What is the molar solubility of manganese sulfide? M
What is the concentration of manganese ions in a saturated solution of manganese sulfide? M
Manganese | |
---|---|
Mn(OH)2 | 1.9 x 10-13 |
MnCO3 | 8.8 x 10-11 |
MnS | 5.6 x 10-16 |
MnS ------------------------> Mn+2 + S-2
S S
Ksp = [Mn+2][S-2]
Ksp = S^2
5.6 x 10^-16 = S^2
S = 2.37 x 10^-8 M
molar solubility = 2.37 x 10^-8 M
concentration of Mn ion in MnS = 2.37 x 10^-8 M
What is the molar solubility of manganese sulfide? M What is the concentration of manganese ions...
The solubility of manganese(ii) sulfide in a 0 274 M sodium sulfide solution is ksp value for MnS is 3x10^-11
RUESLIon (points) For manganese(II) hydroxide, Mn(OH)2, Ksp = 1.6 x 10-13. Calculate the molar solubility of Mn(OH)2 in a solution that contains 0.158 M NaOH. (Hint: this involves calculating the effect of a common ion on solubility.)
The value for Ksp for manganese (II) hydroxide (Mn(OH)2) is 1.6x10^-13. Calculate the molar solubility of Mn(OH)2 in a solution containing 0.020M NaOH
1. A solution contains 8.68×10-3 M sodium hydroxide and 6.04×10-3 M ammonium sulfide. Solid manganese(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of manganese(II) ion when this precipitation first begins? [Mn2+] = M 2. A solution contains 5.04×10-3 M magnesium nitrate and 1.31×10-2 M nickel(II) acetate. Solid sodium hydroxide is added slowly to this mixture. A. What is the formula of...
1.
Using Table 38.3 in the Voyce text, calculate the solubility of
Manganese(II) hydroxide at 25oC
A.
5.7 x 10-5
B.
3.6 x 10-5
C.
4.4 x 10-7
2.
The pH of a 0.0147M KCN solution is:
A.
10.7
B.
5.52
C.
3.3
D.
8.48
3.
The pH of a buffer solution composed of 0.020M HCHO2
and 0.014M NaCHO2 is:
A.
3.59
B.
3.74
C.
3.90
4.
When 400ml of a 0.01M SnCl2 solution is mixed with a
300ml if...
21. What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at 25 °C? The Ksp of Mn(OH)2 is 1.9 x 10- at 25 °C. The concentration of Pb in an aqueous solution is 5.5 x 103 M. What concentration of SO required to begin precipitating PbSO? The Ksp of PbSOa is 2.5 x 10 is 22. must be added to 1,0 L of 0.0180 M Pb2 (aq) to 23. What mass of KCl...
Calculate the solubility product constant, Ksp, for Chromium(III) Hydroxide (Cr(OH)3) which has a solubility of 1.27 x 10-6g/L. 7.0 x 10-23 6.3x10-31 1.87 x 10-24 2.31 x 10-32 3.6 x 10-31 How is the molar solubility (s) of Tin(II) hydroxide related to Ksp? s = (Ksp) 1/2 s-(Ksp/4)1/3 s = (Ksp/108)1/5 s = (Ksp/9)1/3 s = (Ksp/27)1/4 Calculate the concentration of OH ions in a saturated solution of Manganese (1) hydroxide, Mn(OH)2 Ksp for Mn(OH)2 = 4.6 x 10-14 (Report...
1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility calculated in problem 2. Explain the cause of the difference.
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar solubility in mol/L for Zn(OH): in water. Zn(OH): has a Kap value of 1.8 x 10. Also, fill in the provided ICE table in solving this problem. Zn(OH)2(s)Zn2 (ag)20H (aq) Initial concentration (M Change in concentration (M) Equilibrium concentration (M From the molar solubility in question 1, calculate the concentration of OH ions in solution, and the pH of the solution. . Two 10.0...
A student measures the molar solubility of silver sulfide in a water solution to be 2.99x10-17 M. Based on her data, the solubility product constant for this compound is A student measures the so-concentration in a saturated aqueous solution of calcium sulfate to be 5.03x10-3 M. Based on her data, the solubility product constant for calcium sulfate is