One beaker contains 25 mL of 1.60 M HCL, and a second beaker contains 58 mL of 0.40 M NaOH. Both solutions were initially at 20 °C. We pour both beakers into a large insulated container which contains 8 g of ice, initially at -60 °C. Calculate the final temperature of the resulting solution. Note that the heat of neutralization is -57.3 kJ/mol. T (°C)

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At a particular temperature, suppose that 24.4 g solute is added to 50.0 g water and, after mixing, 0.3 g of the solute remains undissolved. What is the solubility of this solute at this temperature in grams per 100 g of water? (Enter in standard notation with one digit after the decimal point) Type your answer......

1. Develop a detailed separation scheme for the separation and determination of the percent composition of your sample which will be a mixture of NaCl, NH.CL, and sand. You are expected to use the properties of the components listed below and some of the techniques listed in the table in the pre-lab queries (and used in Separations I). Keep in mind that any chemistry student should be able to pick up your scheme, understand it, and use it to complete the separation and calculation of % composition. Place the scheme on a separate sheet of paper. Component Solubility (@25°C) Melting Point Hardness sodium chloride, NaCl 35 g/100 mL water 801°C soft ammonium chloride, NH&Cl 37 g/100 mL water sublimes 350°C soft sand, SIQ2 insoluble 1600°C hard Example of compounds in a container. Naci NH.CI sio2 Exploring the Chemical World, PGCC, 2003 4 RESULTS Show all calculations with units in this space.

Please don't  provide handwritten solution .....  The average human body contains 5,830g of blood. What mass of arsenic is present in the body if the amount in blood is 0.55 ppm?

Give correct detailed Solution with explanation needed...don't give Handwritten answer

Please don't provide handwritten solution......

POST-QUESTIONS 1. After a student dissolved 0.5 g of white solid in water, she tested the conductivity and determined that the solution did not conduct electricity. The student then concluded: "when the white solid dissolved it 'just disappeared' so some sort of error must have been made because all solids are ionic compounds and, therefore, are electrolytes." Comment on the student's conclusion. Is her statement a valid conclusion? If so, identify what is correct. If not, write a conclusion that would be correct.

The following evidence was obtained from an experiment to determine the molar concentration of a sodium nitrate solution. A sample of sodium nitrate solution was evaporated to dryness and the mass of solid residue was measured.Evidence:Volume of solution = 10.00 mLMass of beaker = 79.54 gMass of beaker and residue = 82.96 gFrom this data, calculate the molar concentration of the original sodium nitrate solution. Record only your numerical answer with the correct number of significant digits.  You do not need to include units as the units appear for you beside the answer box already.

Masses :  Ca = 40.08 g   S= 32.07 g  O= 16.00 g  A 35.0 mL sample of CaSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution?   step by step please