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B. Determination of the Solubility Product Constant: %T Absorbance [Cr0221 use equation A = 2 -...
help please? this was the only other information given REPORT SHEET Determination of the Solubility-Product Constant...
help please?
this was the only other information given
REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
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,...
please and thank you! Volume of K2Cr04 (mL) Absorbance Molar concentration of CrO42- (M) 2.4 x...
please and thank you!
Volume of K2Cr04 (mL) Absorbance Molar concentration of CrO42- (M) 2.4 x 10-5 1.00 0.89 5.00 1.2*10^-4 0.55 10.00 2.4*10^-4 0.99 15.00 3.6*10^-4 1.37 QUESTION 3 10 points Save Answer Upload the plot of the standard curve. Use excel to construct it. Label the axes and draw the linear relationship. Show the equation of the line on the plot (at the top right away from the data points). Do not label the data points Hint: Once...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the...
Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the following reaction as a function of the concentrations of the products: Ca(103) (s) Ca²+ (aq) + 210,- (aq) 2. Ca(IO3)2 will ionize in water to produce 10, ions. The 10, ions will react with KI. Write the reaction for this reaction. 3. We will be using starch as an indicator. Why? 4. In this experiment, we will first produce Izby mixing calcium iodate with...
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar...
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar solubility in mol/L for Zn(OH): in water. Zn(OH): has a Kap value of 1.8 x 10. Also, fill in the provided ICE table in solving this problem. Zn(OH)2(s)Zn2 (ag)20H (aq) Initial concentration (M Change in concentration (M) Equilibrium concentration (M From the molar solubility in question 1, calculate the concentration of OH ions in solution, and the pH of the solution. . Two 10.0...
Muyuulin (1JJ. Part III: Determination of a Solubility Product In Part Ill you will prepare a...
Muyuulin (1JJ. Part III: Determination of a Solubility Product In Part Ill you will prepare a saturated solution of silver carbonate (Ag2CO3) and deten solubility product constant of Ag2CO3. Ag2CO3(s) = 2 Agt(aq) + CO32-(aq) (17) In making the solution, 1.0 mL of 0.10 mol/L AgNO3 will be added to specified volume mol/L Na2CO3. The limiting reagent in this reaction will be the silver ions. Use of an excess an of anion allows for a relatively simple calculation of the...
Determination of the Solubility Product Constant of an Organic Salt Prepurod by Judith C.Foster, ...
Determination of the Solubility Product Constant of an Organic Salt Prepurod by Judith C.Foster, Bosndoin College PURPOSE OFTHE EXPERIMENT Determine the solubility and solubility product constant of potassium hydrogen tartrate by titrimetry BACKGROUND INFORMATION A complete characterization of a chemical system involving substances dissolved in water includes studying the relevant equilibria. For the gene ralized chemical reaction aA +bBcC+ dD, the equilibrium constant expression is Eq.1 In the case of an acid salt, such as sodium hydrogen oxalate monohydrate (NaHC,0,-H,O)...
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...
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, 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....
help please?
this was the only other information given
REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
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,...
please and thank you!
Volume of K2Cr04 (mL) Absorbance Molar concentration of CrO42- (M) 2.4 x 10-5 1.00 0.89 5.00 1.2*10^-4 0.55 10.00 2.4*10^-4 0.99 15.00 3.6*10^-4 1.37 QUESTION 3 10 points Save Answer Upload the plot of the standard curve. Use excel to construct it. Label the axes and draw the linear relationship. Show the equation of the line on the plot (at the top right away from the data points). Do not label the data points Hint: Once...
. Determination of an equilibrium constant Use the calculated absorbance values from Table 4 in Part II (y values and the best-fit line equation from Part I to calculate the [FeSCN2"), at equilibrium. Show two sets of calculations and complete Table 6 below. Sample Calculation with hypothetical values of Absorbance from Table 4 & fitted egn. from Table 3 y = mx + b (y is absorbance) 0.0620 - 2000x -0.0250 x-0.0620+ 0.0250 2000 = 4.35 x 10 с D...
Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the following reaction as a function of the concentrations of the products: Ca(103) (s) Ca²+ (aq) + 210,- (aq) 2. Ca(IO3)2 will ionize in water to produce 10, ions. The 10, ions will react with KI. Write the reaction for this reaction. 3. We will be using starch as an indicator. Why? 4. In this experiment, we will first produce Izby mixing calcium iodate with...
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar solubility in mol/L for Zn(OH): in water. Zn(OH): has a Kap value of 1.8 x 10. Also, fill in the provided ICE table in solving this problem. Zn(OH)2(s)Zn2 (ag)20H (aq) Initial concentration (M Change in concentration (M) Equilibrium concentration (M From the molar solubility in question 1, calculate the concentration of OH ions in solution, and the pH of the solution. . Two 10.0...
Muyuulin (1JJ. Part III: Determination of a Solubility Product In Part Ill you will prepare a saturated solution of silver carbonate (Ag2CO3) and deten solubility product constant of Ag2CO3. Ag2CO3(s) = 2 Agt(aq) + CO32-(aq) (17) In making the solution, 1.0 mL of 0.10 mol/L AgNO3 will be added to specified volume mol/L Na2CO3. The limiting reagent in this reaction will be the silver ions. Use of an excess an of anion allows for a relatively simple calculation of the...
Determination of the Solubility Product Constant of an Organic Salt Prepurod by Judith C.Foster, Bosndoin College PURPOSE OFTHE EXPERIMENT Determine the solubility and solubility product constant of potassium hydrogen tartrate by titrimetry BACKGROUND INFORMATION A complete characterization of a chemical system involving substances dissolved in water includes studying the relevant equilibria. For the gene ralized chemical reaction aA +bBcC+ dD, the equilibrium constant expression is Eq.1 In the case of an acid salt, such as sodium hydrogen oxalate monohydrate (NaHC,0,-H,O)...
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...
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....
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