1-3: A stock solution of 70% v/v ethanol was diluted with distilled water to prepare 1L of 21% v/v ethanol. (Density of ethanol =0.789 g/mL; MW of ethanol = 46 g/mol)1.Determine the initial volume of 70% v/v ethanol used in the preparation.2.How much water was added to the stock solution to make 1L of the final concentration?3.The molarity of 5.0 mL of 70% v/v ethanol was found to be4-6: A solution contains 45.0 g of methanol, CH3OH, dissolved in sufficient water to give a total mass of 210.6 g.4. Compute for the number of moles of the solute present in the given solution.5. What is the mass (in kg) of water used to dissolve the solute from the given problem?6. Determine the molal concentration of the said solution.5-7: A 10.34 molal aqueous nitric acid solution was prepared.(Density of nitric acid = 1.51 g/mL, density of water = 1.0 g/mL, and the MW of nitric acid = 63 g/mol)5. How many grams of HNO3 were used to prepare the solution?6. What is the Molarity of the solution?7. What is the concentration (%"/,) of the solution?

Answered: Image /qna-images/answer/9f1870e9-1335-4f1f-9514-4b5a18f2314c.jpg

1-3: A stock solution of 70% v/v ethanol was diluted with distilled water to prepare 1L of 21% v/v ethanol. (Density of ethanol = 0.789 g/mL; MW of ethanol = 46 g/mol) 1. Determine the initial volume of 70% v/v ethanol used in the preparation. 2. How much water was added to the stock solution to make IL of the final concentration? 3. The molarity of 5.0 mL of 70% v/v ethanol was found to be

1-3: A stock solution of 70% v/v ethanol was diluted with distilled water to prepare 1L of 21% v/v ethanol. (Density of ethanol = 0.789 g/mL; MW of ethanol = 46 g/mol) 1. Determine the initial volume of 70% v/v ethanol used in the preparation. 2. How much water was added to the stock solution to make IL of the final concentration? 3. The molarity of 5.0 mL of 70% v/v ethanol was found to be

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Need help, please.
INSTRUCTIONS: Solve the problems below. Show the necessary calculations. 1. Calculate the grams of the substance required in preparing 250 ml of 0.2 M sucrose. II. Calculate the molarity of 66.80 g of CaQ in 4.00 L of solution. II. Calculate the molarity of HCIO4, density = 1.242 g/ml, 75.8% HCIO4 by weight (w/w) IV. What volume of water will be added to 200 ml of a 0.5 M HCI solution to make the molarity 0.125? V. Express the concentration in percent (w/v) of 0.75 N CuSO4
Tags rosy) alcohol is mixed with water to produce a 37% (v/v) alcohal solution How many milliliters of each component are 745 ml. of this solution ? present mn те alcohol = me Water me.
The solubilities of three salts in water are shown in the graph. For each salt, determine how much will remain undissolved if 500 g is mixed into a liter of pure water at 40 °C. One significant figure is sufficient in each answer. Pb(NO3)2: KC1: K₂Cr₂O7: OD g 6.D Solubility (g/L) 1000 900 800 700 600 500 400 300 200 100 Pb(NO3)2 K₂Cr₂O, КСІ 0 10 20 30 40 50 60 70 80 90 100 Temperature (℃)
OMacmillan Learning Express the concentration of a 0.0160 M aqueous solution of fluoride, F, in mass percentage and in parts per million (ppm). Assume the density of the solution is 1.00 g/mL.. mass percentage: ppm: 30.4 Incorrect 0.0304 28 ppm
50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQ
Refer to the table. Identify unknown 1 based on the result. Unknown 1 is D Unknown 1 is C Unknown 1 is B Unknown 1 is A information is insufficient to identify unknown 1
A 575 mL sample of Pb(NO3)2 aqueous solution has a mass of 575.78 g. After the Pb(NO3)2 solution is evaporated to dryness, the dry salt has a mass of 27.5g of Pb(NO3)2. a. What is the solvent used and what could the mass of this solvent be? b. Calculate the % (m/m) concentration of solution c. Calculate the molarity (M)
An 7.50 ml aliquot of a 125 ppm stock Red 40 dye solution was diluted to a final volume of 25.0 mL with deionized water. What is the concentration of the dilute Red 40 dye solution (in ppm)? 37.5 ppm is the answer. (please show me how to calculate)
1. Make up 0.1 M solutions (100 ml) of Na2HPO4 (FW=177.99) and NaH2PO4 (FW=137.99) using a 100 ml volumetric flask. 2. First calculate the amount of each compound needed by using its formula weight. Weigh each compound out in its own 150 ml beaker, add 70-80 ml of water and stir until all the compound is dissolved
Answer number 1 to 3. I don't want to waste my money here
1. How many grams of pure H3PO4 are needed in the preparation of 250 mL of a 3.5 M solution of H3PO4? 1. How many ml of 86% w/w H3PO4 with a density of 1.71 g/ml are needed in the preparation of same volume of a 3.5 M solution of H3PO4? Please provide the GIVEN, REQUIRED TO BE SOLVED and the COMPLETE SOLUTION of the problems given above.