==> NaHCO3(aq.) + NaCl(aq.) We will standardize the HCl solution to use it in the titration. The standardization will come as a result of the 1:1 molar ratio above. Thus, the molarity of the HCl solution can be calculated by dividing the number of moles of HCl by the volume of HCl (in liters) used to neutralize the Na2CO3 .
What is the volume of object 1? ______ 14.0 cm3 _______________________ Note: While milliliters (mL) are used to measure liquid volumes, the equivalent unit cubic centimeters (cm3) are used for solids. Therefore, write the volume of object 1 in cm3. Drag object 1 into the Beaker of Liquid. Does it sink or float?
0.0625mol/0.125M=0.5L=500mL Calculation for preparing the EDTA solution Exercise 6 a. 1L*0.02M=0.02mol 0.02mol*372.24g/mol=7.4g EDTA b. Exact molarity of 7.4448g /1.00L would be .0200 M Exercise 7 a. 0.5M*100*10-3L=0.05mol acetic acid b. 0.05mol/6M=8.3*10-3 L=8.3mL stock solution c. 100mL-8.3mL=91.7mLwater Add 91.7 water to 6M stock solution to prepare 0.5M acetic acid.
In the Pledges worksheet, create an Excel table with the Medium 7 table style using data in the range A1:H29. Rename the table as PledgeData. 4. Make a copy of the Pledges worksheet, and then rename the copied worksheet as Q4-6 (for “Question 4-6”). (Hint: Press the Ctrl key and drag the sheet tab to the right of the Pledges sheet tab to make a copy of the worksheet.)
Subtract the weight of the funnel and the filter paper from this weight to get the weight of the precipitate Results: wt. of filter paper | wt. of empty funnel | mL of NaOH | wt. of funnel with Zn(OH)2 | wt. of penny | wt.
Table of Contents/Labs Lab # | Title | Page | | Informal Lab Report Procedures & Grading Rubric | 2-4 | 1 | How Many Drops Of Water Can Fit On A Penny? | 5-6 | 2 | Is The Potassium Chloride Mixture Homogeneous or Heterogeneous? | 7 | 3 | What Are The Densities Of Pre- And Post-1982 Pennies? | 8 | 4 | Which Type Of Glassware Is Most Accurate? | 9 | 5 | What Is The Relative Abundance Of Pre- And Post-1982 Pennies In A Sample of 1982 Pennies?
Pre-Lab Questions 1. A determination of the molar mass of methyl alcohol (CH3OH) yielded the following data. Temperature of boiling water bath 99.5o C Barometric pressure 738 mm Hg Temperature of room temperature water 24.0o C Density of room temperature water 0.9973 g/mL Trial 1 Mass of empty pipette 1.557g Mass of piet and condensed methyl alcohol 1.571g Mass of pipet and water 16.001g Mass of condensed methyl alcohol 0.014g Mass of water in filled pipet 14.444g Volume of pipet 14.483mL Molar mass of methyl alcohol (experimental) 28.69 g/mol Molar mass of methyl alcohol (theoretical) 32.05 g/mol Using the data, fill in the rest of the table. The volume of the pipet is equal to the volume of water inside the pipet. Use the relationship of mass and density to determine this volume.
Calculate the mass of KCl required to prepare 250. mL of 0.250 M solution. 3. Calculate the volume of 0.30 M KCl solution that contains 6.00 g of KCl. 6.00 g x 1 mole x 1 L = 0.27 L 74.6 g 0.30 mol 4. Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4.