5. 3 % of NaOH solution is required during clay content determination laboratory work. Describe briefly how you will prepare such solution for your work. Show any calculations involved.
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- A commercial base solution, NH3 has a specific gravity of 0.898. Calculate the molarity of a 28.0 % (w/w) NH3 (17.02 g/mol) solution. (Assume specific gravity has the same units as that of density)50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known volume of pure liquid pyridine and diluting to 500 mL with ethanol. The molar mass of pyridine is 79.1 g/mol, and its density at room temperature is 0.982 g/mL. What volume of pyridine is required for this solution?24 g of sodium hydride were added to 1 L.of water. The result solution reacted with 100 ml of water solution of nitric acid (HNO3) = 30 %, 0 = 1.18 g/ml). Calculate mass fractions of all compounds in the final solution.
- What is the boiling point of a 0.50m aqueous solution of aluminum nitrate? (The boiling point elevation constant for water is 0.512C kg solvent/ mol solute) Answer choices are: a.) 100.51 b.) 101.02 c.)102.05 d.)106.60 I know the answer is B but i would like to see step by step how to solve this problemA. Calculate the concentration of sugar in this solution using the volume percent equation. For the purpose of this exercise, it can be assumed that the weight of the drink mix is 0.00 g. The volume of the solution is 3 and 1/3 cups. Calculate and record the volume percent (g/mL). (Note that 1 cup = 236 mL). Volume %=Volume of Solute / Volume of Solution ×100% I used 1/2 cup of granulated sugar and 1/2 tsp of the drink mix, and 3 cups of water. B. Calculate the concentration of each diluted solution using the equation below and the volumes in Table. C1V1=C2V2 Where: C1=concentration of stock solution V1=volume of stock solution C2=concentration of diluted solution V2=volume of diluted solution (This is all the information that I have)How much amount of solids (in grams) do you need to prepare the following solutions? Preparation of SolutionsPrepare the following solution quantitatively using boiled distilled water per class:1. 250.0 mL 1.0 M stock HCl solutionNOTE: Use the 3.0 M HCl solution from Solution Preparation experimentPrepare the following solution quantitatively using boiled distilled water per group:1. 250.0 mL 0.0500 M standard HCl solution from 1.0 M HCl
- 28. A solution contains 125 g of a compound and 555 g water. The boiling point of the pure solvent is 100.00 oC. The solution has the boiling point of 102.40 oC. Calculate molar mass of compound. Kb for H2O : 0.52 oC kg / mole i = 3 a.146 g/ moleb.65.9 g /molec.125 g/ moled.14.5 g/ mole30.0 g of K2Cr2O7 is completely dissolved in 50.0 g of hot H2O. This solution is then cooled to 20 °C. What mass of K2Cr2O7 would precipitate?Provide your answer rounded to 2 significant figures.Ab asked Mi to perform an experiment on freezing point depression. The solution was prepared by dissolving 2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). Mi determined the freezing point of the solution to be -3.48 °C. She later found out that the salt she used was sodium chloride that was contaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium chloride present in the salt sample.
- Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?A solution of 655 mL of 0.852 M CO(NH2)2 is mixed with a solution of 432 mL of 0.487 M CO(NH2)2. It is then evaporated on a hotplate to a volume of 825 mL. What is the molarity of CO(NH2)2 in this final solution? [Be aware that evaporation only changes the amount of water, not the amount of CO(NH2)2, because the boiling point of CO(NH2)2 is nearly 200 °C, too high to evaporate out of the solution to a significant extent].Atrazine is a herbicide that is commonly used in the United States. The Henry's law constant of atrazine is 3 × 10−6 atm-L/mol or 1 × 10−7 (dimensionless) at 20 oC. The vapor pressure is 4 × 10−10 atm. a. Calculate the solubility of atrazine in soil pore water in mg/Lwater (Hint: use molecular weight of 216 g/mol to convert mol/L into mg/L). b.Calculated the concentration of atrazine in soil air in mg/Lair. c.What is the % of total atrazine mass in the soil gas? Assume the aquifer contaminated with atrazine has a residual gas saturation (i.e., the % of soil pores occupied by gas) of 15%. d. Can SVE be used to remediate atrazine-contaminated vadose zone? Justify your answer as to why or why not.