utions Procedure: 1. Prepare 50 mL of a 0.100 M solution of LiCl. 2. Using this stock solution, prepare a series of solutions (20 mL each) with the following concentrations: 0.0500 M, 0.0250 M, 0.0125 M, and 0.00625 M. The dilutions should leave-30 mL of the 0.100 M stock solution to finish the series. (Note that each solution in the series is ½ the concentration of the previous solution.) 3. Using the information in the tables below, plot conductivity (mS cm') vs. concentration (mol/L) using Excel (or other plotting software) and apply a linear regression analysis to the plot. 4. Repeat steps 1-3 for formic acid. LICI Formic Acid mS cm 10.66 mol/L 0.10000 ms cm mol/L 1.79 0.10000 7.75 6.30 5.57 0.05000 1,60 0.05000 0.02500 0.01250 1.50 0.02500 1.45 0.01250 5.21 0.00625 1.43 0.00625 Questions: 1. Determine the mass of LICI (42.394 g/mol) required for Step 1. 2. Show your calculations for the volume of 0.100 M LịCI required for each dilution in Step 2. (HINT: dilution law: M,V; = M¿V2) 3. Submit your two clearly labeled plots (including their lincar fits) from Excel (or other plotting software). There is a short video on D2L on how to plot using Excel. 4. Which compound is the stronger electrolyte? What do you believe to be the major factor accounting for the difference?

NaHCO3 (aq) + CH3 COOH (aq) —> CO2 (g) + H2O (l) + CH3 COONa (aq)   Calculate the molar concentration of 100ml of vinegar (CH3COOH) and 2.5 ml of baking soda (NaHCO3). Note that the concentration of table vinegar is about 1 mol/L and the density of baking soda is 2.2 g/cm3

Convert the following pH or pOH values to [H*] or [OH] concentration Example: pH = 7.0, [H*] = 1.0 x 10-7 M pH = 5.3, [H*] = РОН 3 11.1, [Н']]- РОН 3 6.6, [ОН]- pH = 2.5, [OH]] = In two or three sentences, compare and contrast the Bronsted-Lowry definition of acids/bases and the Arrhenius definition. What are the similarities and differences? Complete the acid-base equation, providing the missing species. Under each species, write A, B, CA, or CB for acid, base, conjugate acid, or conjugate base, respectively. H2O + HCO3 + H3O*

ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?

Consider each chemical equation and select all that represent a chemical reaction.     2NaI(aq)  +  Pb(NO3)2(aq)  →  2NaNO3(aq)  +  PbI2(s)     2KBr(aq) + MgCl2(aq) → 2KCl(aq) + MgBr2(aq)     HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Match each pollutant with their final product in our atmosphere. > SO₂ NO₂ CO CH4 1. CO2 2. H₂SO4 3. HNO3

In one experiment, 0.150 L of SnCl4 (d = 2.226 g/mL) was treated with 0.323 L of triethylaluminum (Al(C2H5)3); d = 0.835 g/mL).What is the theoretical yield in this experiment (mass of tetraethylstannane, Sn(C2H5)4)?

7) The most important reaction that allows our cars to do work is octane (CSH18) combustion 2 C8HI8 + 25 02 à 16 C02 + 18 H20 a) Theoretically speaking, if we fully combust 3.0 kg of octane, and keep the products at STR, what volume of gas do we expect to be produced? b) If the % yield for this combustion reaction is 90%, what is the actual volume? 8) Name two characteristics that describe real gases and not ideal gasses. 9) a) A climber takes a mole of ideal qgas to the top of Mount Everest, where the pressure is 304 torr and the temperature is subzero at -17° C. What is the volume of the gas? b) The gas taken to Mount Everest is oxugen gas. What is the root mean square velocity of gas molecules in that sample of gas? 10.) a) An 8.00L tank at 7.3° C is filled with 24 g of dinitrogen monoxide (N2O) and 8.2 g of sulfur hexafluoride gas (SF6). What is the mole fraction of sulfur hexafluoride? b) What is the ratio between the rates of effusion of sulfur hexafluoride and dinitrogen…

I have 3.025 lb H2SO4 and 200 gal of water.  How many molecules of sulfuric acid do I have?  What is the pH? All hydrogen atoms convert to hydronium ions. 1 oz= 28.35 g 1 gall=3.785 L

Answer With Work Shown Please . 1. CaO + H2O → Ca(OH)2 If you start with 2400 g of CaO, add excess water, and produce 2060 g of Ca(OH)2, what is the percent yield of the reaction? 2.Draw the Lewis dot structure of SiCl4 then determine if the molecule has polar bonds and if it is a polar or non-polar molecule. 3.If you have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 870C, how many moles of gas do I have? R=0.0821 L*atm/K*mol