The Ksp of PbBr2 is 6.60*10^-6
What is the molar solubility(M) of PbBr2 in pure water?
What is the molar solubility(M) of PbBr2 in 0.500M KBr
solution?
What is the molar solubility(M) of PbBr2 in a 0.500M Pb(NO3)2
solution?
Solubility:
Solubility is defined as the maximum quantity of solute dissolved in a given amount of solvent to make a saturated solution at a particular temperature.
Molar solubility:
Molar solubility is the number of moles of a solute that can be dissolved in one liter of a solution. It is expressed as mol/L or M (molarity).
Common ion effect:
Common ion effect is defined as the solubility of a partially soluble salt which will decrease with the addition of a soluble salt that has an ion in common with it.
Consider a general reaction:
The relation between solubility product and molar solubility is as follows:
Where,
Solubility product =
Molar solubility of M ion =
Molar solubility of X ion =
Therefore, the molar solubility (M) of in pure water is
.
Therefore, the molar solubility (M) of in
is
.
Therefore, the molar solubility (M) of in
is
.
The molar solubility (M) of in pure water is
.
The molar solubility (M) of in
is
.
The molar solubility (M) of in
is
.
The ksp of pbbr2 is 6.60 10 6. What is the molar solubility(M) of PbBr2 in pure water?
The Ksp of PbBr, is 6.60 x 10-6. What is the molar solubility of PbBr, in pure water? molar solubility: What is the molar solñbility of PbBr, in 0.500 M KBr solution? molar solubility: What is the molar solubility of PbBr, in a 0.500 M Pb(NO,), solution? molar solubility:
1. a.) What is the molar solublitlity of PbBr2 in pure water? Ksp of PbBr2=4.67*10^-6 b.) How does thee molar solubility of PbBr2 change when you try to dissolve it in a 0.10 M solution of KBR?
Q. Given that the solubility product of PbBr2 is 6.200×10-6 determine the molar solubility of PbBr2: a) In pure water: b)In a 0.201 M KBr solution: c)In a 0.364 M Pb(NO3)2 solution:
Q. Given that the solubility product of PbBr2 is 6.200×10-6 determine the molar solubility of PbBr2: a) In pure water: b)In a 0.201 M KBr solution: c)In a 0.364 M Pb(NO3)2 solution:
The Kp of PbBr, is 6.60 x 10 What is the molar solubility of PbBr, in pure water? molar solubility: м What is the molar solubility of PbBr, in 0.500 M KBr solution? molar solubility: M What is the molar solubility of PbBr, in a 0.500 M Pb(NO,) solution? molar solubility: м
The K., of PbBr, is 6.60 x 10-6 What is the molar solubility of PbBr, in pure water? molar solubility: What is the molar solubility of PbBr, in 0.500 M KBr solution? molar solubility: What is the molar solubility of PbBr, in a 0.500 M Pb(NOx), solution? molar solubility:
HCM The K., of PbBr, is 6.60 x 10-6. What is the molar solubility of PbBr, in pure water? molar solubility: 1.18 x10-2 What is the molar solubility of PbBr, in 0.500 M KBr solution? molar solubility: What is the molar solubility of PbBr, in a 0.500 M Pb(NO), solution? molar solubility:
he solubility product (Ksp) of PbBr2 is 8.9 X 10. Please calculate the molar solubility in: A) Pure water B) 0.20 M Pb(NOs)2 Pb Brs) Pbap +2 Br 8.9- M0T 2 LOZJLES . 45 25 O.Zts Zs 4.45./05 4 4s 0.2x0.2+s 13:105- J S0-60334 9. The solubility of an ionic compound MX (molar mass = 346 g/mol) is 4.63 X 103 g/L. What is the Ksp for this compound? HoW
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
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...