You have prepared a solution using 2.08 g of NaOH (M.W.=40.00 g/mole) and 2.54 moles H2O(MW 1 =18.02g/mole), resulting in a solution of density 1.05g/mL Use this information to complete the table

What is the %v/v of a solution made from 231.1 g of ethylene glycol (density is 1.11 g/mL) in water (density 1.00 g/mL) to form a total volume of 500.0 mL

Calculate the volume of stock glucose solutions (2.5 % and 15%) that need to be used to prepare 800 mL of glucose solution with a concentration of 13%. In this case % refers to the grams of glucose per 100 mL of water. V1= volume of stock solution with concentration C (2.5%) V2= volume of stock solution with concentration C2 (15 %) You need to determine V, and V2 in mL

What is the molarity of a solution prepared by dissolving 317 g of CaCI2 into enough water to make 2.50 L of solution? ( MW CaCI2= 110.98 g/mol)

What is the freezing point, in °C, of a solution made with 1.56 mol of CHCI3 in 530.0 mL of solution? The solvent is CCI4 which has a Kf = 29.8 °C/M and a normal freezing point, Tf = -22.9 °C. Provide your answer to 1 decimal point.

50.00 ml of 0.120 mol/L MgSO4 solution is made to be using MgSO4. 7H2O, which has a molar mass of 246.47 g/mol.  a. How many moles of solid MgSO4. 7H2O are required?

Given a concentration of a solution, determine the amount of solute. a) Percent weight to weight is the ratio of the mass of solute to the mass of the entire solution. A 5.00% (w/w) aqueous sodium chloride solution has 10.0 g solution. g of NaCl in a b) Percent volume to volume is the ratio of the volume of solute to the volume of the entire solution. > mL of ethanol per glass (250.0 A beer that is 2.50% (v/v) alcohol has mL) of beer. c) Percent weight to volume is the number of grams of solute in 100 mL of the solution. A 5.00% (w/v) of aqueous glucose has g of glucose in 150.0 mL of solution.

A solution is prepared by dissolving 155.0 mL of methanol (CH3OH, density = 0.791 g/mL) in 250 mL of water (density 1.00 g/mL) to give a final solution volume of 350.0 mL. Calculate the (a) molarity of the solution, (b) %wt/wt, (c) %wt/vol, (d) %vol/vol

A copper(II) sulfate solution is 14.0% CuSO4 by mass. It is simultaneously 1.01 M at 20 °C. (a) Compute the density of this solution. Density= 8 cm-3 (b) What volume of this solution should be used in preparing 1.44 L of a 9.60×10-² M copper(II) sulfate solution? Volume mL