Calculate Ksp of a salt, M2S, where M is a +1 metal. It's solubility is 5.13 x 10-6 M
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Calculate Ksp of a salt, M2S, where M is a +1 metal. It's solubility is 5.13...
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 ?
7.Calculate the molar solubility for the binary salt MX3 with Ksp=0.0000071. Enter your answer as a decimal number with two significant figures. 8.Calculate the molar solubility of the binary salt MX2 with Ksp=0.000016. Enter your answer as a decimal with two significant figures. 9. Calculate the molar solubility of MX2 (Ksp=0.0000011) in 0.085 M NaX. Enter your answer as a decimal with two significant figures. 10.Determine the molar solubility of MX (Ksp=4.2x10-8) in 0.083 M NaCN. The metal ion M+...
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 ?
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...
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
Complete Table 1:
Ksp data
Salt
[cation] (M)
[anion] (M)
molar solubility (M)
Ksp
AgCl
SrSO4
Ag2CO3
Sr(IO3)2
1) Rank the salts in order of increasing molar solubility.
2) Rank the salts in order of increasing Ksp
(remember 10–10 < 10–5)
3) If these rankings are not in the same order, why might
Ksp not always scale directly with molar solubility?
Design experiments in the virtual lab to answer the follow questions, 1). Use the virtual lab to determine the...
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z. a. 2.9 x 10-5 M b. 5.7 x 10-5 M c. 9.4 x 10-5 M d. 3.7 x 10-5 M
Calculate the molar solubility for Pb3(PO4)2 given that Ksp for this salt = 1.0 x 10-57
The molar solubility of Ag(CH3COO) at 298K is 6.6332×10-2 M. Determine the Ksp of this salt. The Ksp of Cu(OH)2 at 298 K is 1.60×10-19. Determine the molar solubility of this salt. How many grams of CaF2 (molar mass = 78.077) will dissolve in 400 mL of 0.60 M NaF solution? The Ksp for CaF2 is 3.8904e-11.
The solubility product for an insoluble salt with the formula
ML2 is writen as ___, where x is the molar solubility.
, where x is the molar The solubility product for an insoluble salt with the formula ML is written as solubility. K-274 0 Ksp 4x² Ksp 2x² Not enough information Kyp=108x5