Lab 1 - Crystallization

Dissolution Distilled H20 Concentration 0.01 M HCI Concentration (mg/ml) Time Total amount A Total amount A (mg/ml) (mg) (mg) 5 0.16 0.1 10 0.24 0.18 15 0.35 0.25 20 0.48 0.34 25 0.58 0.4 30 0.67 0.5 1. Plot the given data on an ordinary paper and find the slope for each line then calculate the IDR constant for aspirin in the two dissolution media, water and HCI. NOTE: Slope of the calibration curve = 1.0 (mg/ml and saturation solubility of salicylic acid is equal to 2.0 gm/L.

experiment A pair of 100 mL samples of water are taken from a well bored into a large underground salt (NaCl) deposit. Sample #1 is from the top of the well, and is initially at 32 °C. Sample #2 is from a depth of 50. m, and is initially at 42 °C. Both samples are allowed to come to room temperature (20. °C) and 1 atm pressure. An NaCl precipitate is seen to form in Sample #1. Two 250 mL samples of water are drawn from a deep well bored into a large underground salt (NaCl) deposit. Sample #1 is from the top of the well, and is initially at 42 °C. Sample #2 is from a depth of 150 m, and is initially at 8 °C. Both samples are allowed to come to room temperature (20 °C) and 1 atm pressure. An NaCl precipitate is seen to form in Sample #1. predicted observation (choose one) A bigger mass of NaCl precipitate will form in Sample #2. A smaller mass of NaCl precipitate will form in Sample #2. The same mass of NaCl precipitate will form in Sample #2. No precipitate will form in Sample #2. I…

C. 92.3 m d. 226 mL 4. Solution B was prepared from solution A as shown below. The concentration of solution B is: 2. 2.00 M b. 2.00 x 10-3 C. 8.00 M d. 8.00 x 10-3 هایی ناخذ الكيو ستة آلية deez 2.00 ml A 500.00 ml M = 2.00 M X 500.00 ml M = ??

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Chemistry HW need help, how to do these caculation and answer these questions?

Can I get detailed explanation for this table , mentioning the apparatus and when’s the timer is started ? What happens next

At 0 oC, the solubility of sodium acetate in water is 36.1 g per 100 g of water and at 40 oC, the solubility is 66.4 g per 100 g of water. A 100 g sample of sodium acetate is dissolved in 250 g of water at 40 °C. The solution is cooled to 0 °C and a small amount of solid is observed. This solution is ________. - supersaturated - saturated - unsaturated  - hydrated

Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…

5. Suppose you have a mixture of water and your 2-chloro-2-methylbutane product in a separatory funnel. Use densities to predict which phase will be the top layer in the funnel. a. 2-chloro-2-methylbutane (organic phase) b. water (aqueous phase) c. there would only be one phase since the substances are miscible

Pre-lab question #8: Suppose you were dissolving a metal such as zinc with hydrochloric acid. How would the particle size of the zinc affect the rate of its dissolution? As the particle size of the zinc increases, the rate of dissolution AA (decreases/increases).

Molar concentration of the bleach stock solution: .134 mol/L Solutions(Dilutions) Concentration% Experiment 1 0.25 Experiment 2 0.50 Experiment 3 1.0 Fill in the OCl- molar concentrations for each experiment. Solutions(Dilutions) OCl- Concentrationmol/L Experiment 1   Experiment 2   Experiment 3

Predict what will be observed in each experiment below. experiment predicted observation (choose one) A bigger mass of NaCi precipitate will form in Sample 2 A pair of 100 ml. samples of water are taken from a well bored into a large underground salt (NaCI) deposit. Sample 1 is from the top of the well, and is initially at 32 C. Sample 2 is from a depth of 50. m, and is initially at 42 °C. Both samples are allowed to come to room temperature (20. "C) and I atm pressure. An NaCI precipitate is seen to form in Sample #1. A smaller mass of NaCl precipitate wi form in Sample 2. The same mass of NaCl precipitate will form in Sample 2. O No precipitate will form in Sample 2. I need more information to predict whether and how much precipitate will form in Sample #2. OA bigger mass of NaCl precipitate wil form in Sample 2 Two 250 ml samples of water are drawn from a deep well bored into a large underground salt (NaCI) deposit. Sample 1 is from the top of the well, and is initially at 42 °C.…

Rearrange equation 1 to solve for the molecular weight of a compound assuming you know the mass of solute added

A student wants to determine how different factors affect the rate of dissolving a solid in water. Trial Size of Particles Rate of Dissolving 1 small 10 sec medium 20 sec 3 large 30 sec What procedures can be performed on trials 2 and 3 so that the rate of dissolving is the same as trail 1? The student can decrease the temperature The student can decrease the pressure The student can increase the pressure The student can increase the temperature

Data Sheet 4 ble gives the recommended mass of salt to dissolve in each of the four test tubes. Show a sample calculation for the solubility of KNO, using your actual mass from tube #1. Complete your graph on the back of this sheet. Solution # Recommended mass KNO3 Actual mass of KNO, (g per 5 mL H₂O) Solubility & KNO, 100 g H₂O Saturation temperature (°C) (g) 1 2.0 51.3 2.1971 2 62.5 4.0 11.1568 3 72.7 6.0 6.0112 83.6 4 8.0 806 Sample Solubility Calculation: Questions 1. According to your data, how does the solubility of KNO, change with increasing temperature? Does this indicate an endothermic or exothermic dissolving process? Explain. 2. Using your graph, indicate if each of these solutions would be saturated or unsaturated: a) 110 g of KNO3 in 100 g of water at 40 °C b) 60 g of KNO3 in 100 g of water at 70 °C c) 140 g of KNO3 in 100 g of water at 60 °C 3. According to your graph, what mass of KNO3 will dissolve in 100 g of water at 30 °C?

