Homework Answers
Concentration of I2 in CHCl3 = 0.00102
Concentration of I2 in H2O(aqeous) = 0.000112
Distribution constant = 0.00102/0.000112 = 9.107
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To determine the equilibrium constant for the reaction 12 +2SCNI(SCN)2 I 25.0 mL of a 0.0100...
In a hypothetical experiment, a student performs an extraction by shaking 25.0 mL mineral oil with...
In a hypothetical experiment, a student performs an extraction by shaking 25.0 mL mineral oil with 50.0 mL of 1.00 M I2 aqueous solution. After allowing the layers to separate the student observes that the mineral oil layer has become purple in color, indicating that some of the I2 has been transferred from the aqueous layer to the mineral oil layer. The student then removes the aqueous layer and titrates it with 5.00 mM Na2S2O3 solution. At the endpoint of...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the intial concentration of the SCN- f...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to...
Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to 50.0 mL, what is the concentration of Fe^+3 in the diluted solution? 2) Write the equilibrium for the following reaction. Co^+2 +4SCN^-1 <--> Co(SCN)4 ^-2 3) How many mmoles of SCN^-1 ion are there in 3.0 mL of 0.00200 M KSCN?
A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI.
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.
44. A 25.0 mL sample of a 0.100 M solution of aqueous trimethylamine is titrated with...
44. A 25.0 mL sample of a 0.100 M solution of aqueous trimethylamine is titrated with a 0.125 M solution of HCI. What is the pH of the solution after 10.0, 20.0 and 30.0 mL of acid have been added? Acids К. Acetic 1.76 x 105 Bases Кь Ammonia Methylamine Dimethylamine Trimethylamine 1.76 x 10 4.4x 104 5.9 x 104 6.46 x 105 Salts Кар 3.3 x 108 PbF2 PbCl2 1.7 x 10 5.3 х 10° CaF2
I need help with calculating the missing spots in the table below: Mix 10.0 mL of...
I need help with calculating the missing spots in the table below: Mix 10.0 mL of NaOH with 25.0 mL of HX. Stir to mix thoroughly. Measure the pH and temperature of this solution. Before mixing, [HX] 1.02 M Before mixing, [NaOH] 1.04 M Temperature 20.0 c Concentration of Unreacted [HX] M Concentration of [X-] after reaction pH of solution 4.47 Equilibrium Concentration [HX] M Equilibrium Concentration [X-] M Equilibrium Concentration [H3O+] M Ka
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2....
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2. In part A of Experiment 34, it was assumed that all of the SCN added to the reaction mixture was converted to product (FeNCS). Which of the following best explains why that assumption was valid? A) The moles of Fe added equaled the moles of SCN- added. B) In part A, the SCN was the limiting reactant whereas in part B,...
Determine the equilibrium concentration of FeSCN2+ in each solution. (Page below are the initial concentrations of...
Determine the equilibrium concentration of FeSCN2+ in each
solution. (Page below are the initial concentrations of FE3+ and
scn- for each solution )
Secondly, use stoichiometry to determine equilibrium FE3+ and
SCN -. ( concentration used for FE and KSCN are both 0.002M )
the absorbance of each standard in the same test tube used to blank the spectrophoto standards from least to most concentrated, rinsing with a small amount of the next sta tilling the test tube. Record absorbance...
Titration of Strong acid with strong base 2. Consider the titration of 25.0 mL of 0.100...
Titration of Strong acid with strong base 2. Consider the titration of 25.0 mL of 0.100 M HCI with 0.100 M NaOH. a) Write down the chemical equation. Hellmunt Hell Hotele lua b) Calculate the volume of NaOH required to reach the equivalence point. Rome 250ML 0.25 0. In 2008 was x I c) Calculate the initial pH of the acid solution. (before adding NaOH). pol of Helin 0.1ac plte -log [ol 1] d) Calculate the pH after adding 5.00...
56,57,58,59,60,61,62 56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [...
56,57,58,59,60,61,62
56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [NHs] 7.62 M 57) When a sample of aqueous hydrochloric acid was neutralized with aqueous sodium hydroxide in a calorimeter, the temperature of 100.0 g of water surrounding the reaction increased from 25.0°C to 31.50. If the specific heat of water is 1.00 calV(g.°C), calculate the quantity of energy in calories involved...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
44. A 25.0 mL sample of a 0.100 M solution of aqueous trimethylamine is titrated with a 0.125 M solution of HCI. What is the pH of the solution after 10.0, 20.0 and 30.0 mL of acid have been added? Acids К. Acetic 1.76 x 105 Bases Кь Ammonia Methylamine Dimethylamine Trimethylamine 1.76 x 10 4.4x 104 5.9 x 104 6.46 x 105 Salts Кар 3.3 x 108 PbF2 PbCl2 1.7 x 10 5.3 х 10° CaF2
I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2. In part A of Experiment 34, it was assumed that all of the SCN added to the reaction mixture was converted to product (FeNCS). Which of the following best explains why that assumption was valid? A) The moles of Fe added equaled the moles of SCN- added. B) In part A, the SCN was the limiting reactant whereas in part B,...
Determine the equilibrium concentration of FeSCN2+ in each
solution. (Page below are the initial concentrations of FE3+ and
scn- for each solution )
Secondly, use stoichiometry to determine equilibrium FE3+ and
SCN -. ( concentration used for FE and KSCN are both 0.002M )
the absorbance of each standard in the same test tube used to blank the spectrophoto standards from least to most concentrated, rinsing with a small amount of the next sta tilling the test tube. Record absorbance...
Titration of Strong acid with strong base 2. Consider the titration of 25.0 mL of 0.100 M HCI with 0.100 M NaOH. a) Write down the chemical equation. Hellmunt Hell Hotele lua b) Calculate the volume of NaOH required to reach the equivalence point. Rome 250ML 0.25 0. In 2008 was x I c) Calculate the initial pH of the acid solution. (before adding NaOH). pol of Helin 0.1ac plte -log [ol 1] d) Calculate the pH after adding 5.00...
56,57,58,59,60,61,62
56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [NHs] 7.62 M 57) When a sample of aqueous hydrochloric acid was neutralized with aqueous sodium hydroxide in a calorimeter, the temperature of 100.0 g of water surrounding the reaction increased from 25.0°C to 31.50. If the specific heat of water is 1.00 calV(g.°C), calculate the quantity of energy in calories involved...
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