iew | Constants | Periodic Table A red blood cell has been placed into each of three different solutions. One solution is isotonic to the cell, one solution is hypotonic to the cell, and one solution is hypertonic to the cell. Sort each beaker into the appropriate bin based on the cell's reaction in each solution. Drag each item to the appropriate bin. • View Available Hint(s) Reset Help Hypertonic Isotonic Hypotonic

iew | Constants | Periodic Table A red blood cell has been placed into each of three different solutions. One solution is isotonic to the cell, one solution is hypotonic to the cell, and one solution is hypertonic to the cell. Sort each beaker into the appropriate bin based on the cell's reaction in each solution. Drag each item to the appropriate bin. • View Available Hint(s) Reset Help Hypertonic Isotonic Hypotonic

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…
magnesium hydroxide, Mg(OH)2, found in milk of magnesia, has a solubility of 7.05x10-3 gL-1 at 25ºC. Calculate the Ksp for Mg(OH)2 with a tolerance of +8 (Please type answer)
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Use the following data to calculate the Ksp value for each solid. a. The solubility of CdC2O4 is -4 1.2 x 107 mol/L. Ksp - b. The solubility of Bil3 is 1.32 × 10-5 mol/L. Ksp Submit Answer Try Another Version 1 item attempt remaining
How many mL of 0.779 M HNO3 are needed to dissolve 5.15 g of BaCO3? esc 1 F1 AAB 2 Q *** F2 W # 3 80 F3 E $ 4 000 000 F4 2HNO3(aq) + BaCO3(s) Ba(NO3)2(aq) + H₂O(l) + CO₂(g) R Cengage Learning | Cengage Technical Support % er oo 5 F5 MacBook Pro T A 6 F6 & 7 Y F7 mL * DII U F8 8 DO 9 1
4. The Ksp for MgCO3 = 1.1 x 101º. CIRCLE the solubility of MgCO3 in pure water. a) 1.1 x 10-10 M b) 1.1 x 108 M c) 1.1 x 107 M d) 1.1 x 106 M e) 1.1 x 10$ M
6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…
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Please help me out with making flowchart with thes steps. Write the result. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in the centrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in each centrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid in each sample. 5. To the centrifuge containing…