (II) acetate hexahydrate(fw = 289.73 g/mol) in 25.00 mL of water. A second stock solution of internal standard is madeby dissolving 28.43 mg of germanium (I) acetate (fw = 190.74 g/mol) into 25.00 mL of water.These solutions are used to make a series of standards for flame atomic absorption analysiscalibration. The standard solutions (each 10.00 mL total volume) should have the followingconcentrations of copper: 10.00; 25.00; 50.00; 100.0; and 200.0 μM. Each calibration solutionshould also contain 50.00 μM of germanium. What is the analyte stock solution concentration? What is the internal standard stocksolution concentration?Complete this table.

. In C.AJ = - kt.tln [A.o]. t¹/₂ = 0.693 K In = KE •1• [A]o⋅=⋅· 100 ·/. [A] + = left . CAJO. CAJE In. [100] [s] t =.kt K= 0.693 t¼½₂ CAJO t = |n² Ch t = ln [AG] ·K CAJO K= In [At]. t Formulas Problem: Na-24 has a half life of 15 hours. How much of a 20.09. ·Sample would remain after decaying for 60 hours? Plz explain step by step. using the formulas..

I need help with part A,B,C

- 1 A certain liquid X has a normal freezing point of -3.20 °C and a freezing point depression constant K,=5.59 °C·kg•mol A solution is prepared by dissolving some urea (CH¸N,O) in 650. g of X. This solution freezes at -8.1 °C. Calculate the mass of CH,N,O that was dissolved. Round your answer to 2 significant digits.

1. (answer the questions in the tan boxes in the tables below each question) A student conducted an investigation to determine the effect of water temperature on the amount of sugar that dissolves in a beaker of water. Identify components for trial 1 of this investigation. Beaker Number 1 2 3 4 Amount of Water (mL) 100 100 100 100 Amount of Water (mL) Trial 1 Temperature of Temperature of Amount of Sugar Sugar (°C) Water (°C) Dissolved (g) 20 20 20 20 Temperature of Sugar 5 10 15 20 185 189 194 204 Temperature of Water Terms Variable Constant Amount of Sugar Dissolved

A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer.   I'm confused on what the next step is from here. I dont know if I need to switch the 10-3 to the bottom to make the 103 and how would I solve the problem from here?

Sucrose solution for experiment 1: (Question a-c)Prepare a solution of sucrose by accurately weighing 9.0 – 9.25 g of sucrose into a 100mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.NaCl solution for experiment 2: (Question d-f)Prepare a solution of NaCl by accurately weighing approximately 1.5 g of NaCl into a 100 mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.MgCl2٠6H2O solution for experiment 2: (Question d-f)Prepare a solution of magnesium chloride by accurately weighing approximately 3.6 g ofMgCl2٠6H20 into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mLdistilled water. Mix until all the crystals dissolve

An aqueous solution is made of the diprotic acid H₂A to a concentration of 0.11 M H₂A. Kat-3.0 x 104 and K₁2=2.5 x 10-9 What is the [A2] in this solution? Your answer should have 2 significant figures and be expressed in scientific notation (i.e. 3.0 x 102 as 3.0e2)

2. A serum is diluted 1:20 then 2 parts of the resulting dilution is added to 40 parts saline. Then 3 parts of the last dilution was added to saline to have a total volume of 6 parts. What is the final dilution?

A student prepares a 1.1 mM aqueous solution of 4-chlorobutanoic acid (C3H, CICO,H). 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 S

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3A. Determine the Molarity of the Sodium ion in a solution of Na2SO4.10H20 if you add 3.041 grams to a final volume of 150 ml. Add 3.041 g of Na2SO4.10H20 in a beaker pour upto 150ml of water to achieve 0.063 Molar. Calculation Na2SO4.10H20 MW = 322.03g/mol Grams = 3.041 g Vf = 150ml = 0.15L M= mols of solute/ L of solution (3.041g/1) (1mol/ 332.2g) = 0.00915mol Na2SO4.10H20 0.00915mol N22SO4.10H20/ .15l= 0.061 M 2 Na = 2*0.061mol/L = 0.126 mol/L Answer the question below Make a 1:100 solution of Na2SO4.10H20 in 100 ml of water from your previous solution. What is the final concentration of the Sodium lon?

1.) In the Dumas method for determining the molar mass of an unknown volatile liquid, a sample of a volatile liquid that boils below 100 oC is vaporized in a boiling water bath and the mass of the vapor required to fill the flask is determined. The following data was collected:  Flask Volume 100.0 +100.0 + 79.6 mL = 279.6 mL Mass of Flask + Cap 143.85 g Mass of Flask + Condensed Liquid 144.95 g Mass of Condensed Liquid 1.10 g Temperature of Water Bath (oC)  84.1 oC Barometric Pressure (atm) 0.985 atm   a.) What is the molar mass of the unknown?  b.) What will its temperature be when the pressure is 1.20 atm and the volume is 250.0 mL?

Archimedes, a famous Greek scientist, was given a problem by King Hieron II of Syracuse (Sicily). The king suspected that his crown, which was supposed to be made of pure gold, contained some silver alloy, and he asked Archimedes to prove or disprove his suspicion. (It turned out that the crown did not contain silver.) How would you experimentally determined whether or not the crown was pure gold? (Hint: The method came to Archimedes when getting into a full bathtub. See the footnote in Experiment 22 for Archimedes’ solution.)