What is observed when equal volumes of 0.1M aqueous HCl and 0.01 M Na2SO3 are mixed? Group of answer choices Colorless solution and a white precipitate. Colored solution and a white precipitate. Colorless solution and a colored precipitate. Colorless solution, no precipitate and gas evolution
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- A solution of KI is added dropwise to a solution that is 0.0144 M in Pb2+. When the concentration of I- exceeds ________ M, PbI2 will precipitate. Neglect volume changes. Ksp for PbI2 is 1.4 x 10-8. Show all steps please, dont skip any steps.Knowing that Ksp of PbI2 = 10-⁷ find out if precipitate will form when mixing 100ml of 0.01 N Pb solution (NO3) 2 and 200ml of 0.01 M NaI solutionPART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).
- The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solving
- pls complete the table using given dataEffect of Common Ions on the Solubility of Ca(OH)21. Add Ca(OH)2 to 250.0 mL of 0.010 M CaCl2 with stirring until equilibrium is achieved.2. Filter the undissolved precipitate. Measure out 50.0 mL of the filtrate in a 250-mL Erlenmeyer flask. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume of HCl solution used. Perform two more trials.Will a precipitate form when 100.0 mL of a 4.6 ✕ 10-4 M Mg(NO3)2 is added to 100.0 mL of 5.1 ✕ 10-4 M NaOH? (Hint: Ksp for Mg(OH)2 = 8.9 ✕ 10-12) Yes Give the value of Q, to support your answer. __________________________________How much amount (in grams) do you need to prepare the following solutions 500.0 mL 0.1000 M stock EDTA solution from Na2H2EDTA•2H2O (FW=372.24) and MgCl2•6H2O crystals 100.0 mL 0.0500 M stock Ca2+ solution from pure CaCO3 (FW=100.09) and concentrated HCl 250 mL 1.0 M NH3-NH4+ pH 10 buffer solution from NH4Cl and NH3
- The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?TRUE OR FALSE 1. Sodium arsenite is formed due to the solubility property of arsenic trioxide in sodium hydroxide. 2. The permanganate method is always carried out in a highly acidic medium. 3. The color of permanganate solution renders impossible accurate readings at the lower meniscus. 4. Sodium bicarbonate in the standardization of iodine solution acts as a buffer. 5. Sulfuric acid in permanganate titration prevents the formation of reduction products.A solution of NaF is added dropwise to a solution that is 0.0105 M in Ba2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 ⋅ 10-6. A 8.1 ⋅ 10-5 B 1.6 ⋅ 10-4 C 1.8 ⋅ 10-8 D 1.3 ⋅ 10-2 E 3.2 ⋅ 10-3