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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^-10On 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 )For the titration of 100mL of 0.001M NaCl (Cl-) with 0.0100M AgNO3 (Ag+), calculate the voltage at VAg+ = 0.5, 10.0, and 15.0mL Ksp (AgCl) = 1.8 x 10-10.
- What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.875 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 30.00 mL. Ca2+ + Y4- → CaY2- 5.630 g 0.6158 g 0.1500 g 6.158 gCompute the titration curve for Demonstration 16-1, in which 400.0 mL of 3.75 mM Fe21 are titrated with 20.0 mM MnO24 at a fixed pH of 0.00 in 1 M H2SO4. Calculate the cell voltage at titrant volumes of 1.0, 7.5, 14.0, 15.0, 16.0, and 30.0 mL and sketch the titration curve.In which of the following solutions will CdS (Ksp = 1.0 x 10-28) be more soluble than in pure water? Group of answer choices 0.10 M Cd(NO3)2(aq) 0.050 M Na2S(aq) 0.20 M Na2SO4(aq) in none of these solutions
- At 40.0 mL 0.0050 M Sr2 + pH 10, 0.0100 M EDTA is titrated. Calculate the pSr for the equivalence point. Kfor (SrY) = 4.3x108, α4 = 0.35Calculate the silver ion concentration after the addition of 5.00, 30.00, 40.00, 45.00 and 50.00 ml of 0.05000 M AgNO3 to 50.0 mL of 0.0400 M KBr. Construct a titration curve from these data plotting pAg as a function of titrant volume (Ksp (AgBr)=5.0 x 10-13 )Need solution to all parts if not answered I'll downvote solution Find the pH during the titration of 20.00 mL of 0.1910 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.1910 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 20.00 mL (e) 25.00 mL
- 1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.Calculate MW from Average EM. MW (g/mol) = n (eq/mole) x EM (g/eq) where n is the number of H+ ions titrated per moelcule of acid TRIAL # moles of OH- # moles of H+ # equivalents H+ Equivalent Mass (g/eq) 1 0.00264 0.00264 0.00264 113.26 2 0.003295 0.003295 0.003295 91.05 113.26 + 91.05 = 204.31/2 = 102.155 g/eq average EM Acid is Sulfamic AcidPlease answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. A 50.00-mL sample of water containing Ca2+ and Mg2+ is titrated with 10.28 mL of 0.01001 M EDTA in an ammonia buffer at pH 10.00. Another 50.00-mL sample is titrated with NaOH to precipitate Mg(OH)2 and then titrated at pH 13.00 with 6.75 mL of the same EDTA solution. Calculate the concentration of CaCO3 and MgCO3 in the sample in ppm.
