Why is it important the Erlenmeyer flasks be dry upon addition of the saturated Ca(IO3)2 aliquot?
Why is it important the Erlenmeyer flasks be dry upon addition of the saturated Ca(IO3)2 aliquot?
A 10.00 mL sample of saturated Ca(IO3)2 was collected from a solution at 10.2°C. After adding excess KI and H+, the resulting solution required 8.52 mL of 0.0543 M Ca(IO3)2 to titrate to the endpoint. Identify how many moles of Na2S2O3 are in 8.52 mL of 0.0543 M Na2S2O3?
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
Suppose a student titrates a 10.00-mL aliquot of saturated Ca(OH)2 solution to the equivalence point with 14.30 mL of 0.0224 M HCl. What was the initial [OH − ]? WebAssign will check your answer for the correct number of significant figures .064 M 1 Incorrect: Your answer is incorrect. What is the experimental value of Ksp?
Ksp of Ca(IO3)2 lab questions 1) Why is it necessary to filter the calcium iodate solution through dry filter paper, without adding any water? 2) If water had been added during the filtration process, how would this affect your calculated value for the Ksp of calcium iodate? Clearly explain whether your value would be too high or too low compared to the actual Ksp and why.
8-d) Set up mass and charge balance equations for these solutions. i) Solid Ca(IO3)2 is put in deionized water and dissolves until the solution is saturated. ii) Solid Ca(IO3)2 is put in water with 0.010 M Ca(NO3)2. iii) 0.050 M KCl, 0.050 MgCl2, and 0.050 K2SO4, all in the same solution. iv) A solution made by mixing 750 mL of 0.10 M AgNO3 with 250 mL of 0.10 M KI.
Why is it so important to keep the silica gel saturated with solvent at all times during preparation and development of a column? How would the quality of separation be affected if the column was allowed to run dry? 3.
Question Completion Status: QUESTION 1 Why don't you have to accurately record the amount of Ca(OH)2 used in the saturated solution? The Ca(OH)2 only serves as the spectator ions in this experiment. The amount or concentration of Ca(OH)2 is not important in this experiment. We are only interested in the amount of Ca(OH)2 that dissolves at each temperature (which is found after filtration via titration), and not the entire amount of Ca(OH)2 that is used in the saturated solution before...
Part A and Part B.
Also question #3-post lab. (its circled)
A. Molar Solubility and Solubility Product of Calcium Hydroxide Trial I Trial 3 Trial 2 25.0 1. Volume of saturated Ca(OH), solution (mL) 2. Concentration of standardized HCl solution (molU/L) 3. Buret reading, initial (mL 4. Buret reading, final (mL) 5. Volume of HCI added (mL) 6. Moles of HCI added (mol) 7. Moles of OH" in saturated solution (mol) 8. (OH1, equilibrium (mol/L) 9. (Ca2 ], equilibrium (mol/L)...
Dry Lab (use Ksp and Kç values from your text) Which of the following metals will ppt first following the addition of NaOH? Ba or Ca or 1. (2 pts) Co What is the molar solubility of Ca(OH)2? What is the pH of a saturated Ca(OH)2 solution? 2. (3 pts) In the first qual lab, why did PbCl2 (s) dissolve in hot water, but AgCl (s) did not? Answer in terms of Kp and AHsoly (which is endothermic). 3. (3...
ca 2
de that can man have killed millions of fish. In addition mollusks that feed on K. brevis. People who eat these bivalves from paralytic shellfish poisoning, a food poisoning that can cause severe gastrollile symptoms, such as tingling in the fingers or toes. Use your results to explain why these so-called 'red occur in coastal water. 2. Outbreaks of cyanobacterial intoxication associated with lakes and ponds are reported annually. What would cause an increased number of cases in...