Chemistry skill

Solve problems relating to precipitation

With this skill you will learn

Determine whether a precipitate will form
Separate ions by fractional precipitation
Determine whether a precipitate will form in a solution with an ionization equilibrium
Determine whether a precipitate will form in a solution containing complex ions
Control a concentration to cause or prevent precipitation from a solution of complex ions
Determine the solubility of a solute when complex ions form

Solve problems relating to precipitation Questions

Questions that need this skill to solve them

OC user

in Chemistry·

1 Sep 2020

A solution was created by dissolving 1.31 kg of Ba(NO₃)₂ into 1 L of 0.50 M Ca(NO₃)₂. Determine the concentration of SO₄^2- ion is needed to precipitate all of one molecule but leave the other molecule completely unreacted. Ksp (BaSO₄) = 1.08 * 10^-10, Ksp (CaSO₄) = 4.93 * 10^-5.

OC user

in Chemistry·

1 Sep 2020

Will CaSO₄ precipitate if 50 mL of 0.0010 M CaCl₂ is added to 50 mL of 0.010 M Na₂SO₄? (Ksp for CaSO₄ = 2.4 x 10^-5)

OC user

in Chemistry·

1 Sep 2020

The K_sp for strontium chromate is $3.6 \times 10^{}$ and the K_sp for barium chromate is $1.2 \times 10^{}$ . What concentration of potassium chromate will precipitate the maximum amount of either the barium or the strontium chromate from an equimolar 0.30 M solution of barium and strontium ions without precipitating the other?

OC user

in Chemistry·

1 Sep 2020

For the complex ion, [ $F e (H_{2} O)_{(a q)}^{}$ , the Ka = $7.7\times10 -3 at 298K$ . What is the pH of a 50 mL solution that contains 0.02 mols of $F e (N O_{3})_{2}$ ?

OC user

in Chemistry·

1 Sep 2020

If Cl⁻ is added to a solution that contains $0.025 M$ of $A g^{+}$ ions and $0.00448 M$ of $P b^{}$ ions. What concentration of $C l^{-}$ is required to precipitate each ion? $K_{(A g C l) = 1.8 \times 10^{}}$ and $K_{(P b C l_{2}) = 1.6 \times 10^{}}$ Which one will precipitate first?

$K_{s p} (P b C l_{2}) = 1.6 \times 10^{- 5}$

OC user

in Chemistry·

1 Sep 2020

The best explanation for the dissolution of ZnS in dilute HCl is that

OC user

in Chemistry·

1 Sep 2020

What is the best way to ensure complete precipitation of SnS from a saturated H2S solution?

OC user

in Chemistry·

1 Sep 2020

Cyanide ion forms very stable complex ions with a variety of metal ions. What is the molar equilibrium concentration of uncomplexed Ag⁺ in a solution that initially contains 1.3 mol of [Ag(CN)₂]^- per liter of solution . K_f[Ag(CN)2]^- = 4.5 * 10¹⁰

OC user

in Chemistry·

1 Sep 2020

Given the following equilibrium constants,

Zn(IO₃)₂ K_sp = 3.9 * 10^-6

Zn(NH₃)₄²⁺ Kf = 2.9 * 10⁹

Determine Kc for the dissolution of the sparingly soluble salt Zn(IO₃)₂ in aqueous ammonia as shown below:

OC user

in Chemistry·

1 Sep 2020

CO₂ absorbed from the air produced in the swimming pool to form a solution which comtains 2 * 10^-⁴ M [CO₃^2-]. If the pool water was originally 4 * 10^-³ M [Mg²⁺], 6 * 10^-⁴ M in [Ca²⁺] and 8 * 10^-⁷ M in [Fe²⁺], then a precipitate should form of:

OC user

in Chemistry·

1 Sep 2020

What is the pH of a saturated solution of Mg(OH)₂? ( Ksp = 5.61×10⁻¹²)

OC user

in Chemistry·

1 Sep 2020

A solution contains 0.05 M Au⁺, 0.05 M Cu⁺, and 0.05 M Ag⁺ ions. When solid NaCl is added to the solution, what is the order in which the chloride salts will begain to precipitate? Ksp(AgCl) = 1.8 * 10^-10, Ksp(AuCl) = 2.0 * 10^-13, Ksp(CuCl) = 1.9*10^-7

OC user

in Chemistry·

1 Sep 2020

AgCl would be least soluble at 298K in _____.

OC user

in Chemistry·

1 Sep 2020

Caclulate the equilibrium constant for the reaction: