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- 2. Calculate the [I] (after dilution in the 50.00 mL flasks) for the four standard solutions you make up in part B. Use the data given in Table B and show all calculations. Round your answers to the correct number of significant figures. Record these values on the spreadsheet template before the lab.The equivalent conductance of a 0.0140N solution of chloroacetic acid is 109.0 at 25 degrees C. What is the ionization constant (Ka) of chloroacetic acid?6. If molar conductivity of HCl solution at 25° C is 425 Scm? mol'at infinite dilution. The specific conductance is 3.824 Scm", if degree of dissociation is 90%, what is the concentration of the solution? a) 1 mol/L c) 0.10 mol/L e) 0.9 mol/L b) 10 mol/L d) 0.8 mol/L
- What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving 0.637mol0.637mol CuCl2 in water and diluting to 289mL?289mL? What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving CuCl2 in water and diluting to 0.454 and 0.092 2.20 and 2.20 2.20 and 4.41 0.00220 and 0.00220 0.00220 and 2.20A solution of HCl was titrated against sodium carbonate. What is the average normality of acid in the given data? (MW Na₂CO3 = 106) T2 0.3479 0.3562 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (mL) Vol HCl used (mL) 35.10 39.40 N of HCl (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)According to the table below answer the following question: Salt pair NaC KC NaNO 3 KNO 3 Equivalent Conductance (mho cm Vequiv) 108.90 130.10 105.33 126.50 KBr 132.30 NaBr is ? 143.8 106.7 153.5 111.10
- For weak electrolytes, such as acetic acid, at very low concentrations the molar conductivity drops rapidly as the concentration increases. However, at higher concentration, there’s only a slight decrease in the molar conductivity. True False?Which statement is correct about a strong electrolyte It is partially ionized in aqueous solution. .a O The molar conductivity at infinite dilution can be found by extrapolation from a plot of molar conductivity .b O against concentration. Examples of strong electrolytes include CH3CO2H and Na[CH3CO2]. .c O The molar conductivity decreases significantly as the concentration increases. .d OA D E Which of the figures above represents how you expect the conductivity of an aqueous solution of SDS (CH3(CH2)110SO3Na) to vary with concentration. (The y-axis is the conductivity and the x-axis is concentration in each case above.)
- The distribution constant for solute Z. between Water is 3.7. Calculate the remaining consentration of 2. remaining in a solution when 0.036 M and 31 ml. aparous solution of A is extracted with 4 portions of 8 ml. hexane AY 7.28 x 10M B ) 7.37 x 10M C) 148 x 10M D) 2.61 x 10M E ) 1.87 x 10M9. The molar conductivity values at infinite dilution, in units of Sm?mol1, of NHẠCI, NaCl and N2OH are 1.497 x 10², 1.2645 x 10² and 2.478 x 10², respectively. (a) Calculate the molar conductivity at infinite dilution of NH4OH. (b) The molar conductivity of 0.0100 moldm3 NH,OH is 1.13 x 103 Sm?mol. What is the degree of dissociation and the dissociation constant, Kp, of 0.0100 moldm3 NHẠOH?Q3. (i) Write a note on following effects with examples for strong electrolytes (a) Asymmetry affect (b) viscous effect (ii) How ion pairs are formed in the solution. As a result ofion pair formation which properties of the solution are affected