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- b. Calculate the molar concentration of the malonic acid if 38.17 mL of 0.315 M potassium hy- Calculate the mass percent concentration of malonic acid using the molar concentration cal- droxide was required to neutralize 25.0 mL of malonic acid to a phenolphthalein end point. с. culated in part b and assuming the density of the solution is 1.01 g/ml. lo ba Citric acid (abbreviated H,Cit) is a triprotic acid, so 3 moles of hydroxide ions are required per mole of citric acid for complete neutralization. Write the balanced chemical equation for the reaction of citric acid with sodium hydroxide. (Note that citrate ion is actually a polyatomic ion with carbon, hydrogen, and oxygen atoms and an overall charge of -3. For now, express citrate ion as Cit.) a. ele booald sh w h Jf 36.10 mL of 0.223 M NaOH is used to neutralize a 0.515 g sample of citric acid, what is the molar mass of the acid?2H₂(g) + O₂(g) + 2H₂O (g) + energy (heat) 3. Pressure (Recall Gizmo activity: Equilibrium and Pressure) a. If the pressure of the system was increased, what else wuld this have an effect on? Temperature of the system? Concentration of species in solution? Volume?true b. If the volume of the system decreases, do you think the system would want more gas molecules or less gas molecules in the system to relieve the "stress" on the system? Based on this, what would happen to the forward and reverse reaction rates? Why?10 mL 1 M C6H5NH2 and 15 mL 0.1 M Al(NO3)3 are mixed. What concentration of: a. Al3+ is produced from Al(NO3)3 b. OH- is produced from C6H5NH2
- 2. How many grams (g) of CaSO4 is formed when 20 mL of 0.10 M Na2SO4 is added to 100 mL of 0.01 M CaCl2?4- Describe the preparation of 100 ml of 6 M HCl from concentrated solution that has sp.g 1.18 g/ml and 37 % HCI (36.5 g/mole).5. You have 97.0 mL of a 0.500 M stock solution of HCl that must be diluted to 0.200 M. How much water (in mL) should be added? 6. Express the concentration of a 0.120 M solution of NaF in mass percentage (w/w) and in parts per million (PPM). Assume the density of the solution is 1.00 g/mL. 7. Assuming 100% dissociation, calculate the freezing point and boiling point (in °C) of a solution with 98.4 g of AgNO3 in 1.00 kg of water. 8. Calculate the osmolarity of these solutions. Assume density of the solution is 1.00 g/mL. (a) 3.80 M MgCl2 solution Osmolarity = (b) 4.40% w/w glucose (C6H12O6) solution Osmolarity =
- 3. What is the percentage strength of a reagent solution prepared by dissolving 1.5 oz of silver chloride in enough distilled water to make 1 pint? a 0.3% b 1.5% c 9.0% d 9.9%Given that the solubility of Cd3(PO4)2 is 1.2 x 10 mol/L what is its Ksp value? Note: the formula mass of Cd3(PO4)2 is 527 g/mol. OA 2.5 x 10 35 O B. 2.7 x 10 33 C. OC1,5x10 34 10-34 D. 8.6 x 10 14 E. 1.4x 10 1486.5 g of MgCl2 (m.m. = 95.211 g mol−1), asoluble salt, is dissolved in pure water. Howmany moles (to one decimal place) of soluteparticles does this result in?A. 0.9 B. 1.8 C. 2.2 D. 2.7 E. 86.5
- A mixture of ethanol, benzaldehyde and KMnO4 is mixed together. Would you expect a precipitate to form based on the reactants functional groups?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…1. What volume of water is needed to be mixed with 150 ml of alcohol to prepare a 25.0 % alcohol solution ? 2. A 2.5 g sample of groundwater was found to contain 5.4 ug (microgram) of Zn 2+ . What is the concentration of Zn 2+ in parts per million?
