Part A a solution that is 0.19 M in HCHO2 and 0.13 M in NaCHO2 (Ka(HCHO2) = 1.8 × 10-4) Express your answer to two decimal places. ΑΣφ ? pH Submit Request Answer Part B a solution that is 0.16 M in NH3 and 0.17 M in NH, Cl (Kp (NH3) = 1.76 × 10–5) Express your answer to two decimal places. | ν ΑΣφ ? pH = Notes
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- A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture. Note: include up to 4 decimal places Please explain each stepUsing Equation 5.9, show that three extractions with 5-mL portions of a solvent give better recovery than a single extraction with 15 mL of solvent when K =0.5.An analyte has a Rf value of 1. What does that say about the solubility of the analyte in the mobile phase as compared to the stationary phase? (please show me all steps)
- How much amount (in grams) do you need to prepare the following solutions 500.0 mL 0.1000 M stock EDTA solution from Na2H2EDTA•2H2O (FW=372.24) and MgCl2•6H2O crystals 100.0 mL 0.0500 M stock Ca2+ solution from pure CaCO3 (FW=100.09) and concentrated HCl 250 mL 1.0 M NH3-NH4+ pH 10 buffer solution from NH4Cl and NH31. Why is there a need to correct conductivity of the sample solution?2. Cite three possible sources of error in the experiment and discuss their effects on the computed ionization constant of the acetic acid. (See details below----- literature value- Ki, acetic acid= 1.75 x 10^-5). 3. What is the effect of dilution on the fraction of the acetic acid ionized?How would your calculation of the Molarity of KMnO4 have been affected (Higher, Lower, No Change) if . . . you recorded the endpoint volume and then noticed that the color had faded . . . . you did not add more KMnO4 solution? you were unable to complete the 3rd Trial and stored your KMnO4 solution in your desk for 3 days before completing the 3rd titration with the stored solution? you had added twice as much sulfuric acid as was called for in the procedure?
- The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.ALL INFORMATION NEEDED IS PROVIDED, I NEED FIRST QUESTIONS ANSWERED FIRST BEFORE OTHERS CAN BE ANSWEREDRate = -(Delta[RCl])/Delta t andln[RCl]t=-k*t+ln[RCl]0 < [R-Cl]-time equation Test tube A = 0.30 of 0.10M NaOH(aq), 6.70ml DI H2O & 1 drop of bromophenol bue Test Tube B = 3.00M of 0.10M R-CL in acetone. Mix together in 3 water baths Bath A Trial 1= 20C, 53.6s Trial 2= 20C, 49s for color to changeBath B Trial 1= 32C, 18s Trail 2= 32C, 20s Bath C Trial 1= 10C, 204s Trial B= 10C, 200s average out both trials for each bathcolor change happens after 10% of R-Cl has reacted so In terms of R-Cl this means that 10% of the R-Cl has reacted and ____ of the R-Cl is left Q1. at the time of the color change [R-Cl]t=____[R-Cl]o (Fill in the blank) Q4. Substitute the value of [R-Cl]t into appropriate equation listed above and solve for k in terms of [R-Cl] and t. Q5. Use average time for each temp and determine the value of k (with units) at each temperature Q6. Rearrange the Arrhenius…
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