Given the following salts and their Ksp values: (1) Silver Bromide, with Ksp = 5.0 x 10-13 (2) Calcium Carbonate, with Ksp = 4.8 x 109 (3) Cobalt(II) hydroxide, with Ksp =2.6 x 10-16 (4)Iron (II) hydroxide with Ksp = 8.0 x 10-16 and (5) Lead (II) lodide, with Ksp = 1.1 x 10 Question #2) Which of the given salts is the least soluble? (1) (2) (3) (4) (5)
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- Discuss if the following compound will experience solvation and/or dissociation. MgCl2Consider that benzoic acid is a weak acid which has a Ka of 6.3 x 10-5 . C6H5COOH → C6H5COO- + H+ Calculate the [H+ ] ion concentration of a 0.04 M benzoic acid solution. Use your findings from above, determine the pH of the solution.Write the Ksp expression for Cu(OH)2 in terms of [Cu2+] and [OH–].
- Use the information provided to determine the Ksp of the salt. A saturated iron(II) hydroxide solution has a pH of 10.62.Preparation of cpper(1) chloride What color observed for the solution of Na2SO3 in water? What colour observed for solutions of CuCl2.2H2O in water? Which ion is responsible for the colour that is observed in the CuCl2 solution? What is observed when th Na2SO3 solution is added to the CuCl2? Which gas can be smelled when H2SO4 is added to the mixture? What is the colour of the CuCl when it is filtered on Buchner funnel? (before it is exposed to the atmosphere) What is the colour of the CuCl when it is filterd on the Bucher funnel? (before it is exposed to the atmosphere) Does the colour of the CuCl remain the same if you leave it to dry in the atmosphere? Calculate the percentage yields for the experimentFinely ground mineral (0.9315 g) was dissolved in 25 mL of boiling 4 M HCl and diluted with 175 mL H2O containing two drops of methyl red indicator. The solution was heated to 100C, and 50 mL of warm solution containing 2.0 g (NH4)2C2O4 were slowly added to precipitate CaC2O4. Then 6 M NH3 was added until the indicator changed from red to yellow, showing that the liquid was neutral or slightly basic. After slow cooling for 1 h, the liquid was decanted and the solid transferred to a filter crucible and washed with cold 0.1 wt% (NH4)2C2O4 solution five times until no Cl- was detected in the filtrate upon addition of AgNO3 solution. The crucible was dried at 105C for 1 h and then at 500 ± 25 C in a furnace for 2 h. Ca2+ + C2O42- --> CaC2O4.H2O(s) -->500C CaCO3(s) The mass of the empty crucible was 16.9743 g, and the mass of the crucible with CaCO3(s) was 17.198164 g. Find the wt% Ca in the mineral. a) Why is the unknown solution heated to boiling and the precipitant solution,…
- What recommendations can you give in titration of mixed alkali?Beaker Wavelength of Maximum Absorption Absorbance at Maximum Wavelength Form of Indicator in Solution A 438 0.293 HIn B 594 0.812 In- If you wanted to determine the concentration of your indicator in solution, which form of the indicator (HIn or In-) would give more accurate results? Why?Phenolphthalein is an acid–base indicator. In solutions of pH < 8.5, it is colorless; in solutions of pH > 8.5, it is deep red-purple. Account for the change in color.
- A reaction was carried out with Fe3+ and SCN- to produce FeSCN2+. Two best-fit lines for Absorbance vs [FeSCN-] were obtained. The first line produced: y = 200x + 0.005, r2=0.951 and the second line produced: y= 10,000x + 0.005, r2 = 0.993. Determine the best-fit line of two, and then use the line equation to determine the equilibrium concentration of FeSCN2+ if the absorbance = 0.863.1.Determine the color of the indicator in a given condition: METHYL ORANGE IN AN ACIDIC ENVIRONMENT. 2.This is the measure of reproducibility of data within a series of results. 3.This is the chemical to be subjected to testing in titrimetric method of analysis. 4.Determine the type of assay employed for this substance: TARTARIC ACID 5.Determine the color of the indicator in a given condition: PHENOLPHTHALEIN IN AN ALKALINE ENVIRONMENT. Please help me answer this questions. the answers are on the image I attachedThe first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.