Question
In: Chemistry
A water sample contains 1.00*10-4 mass% silver nitrate. Silver chloride's solubility product is Ksp(AgCl) = 1.82*10-10...
A water sample contains 1.00*10-4 mass% silver nitrate. Silver chloride's solubility product is Ksp(AgCl) = 1.82*10-10
a) How much volume of 1,000 M sodium chloride solution must be added to 1.00 L of the solution in order for 90.0% of the silver to precipitate as silver chloride?
b) What is the mass of the precipitated silver chloride?
Solutions
Expert Solution
Volume of NaCl required and mass of AgCl precipitated is calculated as follows -
queen_honey_blossom answered 1 year agoRelated Solutions
Solubility products for AgCl and AgI are: Ksp(AgCl) = 1.82*10-10 Ksp(AgI) = 8.31*10-17 0.010 moles of...
Solubility products for AgCl and AgI are:
Ksp(AgCl) = 1.82*10-10
Ksp(AgI) = 8.31*10-17
0.010 moles of AgCl is added to 100 mL of water, then 0.020
moles of NaI is added. What are the concentrations of Cl and Ions
at equilibrium?
a) Calculate the solubility of silver chloride (AgCl) in a 6.5x10^-3 M silver nitrate (AgNO3) solution....
a) Calculate the solubility of silver chloride (AgCl)
in a 6.5x10^-3 M silver nitrate (AgNO3) solution.
b) Which of the following compounds will be more soluble in acidic
solution than in water:
a) CuS b) AgCl c) PbSO4 ?
a) The solubility product for PbCl2 is 1.6 ∙ 10-5. The solubility product for AgCl is...
a) The solubility product for PbCl2 is 1.6 ∙ 10-5. The
solubility product for AgCl is 1.6 ∙ 10-10. How does the solubility
of lead chloride in a 0.10 M AgNO3 solution compare to the
solubility in pure water? Will it be higher, lower og not
changed?
Please explain your answer briefly as I dont get it.
b) The solubility of a salt MX is 1.1 ∙ 10-3 mol / L. What is
the solubility product Ksp for the salt?
Solid Silver chloride has an extremely low solubility in water. Calculate the molar solubility of AgCl...
Solid Silver chloride has an extremely low solubility in water.
Calculate the molar solubility of AgCl in a mixture of AgCl(s) and
0.08 M NaCl(aq). Ksp = 1.8 × 10-10
Part 1: The Ksp for silver chloride (AgCl) is 1.77 × 10−10. Which of the following...
Part 1: The Ksp for silver chloride (AgCl) is 1.77 × 10−10.
Which of the following represents the Ksp expression for this
substance?
A Ksp = [AgCl]/[Ag+][Cl-]
B Ksp = 1/[Ag+][Cl-]
C Ksp = [Ag+][Cl-]
D Ksp = [Ag+][Cl-]/[AgCl]
The answer was C
Part 2: You add 72.0 mL of a 0.472 M AgNO3 solution to 127.1 mL
of a 0.114 M NaCl solution. Determine the concentration of Ag+ and
Cl- ions in solution as if all remain dissolved. After,...
The solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass of KCl(s) must be...
The solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass
of KCl(s) must be dissolved in 150.00 mL of 1.15M Pb(NO3)2 to
produce a solution that is just saturated in PbCl2?
(a) The solubility product, Ksp, of Sn(OH)4(s) is 1.0 x 10-57. What is its solubility (in...
(a) The solubility product, Ksp, of
Sn(OH)4(s) is 1.0 x 10-57. What is its
solubility (in g/L) in an aqueous solution of NaOH with a pH of
12.80 ? The temperature is 25oC.
(b) For the reaction 2 A(g) ⇋ 3 B(g) + 2 C(g), we start off with
just pure A(g) (there is no B(g) or C(g)). When we reach
equilibrium, the partial pressure of C(g) is 4.19 atm. The
equilibrium constant for this reaction is 8.39 . What...
The Ksp for silver sulfate (K2SO4) is 1.2*10-5. Calculate the solubility of silver sulfate in each of the following situations:
Chemical Equilibrium PracticeThe Ksp for silver sulfate (K2SO4) is 1.2*10-5. Calculate the solubility of silver sulfate in each of the following situations: a. Molar solubility (mol/L) of silver sulfate in pure water. b. Molar solubility of silver sulfate in a 0.10 M solution of AgNO3 (ag). c. Molar solubility of silver sulfate Tn a 1.00 M solution of AgNO3(ag). d. Solubility of silver sulfate in pure water in grams per 100 ml of water. e. Moral solubility of silver sulfate in a 0.43 M solution...
Calculate the molar solubility of silver bromide. The Ksp of AgBr is 7.7 x 10-13. The...
Calculate the molar solubility of silver bromide. The Ksp of
AgBr is 7.7 x 10-13. The Kf of Ag(NH3)2+ is
1.5 x 107.
a) in water
b) in a solution of 1.0M NH3.
ANS: a) 8.8 x 10-7 M b) 3.4 x 10-3 M
I make threesaturated solutions of AgCl (Ksp= 1.8•10-10). The first is in pure water, the second...
I make threesaturated solutions of AgCl (Ksp= 1.8•10-10). The
first is in pure water, the second is in 0.01 M KNO3, and the third
is in 0.01 M NaCl. I measure the concentration of Ag+in each
solution. Which has the highest Ag+concentration? Which has the
lowestAg+ concentration? Please explain why there are differences
in concentrations between the solution with the highest and lowest
concentrations. I’m not asking for the actual concentration, so you
don’t need to do any math.highest:
_________________________________lowest:...
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