![3. Use the provided experimental data to calculate the equilibrium constant, Ke, for the reaction given below. (7) Co3(ag)SCN (ag)CoSCN (ag) Ke-? initial concentration of Co», 1.0 × 10-3 M initial concentration of SCN: 5.0 x 10-4 M absorbance of the equilibrium mixture at 491 nm: 0.167 trendline equation for the [CoSCN2+] calibration curve: y (4.2 x 103)x +0.0074 What, if anything, will happen to saturated PbBr2 solution if more Br ions are added to the solution? Explain your answer. (4) 4. sp Write the expression for the solubility product, Ksp of PbBr2.(2) 5. K, sp](http://img.homeworklib.com/questions/d429f620-9a08-11eb-90ce-2532d367a077.png?x-oss-process=image/resize,w_560)
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3. Use the provided experimental data to calculate the equilibrium constant, Ke, for the reaction given...
3. Use the provided experimental data to calculate the equilibrium constant, K, for the reaction given...
3. Use the provided experimental data to calculate the equilibrium constant, K, for the reaction given below. Note the stoichiometry is not all 1 to 1. (7) Include the units for K Ke=? Co3+(aq) + 2SCN-(aq) = Co(SCN)2(aq) 5.0 ml of 0.10 M CO(NO3)3 was mixed with 5.0 ml of 0.050 M KSCN The absorbance of the equilibrium mixture at 491 nm was 0.157. The linear regression equation for the (Co(SCN)2-) calibration curve was: y = (4.3 x 103)x +...
4. If more Br ions are added to a saturated PbBr solution, will the reaction shift?...
4. If more Br ions are added to a saturated PbBr solution, will the reaction shift? If so, which direction? Explain why or why not (4) PbBry(s) Pb2+ (aq) + 2 Brjag) 5. Write the expression for the solubility product, Kp. of PbBr2 (2) 3. Use the provided experimental data to calculate the equilibrium constant, K, for the reaction given below. Note the stoichiometry is not all 1 to 1. (7) Include the units for K Collaq) + 2SCN (aq)...
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solut...
Determination of the equilibrum constant
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solution A. Preparation of the Calibration Curve Concentration of Fe(NO,), in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO, solution Y Y Flask Number 2 Volume of NaSCN, mL Solution Initial [SCN 1.M Equil. [FeNCs". M Percent T Absorbance B. Determination of the Equilibrium Constant Concentration of Fe(NO,) in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO,...
Write the expression for the equilibrium constant for the following reaction, Fe+3 (aq) + SCN- (aq)...
Write the expression for the equilibrium constant for the following reaction, Fe+3 (aq) + SCN- (aq) ↔ Fe(SCN) +2 (aq) The slope of the calibration curve of [Fe(SCN)+2] vs absorbance is 3.5 x 104 M-1. Given that the absorbance of the solution prepared using 5.0 mL from 0.002 M Fe+3 and 3.0 mL from 0.002 SCN- is 0.422. Calculate the equilibrium constant for this solution.
If the original sodium tartrate solution had a concentration of 1.00 M instead of 0.100 M,...
If the original sodium tartrate solution had a concentration of
1.00 M instead of 0.100 M, what would the concentration of copper
be in a solution created by combining 10 mL of it with 10 mL of the
0.100M copper (II)sulfate solution. Use the Ksp you found in the
experiment.
For the ionic solid copper tartrate, the solubility equilibrium
reaction is: CuC4H4O6 (s) Cu2+ (aq) + C4H4O6 2- (aq) Just like any
equilibrium reaction, an equilibrium expression can be created....
The experimental data needs to be made up using these instructions. Sample Data - Determination of...
The experimental data needs to be made up using these
instructions.
Sample Data - Determination of a Solubility Product Constant Data For each titration trial, pick values that fall within the ranges given. Choose different numbers for Trials 1 and 2. Concentration of standard HCl solution (M): 0.050 Initial burette reading (ml): 1.00-2.00 Final burette reading (ml): 12.00-13.50 Volume of HCl added (mL): calculated Solution temperature (°C): 25.0 Complete the remaining calculations based on your entered data. Determination of a...
values used for table 2 how do you do the Ice tables??? Experiment V. Equilibrium Constant...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred)...
For each equilibrium sample, calculate the initial
concentrations (assuming no reaction occurred) of SCN–
and Fe3+ based on the dilution factors used.
Enter the absorbance values for each sample.
For the standard solution, assume that, when equilibrium is
reached, the [FeSCN2+]eq is equal to
[SCN–]ini. Why is this a good
assumption?
For the equilibrium solutions, calculate the
[FeSCN2+]eq (Ceq) using Eq.
4.
Using Eq. 5 and 6, calculate
[Fe3+(aq)]eq and
[SCN–(aq)]eq for each equilibrium
solution.
Calculate values for the equilibrium...
