M represents a trivalent metal, X represents a singly-charged anion. The solubility of Mx, is 2.501...
M represents a monovalent metal, X represents a doubly-charged anion. The K, of MX, is 5,449 x 10 Compute the concentration of a saturated M,X solution in mol/L.
Suppose we have a salt of low solubility, "MX", X- represents a non-metal anion M+ represents a metal cation. We then employ a voltaic cell with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.355 V. Calculate Ksp of "MX" at 25°C
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.429 V. What is the Ksp of "MX" at 25°C ? Remember: if you want to express...
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.251 V. What is the Ksp of "MX" at 25°C ?
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.186 V. What is the Ksp of "MX" at 25°C ?
What is the molar solubility of AgI in a solution which is 5.1 x 10-4 M in AgNO3? For AgI, Ksp = 8.3 x 10-17. A. 5.1 x 10-2 mol/L B. 4.2 x 10-20 mol/L C. 1.6 x 10-13 mol/L D. 1.1 x 10-5 mol/L E. 8.3 x 10-11 mol/L
addio X4 (9 10. The Kip of Agl is 1.5 x 10-16. Calculate the solubility in mol/L of Agl in a 0.30 M Nal solution. A) 4.5 x 10-17 KS p = Ag+ B) 0.30 I C) 1.5 x 10-6 x+0.30 D) 1.2 x 10 E) 5.0 x 10-16 The following questions (11, 12, 13) refer to the following system: 3.5 x 10 mL of 3.2 M Pb(NO3)2 and 2.0 x 10 mL of 0.020 M NaCl are added together....
Bral -6.3 x 102 M & (Br)-1.2 x10 M. What are the equilibrium concentrations of Br, & Br at 1280C where K, 1.1 x 10'? Show ALL work (hint: test Q first) 9) Calculate (CoL,[Ch] & [COCk] when 5.00 mol COCI, decomposes&reaches equilibrium in 10.Ol flask. K 8.3 x 10* at 360°C 10) Reaction of 0.1050 mol PCl, w/0.0450 mol Cl, & 0.0450 mol PCl, in 0.5000 L flask. K, 4.2 x 10 at 250°c a) Which direction will rxn...
[References) Calculate the molar solubility of Ag, SO4 in pure water. Ksp (Ag, 504) = 1.7 x 10-5 Molar solubility = 1 mol/L Calculate the molar solubility of Ag, SO4 in 0.022MAgNO3. Molar solubility = mol/L Calculate the molar solubility of Ag, SO4 in 0.022MK2SO4. Molar solubility = mol/L APPENDIX Solubility Product Constants for Some Inorganic Compounds at 25°C Substance K Substance 1.6 x 10-16 1.9 X 10-33 1.3 x 10-30 7.8 x 10-21 6.7 X 10-11 24 X 10-...
please help me with all the steps. 15. Which of the following mixtures would result in a buffered solution? a. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NaOH. b. Mixing 100.0 mL of 0.100 M NH3 (K5=1.8 x 10-5) with 100.0 mL of 0.100 M NaOH. c. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NH; (K =18x 10 %. d. Mixing 50.0 mL of 0.100 M HCl with...