I have the density of solution that is 1.092g/ml in an unknown solution, how can I get the sucrose solution % to put on my graph?

1. Solubility Test Table 1. Results for the solubility test. OBSERVATION* INFERENCE SAMPLE Ethyl acetate ** Нехаne Methanol Water Coconut oil Vitamin E Beef fat Miscible (soluble) or immiscible (insoluble) ** polar or nonpolar Sudan IV Test Table 2. Results for Sudan IV test. OBSERVATION* INFERENCE SAMPLE Нехаne Ethyl acetate Methanol Water ** Coconut oil Vitamin E Beef fat Homogeneous or heterogeneous mixture ** polar or nonpolar

At 0 oC, the solubility of sodium acetate in water is 36.1 g per 100 g of water and at 40 oC, the solubility is 66.4 g per 100 g of water. A 100 g sample of sodium acetate is dissolved in 250 g of water at 40 °C. The solution is cooled to 0 °C and a small amount of solid is observed. This solution is ________. - hydrated -saturated -supersaturated - unsaturated

Predict what will be observed in each experiment below. predicted observation (choose one) experiment A bigger mass of NaCl precipitate will form in Sample #2. Two 250 mL samples of water are drawn from a deep well bored into a large underground salt (NaCl) deposit. Sample #1 is from the top of the well, and is initially at 42 °C. Sample #2 is from a depth of 150 m, and is A smaller mass of NaCl precipitate will form in Sample #2. The same mass of NaCl precipitate will form in Sample #2. initially at 8 °C. Both samples are allowed to come to No precipitate will form in Sample #2. room temperature (20 °C) and 1 atm pressure. An NaCl precipitate is seen to form in Sample #1. I need more information to predict whether and how much precipitate will form in Sample #2.

Table 5, Dissolved oxygen of distilled water at different temperatures Temperature (C) Volume of aliquot (ml.) 5.00 Volume of sodium thiosulfate used (mL) Dissolved oxygen (ppm) 10.3 4 13.60 25 5.00 12.20 8.23 73 5.00 5.40 4.03 1. From your data, calculate the dissolved oxygen content in distilled water at 73 °C (data in Table 5) without using the DO formula. Detailed calculation and formulas are required in this answer.

I need help calculating the initial concentrations please.

Can someone check to see if #9 through #12 are correct with the information provided

2. Show solution. Thanks!

1. Answer the following questions based on the table: Pickling Vinegar Conc NaOH (M) 0.1005 Trial #1 Trial #2 Trail #3 Trial #4 Volume Vinegar (mL) 2.00 2.00 2.00 2.00 Initial Volume NaOH (mL) 0.32mL 0.22 1.02 0.44 Final Volume (mL) 24.25mL 24.20 25.00 24.45 Volume NaOH added (mL) 23.93mL 23.98mL 23.98mL 24.01mL a) Calculate the Average Volume NaOH used...show the trials that have %difference within 1% of each other. If you need to discard any trials- make sure to note this. b) Mass percentage of acetic acid in vinegar using your average volume of NaOH from Q1: (include a balanced reaction equation and show all work) c) % error calculation. Show ybur work in full. See Appendix B for details. (Reminder: Regular vinegar is 5.25% listed on bottle, pickling vinegar is 7.34% listed on bottle) d) In the titration of vinegar, a student uses 12.36 mL of NaOH(aq) (Molarity 0.100 M) to titrate a 2.00 mL sample of vinegar. If the student used lithium hydroxide (Molarity: 0.200 M) instead, what…

2. Questions: 1. CHM-202 Lab 2 Freezing Point Depression Rev2 G6-2022 10/14 From your understanding of colligative properties, how would you design an experiment to measure the freezing point of a material which freezes at -2 °C using the same apparatus used in this laboratory and any chemical reagents commonly found in a chemical laboratory. Ice is the only material you have available to cool the solutions. If you measured the boiling point of the solution used in Trial 4, would you predict it would have a boiling point equal to, higher than, or lower than the boiling point of pure cyclohexane? Explain your answer.

Part C: Determination of the alcohol content of unknown liquor Stretien Volume (mL) Sample ТИШТИНА 0.00% alcohol 10.0% alcohol 20.0% alcohol 40.0% alcohol 50.0% alcohol Unknown Mass (g) 1o podina ko 9.8919 9.7899 9.600 9 9.420 д % Alcohol content of the liquor 9.2155 9.5089 2VLELA CVOLION: MEAEK EVI OK DRA IVBOKY LOBAN ocen 10.00 10.00 10.00 10.00 10.00 10.00 Density (g/mL) 0.00% alcohol calculation: ися → о 0.99 во 0.99 To Z si doleW 120.00 supinubst sdi na LANG 411 bet [squardas: 0.97 0.94 in oil to notisalarisi 0.92 0.95

A sample (50 mL) of a bottled water was added to a 100 mL volumetric flask and then diluted to the mark. From this stock solution, 50 mL was taken, added to a 100 mL volumetric flask and diluted to the mark. Final concentration of the serial dilution: 587.7161ppm. 1. what is the concentration in the original bottle (ppm)