Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL. AgCl: Ksp = 1.82 x 10^-10
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Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL.
AgCl: Ksp = 1.82 x 10^-10
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- Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)If a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the MW of calcium carbonate? (use C1 as reference)* 102 g/mol 98 g/mL 100 g/mL 100 g/mol What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852
- On titrating 50 ml of 0.01 M KI with 0.01 M AgNO3 . The value of pAg after addition of 30 ml AgNO3 is ...................................................................... ( Ksp= 5.2 xl0 -13 )What is the solubility of Mg(OH)₂ at a pH of 12.70? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³) Consider the titration of 30.0 mL of 0.275 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. What is the pH of the solution before any acid has been added? Consider the titration of 30.0 mL of 0.275 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. What would be the pH of the solution after the addition of 20.0 mL of HI?5A. Construct the titration curve for a 25.00 mL mixture solution of 0.0800 M in Br- and 0.0600M in IO3- titrated with 0.1000 M AgNO3. Calculate the pAg values of the titration solution after addition of 5.00mL, 20.00 mL, and 30.00 mL of 0.1000 M AgNO3 solution.KSP AgIO3 = 3.0 × 10-8 KSP AgBr = 5.2 × 10-13 Please answer fast i give you upvote.
- 1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, CH3COOH. For 20.0 cm3 of the vinegar, 26.7 cm3of 0.60 mol dm-3 NaOH solution was required.What was the concentration of acetic acid in the vinegar if no other acid was present? (Thanks for your help) A. 0.45 mol dm-3B. 0.60 mol dm-3C. 0.80 mol dm-3D. 1.60 mol dm-3Procedure Preparation of Dilute Solution of Vinegar • Using a 10 mL pipette, transfer 10mL of vinegar into 100 mL volumetric flask. • Dilute to mark of the volumetric flask using distilled water. B. Titration of Diluted Solution of Vinegar • Transfer 25 mL of diluted solution to 250 mL Erlenmeyer flask. • Add 0.5 mL phenolphthalein indicator. Set aside. • Transfer 50mL of 0.110 M NaOH into a 50 mL burette. • Titrate the diluted solution until the phenolphthalein endpoint (very faint pink). • Record volume of NaOH used. Answer the question: What is the experimentally determined concentration of acetic acid in your vinegar solution: (Please give your answer to three significant figures.) ______ M Acetic AcidConsider the titration of 110.0 mL analyte solution containing 0.15 mol L-1 NH3 with 0.10 mol L-1 HCI titrant. Determine the pH of the solution after adding 25.0 mL of titrant. (Kb(NH3) = 1.8 x 10-5, T= 250C).
- 1. What is the concentration of the titrant in Normality? 2. What is the mEq of KOH in mg/gram? 3. Find the acid value of the sample 4. Find the saponification Value of the sampleWhat is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.758 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 35.00 mL. Ca2+ + Y4- → CaY2- 0.1500 g 5.630 g 6.158 g 0.6158 gA 25.0 mL sample of 0.250 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) is titrated with 0.250 M NaOH solution. Calculate the pH after the following volumes of base have been added. a) 0 mL b) 12.5 mL c) 25.0 mL d) 35.0 mL PLEASE SHOW ALL WORK