1. The solutions below were mixed together to carry out the iodination of acetone at 250 °C. 5.0 mL of 3.4 M acetone...
1. The solutions below were mixed together to carry out the iodination of acetone at 250 °C. 5.0 mL of 3.4 M acetone 5.0 mL of 12 M HCl solution 100 ml. of 0.0074 M l solution 5.0 mL of DI HO If the reaction took 516 seconds to go to completion, then what is the value for the rate constant, k, for the reaction at 250 °C? The initial reaction rate is equal to the average reaction rate for...
answer these please 17. The solubility of AgCl is 0.000 013 mol/L. Calculate the Ksp for...
answer these please
17. The solubility of AgCl is 0.000 013 mol/L. Calculate the Ksp for AgCl. 18. If the concentration of chloride ion remaining in solution after silver chloride has been precipitated is 0.2 M, what is the concentration of the silver ion? Kap of AgCl is 2.8 X 10-10 19. What is the experimental Ksp of CaCO3 if the residue after evaporation of a 1.00 L saturated solution is found to have a mass of 0.006 90 g?...
3. Use the provided experimental data to calculate the equilibrium constant, K, for the reaction given below. Note the stoichiometry is not all 1 to 1. (7) Include the units for K Ke=? Co3+(aq) + 2SCN-(aq) = Co(SCN)2(aq) 5.0 ml of 0.10 M CO(NO3)3 was mixed with 5.0 ml of 0.050 M KSCN The absorbance of the equilibrium mixture at 491 nm was 0.157. The linear regression equation for the (Co(SCN)2-) calibration curve was: y = (4.3 x 103)x +...
4. If more Br ions are added to a saturated PbBr solution, will the reaction shift? If so, which direction? Explain why or why not (4) PbBry(s) Pb2+ (aq) + 2 Brjag) 5. Write the expression for the solubility product, Kp. of PbBr2 (2) 3. Use the provided experimental data to calculate the equilibrium constant, K, for the reaction given below. Note the stoichiometry is not all 1 to 1. (7) Include the units for K Collaq) + 2SCN (aq)...
Determination of the equilibrum constant
REPORT SHEET EXPERIMENT Colorimetric 22 Determination of an Equilibrium Constant in Aqueous Solution A. Preparation of the Calibration Curve Concentration of Fe(NO,), in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO, solution Y Y Flask Number 2 Volume of NaSCN, mL Solution Initial [SCN 1.M Equil. [FeNCs". M Percent T Absorbance B. Determination of the Equilibrium Constant Concentration of Fe(NO,) in 0.10 M HNO, solution Concentration of NaSCN in 0.10 M HNO,...
If the original sodium tartrate solution had a concentration of
1.00 M instead of 0.100 M, what would the concentration of copper
be in a solution created by combining 10 mL of it with 10 mL of the
0.100M copper (II)sulfate solution. Use the Ksp you found in the
experiment.
For the ionic solid copper tartrate, the solubility equilibrium
reaction is: CuC4H4O6 (s) Cu2+ (aq) + C4H4O6 2- (aq) Just like any
equilibrium reaction, an equilibrium expression can be created....
The experimental data needs to be made up using these
instructions.
Sample Data - Determination of a Solubility Product Constant Data For each titration trial, pick values that fall within the ranges given. Choose different numbers for Trials 1 and 2. Concentration of standard HCl solution (M): 0.050 Initial burette reading (ml): 1.00-2.00 Final burette reading (ml): 12.00-13.50 Volume of HCl added (mL): calculated Solution temperature (°C): 25.0 Complete the remaining calculations based on your entered data. Determination of a...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
For each equilibrium sample, calculate the initial
concentrations (assuming no reaction occurred) of SCN–
and Fe3+ based on the dilution factors used.
Enter the absorbance values for each sample.
For the standard solution, assume that, when equilibrium is
reached, the [FeSCN2+]eq is equal to
[SCN–]ini. Why is this a good
assumption?
For the equilibrium solutions, calculate the
[FeSCN2+]eq (Ceq) using Eq.
4.
Using Eq. 5 and 6, calculate
[Fe3+(aq)]eq and
[SCN–(aq)]eq for each equilibrium
solution.
Calculate values for the equilibrium...
1. The solutions below were mixed together to carry out the iodination of acetone at 250 °C. 5.0 mL of 3.4 M acetone 5.0 mL of 12 M HCl solution 100 ml. of 0.0074 M l solution 5.0 mL of DI HO If the reaction took 516 seconds to go to completion, then what is the value for the rate constant, k, for the reaction at 250 °C? The initial reaction rate is equal to the average reaction rate for...
answer these please
17. The solubility of AgCl is 0.000 013 mol/L. Calculate the Ksp for AgCl. 18. If the concentration of chloride ion remaining in solution after silver chloride has been precipitated is 0.2 M, what is the concentration of the silver ion? Kap of AgCl is 2.8 X 10-10 19. What is the experimental Ksp of CaCO3 if the residue after evaporation of a 1.00 L saturated solution is found to have a mass of 0.006 90 g?...
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