Calcium carbonate has a Ksp value of 1.4 x 10^-8 at 25 degrees Celsius a) What is the [Ca^2+] in a saturated solution of calcium carbonate at 25 degrees celsius. Write answer as a decimal b) What is the solubility of calcium carbonate in a 0.100M solution of calcium nitrate at 25 degrees celsius. Write answer as decimal c) If you add 20.0 mL of 0.00350M calcium chloride to 40.0 mL of 0.000100M sodium carbonate, will precipitation occur? (Yes or no) (k>q or k

Calcium carbonate has a Ksp value of 1.4 x 10^-8 at 25 degrees Celsius a) What is the [Ca^2+] in a saturated solution of calcium carbonate at 25 degrees celsius. Write answer as a decimal b) What is the solubility of calcium carbonate in a 0.100M solution of calcium nitrate at 25 degrees celsius. Write answer as decimal c) If you add 20.0 mL of 0.00350M calcium chloride to 40.0 mL of 0.000100M sodium carbonate, will precipitation occur? (Yes or no) (k>q or k

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 8P

See similar textbooks

Similar questions

A sodium hydroxide (NaOH) solution was standardized with KHP primary standard. The concentration was found to be 0.1022 M. What is the concentration of a 25.0-ml hydrochloric acid (HCl) solution if it required 32.6 ml of NaOH to reach the phenolphthalein end point?
A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and 0.30 molmol of NH4ClNH4Cl. What mass of the correct reagent should you add? Express your answer using two significant figures.
What is the molar solubility of a saturated solution of calcium hydroxide, Ca(OH)2, in water? The Ksp of Ca(OH)2 is 1.2×10–11. Options: 1.4×10–4 1.8×10–4 3.4×10–6 3.6×10–4
Explain how the calculation of the molar solubility will be affected if a small amount of the sample adhering to the side of the flask was left unreacted when the end point was thought to have been reached. Procedure: Pipet 25 mL of the saturated Ca(OH)2 solution (without added CaCl2) into a 125 mL flask and add 2 drops of methyl orange indicator. Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Titrate two additional 25 mL aliquots of the saturated Ca(OH)2 solution
Average the two percentages and calculate the percentage difference. given : Concentration of acetic acid in the 100 mL sample of titration 1 = 3.238 % Concentration of acetic acid in the 100 mL sample of titration 2 = 3.099 % NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of…
Use the following solubility data to calculate a value of Ksp for each compound: a) CdCO3 : 1.0 x 10^-6 M b) Ca(OH)2 : 1.06 x 10^-2 M c) PbBr2 : 4.34 g/L d) BaCrO4 : 2.8 x 10^-3 g/L
1. If Mg(OH)2 has a Ksp of 7.0 × 10–6, then what is the solubility of Mg(OH)2 in pure water? Give your answer in units of g/L. Express the answer to 4 significant digits and do not use scientific notation. *Use the Ksp given here. Do not look up your own value. 2. 200.0 mL of 0.005 M Na2CO3 are added to 200.0 mL of 0.002 M MgCl2. Does a precipitate form? [Ksp(MgCO3) = 6.82 × 10–6] Question 2 options: No, because Q = Ksp. Yes, because Q > Ksp. No, because Q < Ksp. No, because Q > Ksp. Yes, because Q < Ksp. 3.In order for a precipitate of PbBr2 to form, what is the minimum concentration of Br- that must be present in a solution of 0.00050 M Pb(NO3)2. The Ksp of PbBr2 is 2.20 × 10–6.
In an experiment, a student is attempting to dissolve Lead Bromide (PbBr2) into a 1 L solution that already contains 0.100 M of dissolved Sodium Bromide (NaBr). If the Ksp of Lead Bromide is 4.67*10-6, what is the solubility of Lead Bromide in the solution? (HINT: Use the x is small approximation to simplify your calculations. Please provide your answer to 3 significant figures.)
In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)
A saturated solution of copper (I) chloride, CuCl, has [Cu+] = 1.1X10-3 M and [Cl-] = 1.1X10-3 M. What is the numerical value of Ksp for CuCl?
1)A bottle of concentrated aqueous sulfuric acid, labeled 95.00 wt% H2SO4, has a concentration of 16.5 M. Calculate the density of 95.00 wt% H2SO4. 2)Ascorbic acid in 5 vitamin C tablets was measured by a titration against (100 ± 0.002 M) NaOH solution. It required 10.00 ± 0.05 mL NaOH solution to reach the equivalent point. What is the average quantity of ascorbic acid per vitamin tablet?
Q: The solubility product of Zn(OH)2 at 25oC is 3.0 x 10-6 M3. Calculate the solubility of Zn(OH)2 in water in gdm-3. [Ar: Zn = 65.5; O = 16; H = 1] The Mr for Zn(OH)2 is 99.5. When I multiply it with Ksp, I didn't get the same answer as the given answer which is 0.904 gdm-3.