(6 points) The concentration of calcium in a saturated aqueous solution of calcium carbonate (CaCO3) at...
Explain How and Why, Thank you! 7. Calcium carbonate is dissolved in a solution of 0.0500 M CaCl2 to make a saturated solution. (a) Write all of the pertinent equilibrium reactions in this solution. (b) Write a charge balance equation for the solution. (c) Write two mass balance equations for the solution. (14 points) a Ho(H (aq)+OH (aq) CaCO, (s)Ca2 (a)COj (aq) cơ (aq) + H2O(1) HC0,(aq) + OH (aq) HCO, (a)+H20)- H2CO, (aq) +OH (aq) (e [c]-0.100 M [Ca2+]...
A student measures the Ca2+ concentration in a saturated aqueous solution of calcium fluoride to be 2.18x10-6 M. Based on her data, the solubility product constant for calcium fluoride is Submit Answer Retry Entire Group 9 more group attempts remaining
11. Barium carbonate is used in manufacturing of TV screens and fireworks, as well as rat poison, cement, and ceramic glazes. It is a "sparingly soluble" salt with a ks = 2.58 x 10°at 25 °C. a. Write the balanced equation for the dissolution of barium carbonate and the corresponding Ksp expression. (Remember to include the phase of matter--(s), (aq), (8), etc!) b. What is the MOLAR solubility of barium carbonate in water at 25°C? C. What is the SOLUBILITY...
Fluorite, CaF2, is a slightly soluble salt in water. In a saturated solution, the concentration of [Ca2+] = 2.5 x 10^-4 and [F-] = 4.30 x 10^-4 a. write the dissolution equation for fluorite. b. Write Ksp expression for the dissolution of fluorite. c. Calculate the Ksp.
. The concentration of magnesium, calcium, and nickel(II) ions in an aqueous solution are 0.0010 M. (a) In what order to they precipitate when potassium hydroxide is added?; (b) determine the pH at which each salt will precipitate. The molarity of CrO42– in a saturated Tl2CrO4 solution is 6.3×10–5 mol·L–1, what is the Ksp of Tl2CrO4?
QUESTION 1 1 points 1 points Save Answer Save Answer Calcium hydroxide is a slightly soluble salt. A saturated solution of calcium hydroxide is prepared, and comes to equilibrium: Ca(OH)2 (s) + Ca2+(aq) + 2 OH"(aq) What is the solubility product constant (Ksp) expression for this equilibrium? [Ca2+ [OH-] [Ca(OH)2] A. Ksp = B. Ksp = [Ca2+1OH-] c Ksp = [Ca2+[OH-] [caz+Com'] [Ca(OH)2] QUESTION 2 1 points Save Answer Consider a chemical reaction which has achieved a state of equilibrium....
Q1) A) calculate the concentration of hydroxide in a saturated solution of calcium hydroxide (Ksp= 6.5*10^-6). B) what is the pH of the calcium hydroxide solution above?
1. Calculate the expected concentration of Ca2+ in saturated calcium iodate, ksp=6.47 x 10^-6. 2. Use this result to calculate the concentration of IO3- in saturated calcium iodate.
QUESTION 6 (15 points) A) A saturated solution of calcium fluoride CaF2 is found to contain a concentration of fluoride ions [F] = 3.0 x 10-6 M. What is the value of the solubility product of this salt?
10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp? CaF2(s) -> <- ca2+ (aq) +2 F- (aq) How did Ksp= [Ca2+] [F-]2 become Ksp= [s] [2s]2= 4s3 Cause I thought it was only Ksp= [s] [s]2 = s3 and why 4.28x10-3 have to devide by 10 and why the [F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4...