What is the maximum metallic concentration in 100.0 liters of water from a metallic hydroxide with a Ksp = 3.99 x 10-20 at pH 3.0, 7.0, and 10.0? Show all work and report final answers with three significant figures.
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- Construct a titration curve that is expected to be obtained by titration 50.00mL of 0.1000M Sr2+ with 0.1000M EDTA at pH 11. Kf = 4.3 x 10^8. Use the following volumes to construct the curve: 0.00, 10.00, 30.00, 40.00, 45.00, 50.0, 55.00, 60.00 and 70.00mL.mix 500 ml of 0.1 M HCl solution with 300 ml of 2 M Ba (OH) 2 solution a) indicate the environment of the solution after mixing b) What color will the detectors, phenophthalein and litmus get?The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of the common ion effect: Trial 1: Final Buret reading (ml)-29.50; Initial Buret reading (ml)- 26.10; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-33.30; Initial Buret reading (ml)- 29.50; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 3.40ml; Trial 2- 3.80mL. Report in proper sigfigs. 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Use the dilution formula to determine the initial concentration of the common ion. C1V1 = C2V2 3. Construct an ICE table for the reaction.4. Calculate the molar solubility…
- The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of the common ion effect: Trial 2: Final Buret reading (ml)-33.30; Initial Buret reading (ml)- 29.50; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 3.80mL. Report in proper sigfigs. 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Use the dilution formula to determine the initial concentration of the common ion. C1V1 = C2V2 3. Construct an ICE table for the reaction.4. Calculate the molar solubility (in mol/L) of OH- and Ca2+.5. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol).…The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of the common ion effect: Trial 2: Final Buret reading (ml)-33.30; Initial Buret reading (ml)- 29.50; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 3.80mL. Report in proper sigfigs. 1. Calculate the molar solubility (in mol/L) of OH- and Ca2+.2. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 3. Calculate the Ksp of Ca(OH)2. Make sure to include the effect of the common ion in the calculation.A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating with 0.0400 M AgNO3 requires 25.00 mL to reach the Mohr endpoint. A blank titration requires 0.50 mL to reach the same endpoint. Calculate the %w/w BaBr2 in the sample. Please provide a complete solution.
- I would need help with these problems, please show step by step: 1. A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4 To this solution was added 50.0 mL of 0.15 M hydrochloric acid (HCl). What was the change in pH of the ammonia, ammonium ion solution? 2. Calculate the isoelectric and isoionic pH of 0.010 M threonine? pK1 = 2.15, pK2 = 9.12 3. Find the pH of a 1.00 L aqueous solution containing 12.43 g of tris (FM 121.14) plus 4.67 g of tris hydrochloride ( FM 157.60) ? What would be the new pH after adding 12.0 mL of 1.00 M NaOH to this buffer?Determining the Ksp of Calcium Hydroxide: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2 The molarity of the hydrochloric acid used was 0.050 M. 15.00 mLof filtered Ca(OH) 2 was measured out for the titration.Calculate the Ksp for calcium hydroxide. Explain your calculations Trial Initial Buret Reading Endpoint Buret Reading Endpoint Volume Equivalence Point Volume 1 80ml 9.31 pH 12ml 12.60mlFollowing the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. What specific type of titration is involved? A. Direct Acidemetry B. Direct Alkalimetry C. Residual Acidemetry D. Residual Alkalimetry 2. What is the analyte- titrant chemical reaction involved? A. Strong Base+Weak Acid B. Weak Acid+Strong Base C. Strong Acid+Weak Base D. Weak Base+Strong Acid 3. What is the preferred indicator for the chosen type of reaction above? A. Methyl Orange B. Penolphtalein C. Methyl Red 4. Consider that the burette was completely filled to the 0mp mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 22.2 mL C. 21.3 mL D. 22.7 mL 5. What is the unknown weight (grams) the problem? Your Answer:
- Calculate the water hardness (mg L-1 of CaCO3) (i.e. calculate the mass of CaCO3) please show working out. thank you :) Sample No. 1 2 3 4 Final Burette reading (mL) 24.40 46.90 24.70 47.20 Initial Burette reading (mL) 0.10 24.40 2.10 24.70 Final-Initial Titre (mL) 24.30 22.50 22.60 22.50What conclusion can be derived from the following sentences regarding analytical methods: I. Classical methods (gravimetry and volumetric methods) are no longer useful in analytical chemistry. II. Volumetric methods do not require calibration if a primary standard is used as titrant. III. Instrumental methods are useful with analyte solutions that are less than 1.00 mM. IV. Classical methods yield high precision and accuracy at concentrations greater than 1.00 mM. What conclusion can be derived from the following sentences regarding analytical methods: Two statements are incorrect. All statements are correct. One statement is incorrect. Only one statement is correct. All statements are incorrect.Objective: To determine the percent NaCl (w/v) of a water sample 5.00 mL sample diluted to 50 mL solution 0.1000 M AgNO3 Volume of AgNO3 trial 1=15.30 mL trial 2=14.90 mL trial 3=15.10 ml