79101112A sample of 100 Unit/L is diluted 1 in 10, what is theconcentration of the final solution?2.0 mL of plasma, 3.0 mL of reagent, and 5.0 mL distilledwater are mixed together, what is the dilution of the plasmain the final solution?A sample has been diluted 1 in 5 dilution with a finalconcentration of 5 Units/L, what is the originalconcentration?You are required to prepare 1 in 10 dilution using 0.5 mLplasma, how much diluent do you need?How to prepare 200 mL of 5% albumin solution from 50% albumin?Equation:Volume of 50% albumin required:Volume of solution (water) required:How many grams of CaCl₂ 2H₂O are needed to prepare 200 mL of a 0.2 M CaCl₂solution?1 mole of CaCl2-2H₂O equals to:Equation:CaCl2 2H₂O required in grams with one decimal places:

The formula of dilution is M1V1 = M2V2 Where M1 and M2 are initial and final concentration V1 and…

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A sample of 100 Unit/L is diluted 1 in 10, what is the concentration of the final solution?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 1P: A patient has a “cholesterol count” of 214. Like manyblood-chemistry measurements,this result is...

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Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
A compound has a solubility in water of 250 mg/L at 25C. Should this compound be characterized as a soluble or insoluble compound at 25C?
Refer to Figure 13.10 ( Sec. 13-4b) to answer these questions. (a) Does a saturated solution occur when 65.0 g LiCl is present in 100 g H2O at 40 C? Explain your answer. (b) Consider a solution that contains 95.0 g LiCl in 100 g H2O at 40 C. Is the solution unsaturated, saturated, or supersaturated? Explain your answer. (c) Consider a solution that contains 50. g Li2SO4 in 200. g H2O at 50 C. Is this solution unsaturated, saturated, or supersaturated? Explain your answer. Figure 13.10 Solubility of ionic compounds versus temperature.
6-20 Give a familiar example of solutions of each of these types: (a) Liquid in liquid (b) Solid in liquid (c) Gas in liquid (d) Gas in gas
A patient has a “cholesterol count” of 214. Like manyblood-chemistry measurements,this result is measured inunits of milligrams per deciliter (mgdL1). Determine the molar concentration of cholesterol inthis patient’s blood, taking the molar mass of cholesterolto be 386.64gmol1. Estimate the molality of cholesterol in the patient’sblood. If 214 is a typical cholesterol reading among men inthe United States, determine the volume of such bloodrequired to furnish 8.10 g of cholesterol.
A sample of aluminum sulfate 18-hydrate, Al2(SO4)3. 18H2O, containing 125.0 mg is dissolved in 1.000 L of solution. Calculate the following for the solution: a The molarity of Al2(SO4)3. b The molarity of SO42. c The molality of Al2(SO4)3, assuming that the density of the solution is 1.00 g/mL.
The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?
The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?