Question 5 1 pts You have a saturated solution of Ca(OH), in a flask, meaning there...
D Question 4 1 pts The reaction shown is at equilibrium. If a student adds more X to the system, what happens immediately (at that instant) to Q and K? X Y Z Both decrease Both increase O Qgets larger and gets smaller K gets larger and gets smaller Kremains constant and increases Kremains constant and a decreases 1 pts Question 5 You have a saturated solution of Ca(OH)2 in a flask, meaning there is some solid CaOH)2 sitting at...
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)...
D Question 9 2 pts 15.0 ml of a saturated Ca(OH)2 solution is titrated with 0.050 M HCl. The equivalence point is found to be when 17.1 ml of the HCl has been added. What was the initial concentration of the [Ca2+] O 0.0439 M O 0.0285 M 0 0.0219 M O 0.0570 M
"Hydroxyapatite, Cao(PO)(OH),, has a solubility constant of Ksp = 2.34 x 10-59, and dissociates according to Ca,(PO)(OH),(s) = 10 Ca2+ (aq) + 6 PO (aq) + 2OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2+ in this solution if [OH-] is fixed at 6.50 x 10-M?
1A) How will the calculated Ksp value of Ca(OH)2 be affected if the original Ca(OH)2 solution is not saturated? Explain? B) Does adding distilled water to the titrating flask in order to wash the sides of the flask and the buret tip affect the computed Ksp of Ca(OH)2? Explain? C) How might tap water instead of distilled water affect the calculated Ksp of Ca(OH)2? Explain? D) The temperature of the solution was 21.1 degrees Celcius. Is the molar solubility of...
Question 8 2 pts 15.0 ml of a saturated Ca(OH)2 solution is titrated with 0.050 M HCl. The equivalence point is found to be when 17.1 ml of the HCl has been added. What was the initial concentration of the [OH-]? O 0.0439 M 0 0.0219 M O 0.0285 M. O 0.0570 M • Previous Next
2. Calculate (Ca²+], [OH ], and [H30*] for a solution that is prepared by dissolving 0.600 grams of Ca(OH)2(s) in enough water to make 1.00 liters of solution at 25°C. 3. Calculate the pH of an aqueous solution that is 0.020 M in HNO3(aq) at 25°C. Is the solution acidic or basic? 4. Calculate the pH and the pOH of an aqueous solution prepared by dissolving 2.0 grams of KOH(s) pellets in water and diluting to a final volume of...
You have titrated 30.00mL of an unknown Ca(OH)2(aq) solution to the second equivalence point with 34.93mL of 0.417M HCl(aq). What is the concentration of the Ca(OH)2(aq) solution?
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...
you add an excess of ca(oh)2 to water maintained at particular temperature, stir until the solution is saturated, filter, then determine the OH in the solution by titration with acid. titration of 10.0 ml of the calcium hydroxide solution to the end point requires 4.86 ml of 0.070 M HCl solution. what is the molar quantity of OH- in the 10.0 ml of solution? what are the concentrations of Ca2+ and OH- ? WHAT IS THE SOLUBILITY OF Ca(OH)2 under...