Find Ksp for a CaCl2 solution in which the Ca2+ concentration is found to be 0.125M.
Find Ksp for a CaCl2 solution in which the Ca2+ concentration is found to be 0.125M.
Find the activity coefficient of Ca2+ in a solution of 3.3 mM CaCl2 when the activity coefficient is 0.675 and the size of the ion is 600 pm
When 5.5 g of CaCl2 is dissolved in 1 L of solution, the concentration of CaCl2 is 0.05 molar (0.05 M CaCl2). The solution is also described as being 0.05 M Ca2+(aq) and 0.10 M Cl−(aq). The same solution could be referenced as [Ca2+] = 0.05 M. The circle represents a unit volume. It can be interpreted as “1 L”. Exploring the Model 12. What do the brackets [ ] mean? 13. Explain why the concentration of chloride is twice...
Question 9 Which would you NOT find in a solution of CaCl2(aq)? O H2O molecules Ca2+ ions CaCl, molecules CI ions For the reaction 2 KI + Pb(NO3)2 PbI, + 2 KNO; how many grams of lead(II) iodide, Pbl2, are produced from 35.7 g of potassium iodide, KI? mass of lead(II) iodide: g
If CaCl2 is dissolved in water, what can be said about the concentration of the Ca2+ ion?
Which one of the following expressions is correct for the representation of Ca2+ (aq) concentration involved in the solubility product (Ksp) of Ca3(PO4)2 in the presence of 0.10 M of Na3PO4: 1. [Ca2+] = (Ksp/0.010)1/2 2. [Ca2+] = (Ksp/0.010)1/3 3. [Ca2+] = (Ksp/0.0010)1/2 4. [Ca2+] = (Ksp/0.0010)1/3
QUESTION 30 Which one of the following expressions is the correct representation of Ca2+(aq) concentration involved in the solubility product (Ksp) of Ca3(PO4)2 in the presence of 0.10 M of Na3PO4 Ca2+)-(Ksp/0.010,12 Ca2)-(Ksp/0.101/2 Ca?)-(Ksp/0.001031/2 (Ca2+)-sp/0.01013 Ca2+)-sp/0.0010913
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq)0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq)0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq)Ca2+(aq) when Ag2SO4(s)Ag2SO4(s) begins to precipitate? Solubility-product constants, KspKsp, can be found in the chempendix. Ksp values : silver sulfat (1.20x10^-5) calcium sulfate (4.93x10^-5) [Ca2+]=
Calculate the concentration of ca2+, including activity coefficients, in a 0.08 M NaF solution saturated with CaF2. Ksp=3.2x10^-11 for CaF2, alphaCa2+=600 pm, alphaF-=350 pm.
A solution of Na3PO4 is added dropwise to a solution that is 0.0353 M in Ca2+ and 1.43e-08 M in A13+ The Ksp of Ca3(PO4)2 is 2.07e-33. The Ksp of AlPO4 is 9.84e-21. (a) What concentration of PO4 is necessary to begin precipitation? (Neglect volume changes.) [PO3) = (b) Which cation precipitates first? Ca A13+ (c) What is the concentration of PO43- when the second cation begins to precipitate? (PO43-] = M.
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________