At some specific temperature, silver bromide, AgBr(s), has a measured solubility of 6.51×10-7M.
Calculate the Ksp value for AgBr(s) at this temperature.
At some specific temperature, silver bromide, AgBr(s), has a measured solubility of 6.51×10-7M. Calculate the Ksp...
13. Silver bromide (AgBr) is a light sensitive compound u mide (AgBr) is a light sensitive compound used in nearly all photographic film. The solubility of AgBr in water was measured to be 1.3 x 10-4 L at 25°C. Calculate Ksp for AgBr at that temperature. (5) +14. What is the molar solubility of AgCl in pure water at 25°C? Ksp =1.8 X 10 -10 (5) AgCl Aga + Cl - Kop 15. Will a precipitate oc CaSO4 form a...
Using Appendix D in the textbook, calculate the molar solubility of AgBr in 3.1×10−2 M AgNO3 solution. Silver bromide AgBr 5.0 * 10-13
Calculate the molar solubility of silver bromide in 0.010 M KBr solution.Ksp(AgBr )=5.4 × 10-13 ( ) 9.7 ×10-14mol/L ( ) 4.4 ×10-13mol/L ( ) 7.9 ×10-12mol/L ( ) 5.4 ×10-11mol/L
At 25 °C the solubility of silver bromide is 8.77 x 10' mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect).
Solid silver bromide (AgBr) will disassociate slightly in water to produce Agand Br". AgBr(s) + Agfaq) + Brīaq) Ksp = 1.3 x 10-5 a. Calculate the equilibrium concentration of Ag+ if the solution if the solid AgBr is dissolved in pure water. Assume that the solution is behaving ideally (y = 1) b. Now let's explore the reaction if we take into account non-ideal behavior. Calculate the concentration of Ag+ in solution if the solid if the AgBr is dissolved...
Consider the following information at 25 ºC: AgBr(s) + e- → Ag(s) + Br-(aq) Eº(AgBr(s),Ag(s)) = 0.07133 V Ag+(aq) + e- → Ag(s) Eº(Ag+(aq),Ag(s)) = 0.7996 V What is the value of the solubility product equilibrium constant Ksp(AgBr) of silver bromide? AgBr(s) ↔ Ag+(aq) + Br-(aq) Ksp(AgBr)
1) The solubility of Ni(OH)2 is measured and found to be 3.90×10-4 g/L. Use this information to calculate a Ksp value for nickel(II) hydroxide. Ksp = _______ 2) The solubility of Ag2CO3 is measured and found to be 3.58×10-2 g/L. Use this information to calculate a Ksp value for silver carbonate. Ksp = _________ 3) The mass of silver phosphate that is dissolved in 250 mL of a saturated solution is _____grams. 4)The mass of silver bromide that is dissolved...
Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 3.50×10-16 at a specific temperature.
1a) Silver chromate, Ag2CrO4, has a Ksp of 8.99 × 10–12. Calculate the solubility in mol/L of silver chromate. 1b) Calculate the molar solubility of AgCl (Ksp = 1.6 × 10–10) in 0.0034 M sodium chloride at 25°C. 1c) If 30 mL of 5.0 × 10–4M Ca(NO3)2 are added to 70 mL of 2.0 × 10–4M NaF, will a precipitate occur? (Ksp of CaF2 = 4.0 × 10–11)
The Ksp for lead bromide (PbBr2) is 4.6 x 10-6. Calculate the solubility of lead bromide in each of the following. a. water mol/L Solubility=[ b. 0.16 M Pb(NO3)2 Solubility = mol/L c. 0.016 M NaBr Solubility = mol/L