Lab. work Nacl is a chemical compound of a molecular mass =58.4 1- prepare 10 ml of one molar concentration NaCL. 2- from the solution above prepare 10 ml of 0.3 molar concentration. 3 write all your work stages in a scientific report. Chemicals and supplies: 1- NaCL. 2-Distilled water. 3-2 volumetric flasks of 10 ml volume, or 4-2 cylinders of 10 ml, volume. 5- funnel. 6- sensitive balance.

Lab. work Nacl is a chemical compound of a molecular mass =58.4 1- prepare 10 ml of one molar concentration NaCL. 2- from the solution above prepare 10 ml of 0.3 molar concentration. 3 write all your work stages in a scientific report. Chemicals and supplies: 1- NaCL. 2-Distilled water. 3-2 volumetric flasks of 10 ml volume, or 4-2 cylinders of 10 ml, volume. 5- funnel. 6- sensitive balance.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 86QRT

See similar textbooks

Similar questions

A solution labeled “0.25 M AICl3” would contain _________ le(s) of Al3+ and mole(s) of Cl- in each liter of e solution.
In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using the given information. a. 2.0 m KCl in water (density of H2O = 1.00 g/cm3) b. 15% NaOH by mass in water (d = 1.00 g/cm3) c. 25% NaOH by mass in CH3OH (d = 0.79 g/cm3) d. 0.10 mole fraction of C6H12O6 in water (d = 1.00 g/cm3)
NaOH Concentration (M): 0.09669M Trial 1: Inital Volume of NaOH: 0.55mL Final Volume of NaOH: 28.25 mL Trail 2: Intial Volume of NaOH: 18.1 mL Final Volume of NaOH: 46.1 mL Concentration of HCl Solution Subtract the initial buret reading from the end point reading. Convert the readings to liters by dividing by 1000. Solve this equation for the concentration of HCl: (CHCl) (0.01000 liters ) = (CNaOH) (volume of NaOH in liters). CNaOH is the normality of the NaOH you recorded from the bottle. Average the two HCl concentrations.
What volume (in mL) of 30.0% hydrogen peroxide solution is required to provide the mass required in question 8 above? Mass=10.2g of a 30% hydrogen peroxide soltuion. Density of 30.0% H2O2 = 1.11 g/mL Answer with 3 sig figs.
Consider a 1.000-L stock solution of 9.69 M Na3PO4. A 2.000-mL aliquot is taken from this stock solution and diluted to a final volume of 1.000 L. A 5.000-mL aliquot is then taken from this new solution and further diluted to make a new solution with a final volume of 750.0 mL. Calculate Na+ in the final solution.
Part 1: A solution of sulfuric acid was made by dissolving 20.0g of 98% sulfuric acid in 250mL of water. (H2SO4 = 98.078 g/mol; H2O = 18.015 g/mol)Answer these items 1-4 for part 1:1. Express the concentration of this solution in % by weight. Additional information for items 2-3: What if the solution has a total volume of 262mL?2. Express the concentration in molarity3. Express the concentration in normality4. Express the concentration in molality Part 2: An alcohol, Ethanol (C2H5OH), is present in 1L of wine that is 12% alcohol by volume. The density of the solution is 0.984 g/mL, and the density of pure alcohol is 0.789 g/mL. (C2H5OH = 46.07 g/mol)Answer these items 1-2 for part 2:1. What is the weight of the alcohol present in wine?2. What is the molarity of the solution?
Run 1 Run 2 Molarity of KMnO4 solution (M) from bottle 0.00101 0.00101 Initial reading of buret KMnO4 (mL) 0.62 11.35 Final reading of buret KMnO4 (mL) 11.33 21.70 Run 1 Run 2 Volume of KMnO4 solution (mL) Moles of MnO4- used for titration (mol) Moles of C2O42- in 100.0 mL of solution (mol) Molarity of C2O42- (M) Molarity of Cd2+ (M) Ksp of CdC2O4 Average Ksp of CdC2O4 Calculations: Moles of MnO4- used for titration of saturated solution CdC2O4 Moles of C2O42- in 100.0 mL of saturated solution of CdC2O4 Molarity of C2O42- in saturated solution of CdC2O4 Molarity of Cd2+ in saturated solution of CdC2O4 Solubility product, Ksp, of CdC2O4
A solution of sulfuric acid was made by dissolving 20.0g of 98% sulfuric acid in a 250mL of water. (H2SO4 = 98.078 g/mol; H2O = 18.015 g/mol)Additional information for 35-37 What if the solution has a total volume of 262ml? 1. Express the concentration of this solution in % by weight.a. 7.3%b. 4.4%c. 8.0%d. 7.8% 2. Express the concentration in molaritya. 0.10 Mb. 2.00 Mc. 0.76 Md. 0.93 M 3. Express the concentration in normalitya. 2.0 Nb. 1.5 Nc. 1.0 Nd. 0.76 N 4. Express the concentration in molalitya. 0.80 mb. 0.77 mc. 1.00 md. 1.50 m
CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) A laboratory is well-stocked with 1.0 M H2SO4 and 6.0 M H2SO4, but 500 mL of 2.5 M H2SO4 areneeded for an experiment. Unfortunately, the water supply has been temporarily cut off, so the 2.5M solution must be made from the existing solutions. How many milliliters of 1.0 M and 6.0 MH2SO4 must be mixed in order to prepare 500 mL of 2.5 M solution?
How much amount of solids (in grams) do you need to prepare the following solutions? 1. 500.0 mL 0.1000 M stock EDTA solutiona. Weigh an appropriate amount of Na2H2EDTA2H2O (FW=372.24) to the nearest 0.1 mg 2. 100.0 mL 0.0500 M stock Ca2+ solutiona. Weigh appropriate amount of pure CaCO3 (FW=100.09) to the nearest 0.1 mg into a 250 mL beaker.
1) 0.1% w/v = ? mg/100 ml? Only include the number and not any units 2) 0.1% = ? ug/ml? Only include the number and not any units 3) What is the concentration of your stock in ug/ml? Only include the number and not any units 4)The molecular weight of tartrazine is 534.4 g/mole. What is the concentration of your stock solution in mM? Be sure to give your answer in milliMolar to TWO decimal places. 5)What dilution of your stock do you need to get the first standard (100 ug/ml)? Express as 1:x, where x is the fold dilution needed.
1) 0.1% w/v = ? mg/100 ml? Only include the number and not any units 2) 0.1% = ? ug/ml? Only include the number and not any units 3) What is the concentration of your stock in ug/ml? Only include the number and not any units 4)The molecular weight of tartrazine is 534.4 g/mole. What is the concentration of your stock solution in mM? Be sure to give your answer in milliMolar to TWO decimal places. 5)What dilution of your stock do you need to get the first standard (100 ug/ml)? Express as 1:x, where x is the fold dilution needed. 6)What weight of tartrazine (in mg) would you need to make up 250 mL of a 2.5 mM solution (MW of tartrazine is 534.4 g/mole)? Give your answer to the nearest whole number. write the number only, not the units