Which of the following would lead to a negative percentage error in the determination of Ksp of Ca(OH)2? a. Unsaturated Ca(OH)2 solution was used in the titration. b. The volume of saturated CaCl2 used in the titration was in excess. c. The volume of HCl used was beyond the equivalence point of the reaction. d. A more concentrated HCl solution was used in the titration of Ca(OH)2.
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- In this experiment, the color change from pink/violet to colorless during the titration is caused by: change from MnO4– to Mn2+ change from Fe2+ to Fe3+ change from H+ to H2O the addition of an indicator.Calculations: Standardization of HCl Titrating Solution: Using your best two or three standardization titrations, calculate the concentration of the HCl titrating solution for each trial using the balanced equation between HCl and Na2CO3. What is the average concentration of your HCl solution? Ksp Determination at both temperatures Calculate the room temperature Ksp for borax. From the HCl volume used in each titration, calculate the concentration of borate in each room temperature aliquot using the equation between HCl and borate From the stoichiometric relationship between borate and sodium ion, calculate [Na+ ] in each aliquot. Calculate the room temperature Ksp for each titration using the following equation calculate the average Ksp value. Ice Bath Temperature Ksp Determination: Calculate Ksp for borax as you did for the room temperature system. Calculate the concentration of borate in each ice temperature aliquot. Calculate [Na+ ] for each ice temperature aliquot.…7. What specific chemicals are used to identify each of the methods? (Volhard's Method, Fajan's Method. and Mohr's Method) 8. What color reactions are expected at the end of the equivalence point? 9. How does acid-base titration differ from precipitation titration?
- A 10.0 mL of river water containing Ca2+ is titrated with EDTA. 5.0 mL of 0.10 M EDTA is used to reach the equivalence point in the EDTA titration. What is the concentration of Ca2+ in the river water? Assume that Ca2+ is the only cation in this sample. 0.000050 M 0.0050 M 5.0 M 0.050 M What is the correct charge balance expression for a solution that contains NaCl and HCl? [H+] + [Na+] = [Cl–] [H+] = [Cl–] [H+] + [Na+] = 2[Cl–] [Na+] = [Cl–]If you plot pBr instead of pAg against the added volume of AgNO₃, what do you think will happen to the shape of the titration curve with respect to the original?Calculation of the Solubility from EDTA Titration Data 1. A 10.0 mL sample of supernatant liquid was titrated with 0.01022 M EDTA solution. It required 16.90 mL of EDTA to reach the end point. Calculate the [Ca^ 2+ ] and hence the solubility of CaSO 4 in 10.0 mL sample. 2. List important practical applications of complexometric titration of Ca^ 2+ ions . Please show all steps
- A titration is carried out to determine the molecular weight of oxalic acid. In this experiment, 0.617g of oxalic acid was dissolved in water and 18.3 mL of 0.75 M NaOH were used to reach the equivalence point of the titration. However, each mol of oxalic acid reacts with 2 mols of NaOH. A.What is the molecular weight of oxalic acid? B. What is the concentration of oxalic acid in the original solution if the total volume was 100mL2. EDTA is one of the common reagents used in a complexometric titration. a. Can we use EDTA titrations to determine the concentration of halides in a sample? Give reason for your answer. b. Why is EDTA used to determine concentration of a metal ion ina solution. c. Why is Erichrome black -T used as the indicator in EDTA titrations ? d. Explain hardness of water. Why is it usually expressed in terms of Ca2+ ions?Determining the ksp of Calcium Hydrioxides Titration of Calcium Hydroxide with HCl Mass of Erlenmeyer flask: 25.52 g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) (g): 28.44 g Mass of Calcium Hydroxide Solution (g): 2.92 g Volume of Ca(OH)2 Density = 1.000 g/mL (mL) - 2.92 mL Concentration of HCl (M) - How do you find this? HCl 0.10 M solution used Initial HCl volume = 0.79 mL Final HCl volume = 0.09 mL volume of HCl delivered = 0.70 mL Moles of HCl delieverd - how do I calculate this? Moles of OH- in sample - how do I calculate this? Moles of Ca2+ in sample - how do I calculate this? Thank you!
- Determining the ksp of Calcium Hydrioxides Titration of Calcium Hydroxide with HCl Mass of Erlenmeyer flask: 25.52 g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) (g): 28.44 g Mass of Calcium Hydroxide Solution (g): 2.92 g Volume of Ca(OH)2 Density = 1.000 g/mL (mL) - 2.92 mL Concentration of HCl (M) - How do you find this? HCl 0.10 M solution used Initial HCl volume = 0.79 mL Final HCl volume = 0.09 mL volume of HCl delivered = 0.70 mL Moles of HCl delieverd - 0.07 x 10^-3 mol Moles of OH- in sample - 0.07 x 10^-3 mol Moles of Ca2+ in sample - 0.035 x 10^-3 mol How do I calculate molar solubility and ksp? Thanks!!1. The concentration of sulfate in a solution containing a mixture of sulfuric acid is to be determined. A 25.0 mL portion of the sample is treated with 10.00 mL of 0.0500 M BaCl₂. The resulting precipitate is filtered off and the supernatant solution containing the Ba²⁺ is then titrated with 0.0354 M EDTA which gives an end point at 7.45 mL. (a) Identify the type of EDTA titration method used. (b) Calculate the molar concentration of sulfate in the sampleAt some other temperature, a solid sample of Ca(OH)2 is shaken with 0.0100 M CaCl2.Once equilibrated, some solid Ca(OH)2 remains undissolved.The solution is filtered and a 20.00 mL sample requires 39.04 mL of 0.0100 M HCl to neutralize it.Calculate the value for Ksp of Ca(OH)2 from this data.