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Prepare your solvent, which will be a 1.0 M Metal Free HCl solution. First, calculate the volume of the concentrated acid necessary to prepare 600.0 mL of 1.0 M HCL. (I believe we are give 3 M HCl to dilute here). Put about 300 mL of DIW in your 800 mL beaker, and then VERY carefully add the calculated volume of concentrated HCl to the water. YOU SHOULD ALWAYS ADD ACID TO WATER, NOT THE OTHER WAY AROUND. Do not pour the acid from the large bottle into your graduate cylinder; instead pour it first into a beaker then pour from the beaker into your graduated cylinder. After adding the acid, fill the beaker to ~600 mL and then transfer your solution into your 1.0 L stoppered bottle and label the bottle. You will use this solvent for the next two weeks.
Prepare a calcium standard solution by accurately weighing between 0.35 - 0.40 g (I'm using .38 specifically) of standard calcium carbonate and quantitatively transferring the solid to a 250 mL beaker. Slowly add dropwise 6 M HCl until the sample stops effervescing and completely dissolves. Make the volume up to about 50 mL with DIW. Quantitatively transfer the solution into a 250 mL volumetric and dilute to the mark. Mix the solution carefully. Calculate the concentration of the Ca2+ in ppm (or mg/L) using the correct number of significant figures assuming the 1.0 HCl has a density of 1.000 g/mL. Show these calculations clearly in your notebook and on your report form. Recall that calcium is only ~40% of the CaCO3.
Carryout the following conversions. Report your answer to the correct number of significant figures
a 70g piece of ice at 0c is added to a sample of water at 8c, all of the ice melts and the temp of the water decreases to 0c, how many grams of water were in the sample?
525 mm of Hg; neon, 65 mm of Hg, and nitrogen, 250 mm of Hg. What is the total pressure of the mixture?
The normal melting and boiling points of O2 are -218C and -183C respectively. Its triple point is at -219C and 1.14 torr, and its critical point is at -119C and 49.8 atm.
Find the molarity of a Ca(OH)2 solution,given that 363 mL of it is neutralized in a titration by 187 mL of 0.0058 M HNO3.
2H2S (g) + 3O2 (g) → 2H2O (g) + 2SO2 (g) If 3.50 G Of H2S Are Used In The Above Reaction, What Will Be The Theoretical Yield Of Water In Grams?
A 1.50L sample of neon gas at 1.10 atm and 25 degrees celsius is heated to 45 degrees celsius. The neon gas is then subjected to a pressure of 1.50 atm. Determine the new volume of the neon gas.
what is the enthalpy change per mole of ethanole burned. the spacefic heat capacityof H2O is 4.184J/gC
Explain the use of nuclear isotope in medical field and Write a paragraph expaining what nuclear isotope can be used for medical purpose
C4H10(g) + O2(g) CO2(g) + H2O(g) Consider the above unbalanced equation. What volume of O2 at 555 mm Hg and 56.0°C is required to produce 285 mL of CO2 at 780. mm Hg and 131°C?
The wavelength of maximum absorbance is solvent dependent. in water, the wavelength of maximum absorbance is 453 nm.
What phase or phases are present when 250. kJ of energy is removed from this sample? Specific heat capacities:
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