Mass of Erlenmeyer Flask (g) 24.33 24.37 24.44 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (g)   (g)(lime water) 27.22 27.29 27.33 Mass of Calcium Hydroxide Solution (g) 2.89 2.92 2.89 Volume of Ca(OH)2 Density = 1.000 g/mL 2.89 2.92 2.89 Concentration of HCl (M) 0.1 0.1 0.1 Initial HCl Volume in Syringe (mL) 1.00+1.00 1.00+1.00 1.00+1.00 Final HCl Volume in Syringe (mL) .72 .66 .54 Volume of HCl Delivered (mL) 1.28 1.34 1.46 Moles of HCl Delivered

3 Dilution is a process in which the concentration of a solution is lowered by adding more solvent. Some of the reasons dilutions are performed are to minimize measurement errors when preparing a series of solutions at different concentrations, to save time and laboratory space, and to make more accurate measurements on an analytical balance when the target concentration is very low. The new concentration of a diluted solution can be determined from the following equation, sometimes called the dilution equation, Y M₁ V₁ = M₂V₂ where M₁ is the concentration of the initial solution, V₁ is the volume of the initial solution, M₂ is the concentration of the final solution, and V₂ is the volume of the final solution. The terms M₁ and M₂2 are often expressed in molarity, M, which is equal to mol/L. Another way to write the equation is to replace subscripts of 1 and 2 with abbreviated notations representing concentrated and diluted, as follows: E Meone Veone Mail Vail Based on the inverse…

Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask (g) 24.33 24.37 24.44 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (g)   (g)(lime water) 27.22 27.29 27.33 Mass of Calcium Hydroxide Solution (g) 2.89 2.92 2.89 Volume of Ca(OH)2 Density = 1.000 g/mL 2.89 2.92 2.89 Concentration of HCl (M) 0.1 0.1 0.1 Initial HCl Volume in Syringe (mL) 1.00+1.00 1.00+1.00 1.00+1.00 Final HCl Volume in Syringe (mL) .72 .66 .54 Volume of HCl Delivered (mL) 1.28 1.34 1.46 Moles of HCl Delivered       Moles of OH- in Sample       Moles of Ca2+ in Sample       Molar Solubility (M)       Calculated Ksp       Average Calculated Ksp       I am very confused how to solve the blank spots in the table. Everything including and after "Moles of HCl Delivered" confuses me. Please help me figure out how to solve the sections correctly. Also feel free to…

A & B

H8.

You have three sodium carbonate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M sodium carbonate.Solution 1 contains 100.0 mL of the 3.00 M solution.Solution 2 contains 50.0 mL of the 3.00 M solution.Solution 3 contains 10.0 mL of the 3.00 M solution.What volume of water (in mL) must evaporate from Solution 1 in order to have a concentration of 4.88 M?

What is the average?

What is the volume of 1.80 M NaCl solution that can be prepared by the dilution of a 50.0 mL of brine solution containing 32.0 wt% NaCl? (Assume the density of a brine solution is 1.10 g/mL and formula mass of NaCl=58.4 g/mol) a. 6.03 mL b. 167 mL C. 301 mL d. 438 mL

1. In the laboratory, a student dilutes 12.8 mL of a 11.9 M hydroiodic acid solution to a total volume of 125.0 mb What is the concentration of the diluted solution? Concentration = M 2. How many milliliters of 10.3 M hydroiodic acid solution should be used to prepare 2.50 L of 0.600 M2 mL 3. In the laboratory, a student adds 54.8 mL of water to 23.5 mL of a 0.896 M hydroiodic acid solution. What is the concentration of the diluted solution? Assume the volumes are additive. Concentration = I M

mol 702.7 mol ÷ 0.31 L %3D L 614.9 m ÷ 62.4 s = g 20.947 mL х 26, mL E