What is the common ion effect and how may the common ion effect be used to...

What is the common ion effect and how may the common ion effect be used to prevent the dissolution of certain sparingly soluble salts into water solution? Calculate the concentration of CaF2 in 0.002 M KF.

Expert Solution

1)
Common ion effect is decrease in solubility of a sparingly soluble salt in presence of a common ion
For example when we mix CaF2 with KF
CaF2 dissolves as:
CaF2 <----> Ca2+ + 2 F-

when we add KF, we are adding more of F-. This is adding a prduct in equilibrium. So, equilibrium shifts to reactant side hence decreasing the solubility

2)
KF here is Strong electrolyte
It will dissociate completely to give [F-] = 0.002 M
At equilibrium:
CaF2 <----> Ca2+ + 2 F-
s 2*10^-3 + 2s
Ksp = [Ca2+][F-]^2
3.45*10^-11=(s)*(2*10^-3+ 2s)^2
Since Ksp is small, s can be ignored as compared to 2*10^-3
Above expression thus becomes:
3.45*10^-11=(s)*(2*10^-3)^2
3.45*10^-11= (s) * 4*10^-6
s = 8.625*10^-6 M
Answer: 8.6*10^-6 M

queen_honey_blossom answered 2 years ago

± Common-Ion Effect on Solubility for Lead Thiocyanate Lead thiocyanate, Pb(SCN ) 2 Common-Ion Effect Consider...

± Common-Ion Effect on Solubility for Lead Thiocyanate Lead thiocyanate, Pb(SCN ) 2 Common-Ion Effect Consider the dissolution of AB(s) : AB(s)⇌A+(aq)+ B − (aq) Le Châtelier's principle tells us that an increase in either [ A + ] or [ B − ] will shift this equilibrium to the left, reducing the solubility of AB . In other words, AB is more soluble in pure water than in a solution that already contains A + or B − ions....

What is common ion effect? Explain it through H2PO4 - (aq) + H2O(l) ⇋ H3O +...

What is common ion effect? Explain it through H2PO4 - (aq) + H2O(l) ⇋ H3O + (aq) + HPO4 2- (aq

What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the...

What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the following are added to a basic buffer solution of equal concentrations of ammonia and ammonium nitrate: a) KI b) NH3 c) HI d) NaOH e) NH4Cl. Can you explain what happens to the ammonium nitrate--is it ignored?

1.In gravimetric analysis, it is possible to use the common-ion effect to favor the production of...

1.In gravimetric analysis, it is possible to use the common-ion effect to favor the production of solid precipitate. In this problem you will test this approach to see how effective it is for the gravimetric determination of calcium. Suppose the reaction flask in the gravimetric analysis experiment contains 175 mL of solution before filtering through the Gooch crucible. A precipitate of calcium oxalate monohydrate is collected in the crucible and dried, where: CaC2O4 * H2O <--> Ca2^+ + C2O4^2- +...

The Common Ion Effect: Calculation of pH. When a weak, nitrogen base is protonated, the resulting...

The Common Ion Effect: Calculation of pH. When a weak, nitrogen base is protonated, the resulting conjugate acid is given the "ium" suffix to show that it has been protonated and has an overall +1 charge. Thus, the weak base ammonia is protonated to form the ammonium (NH4+) cation. What is the pH of a 0.68 M solution of (CH3)2NH that is also 0.65 M in dimethylammonium sulfate, the salt of it's conjugate acid? The Kb for (CH3)2NH = 5.4...

The common-ion effect and solubility The solubility of a slightly soluble compound can be greatly affected...

The common-ion effect and solubility The solubility of a slightly soluble compound can be greatly affected by the addition of a soluble compound with a common ion, that is, with one of the ions in the added soluble compound being identical to one of the ions of the slightly soluble compound. The general result of the addition of the common ion is to greatly reduce the solubility of the slightly soluble compound. In other words, the addition of the common...

Read up on the phenomenon called the common ion effect in your text. You add a...

Read up on the phenomenon called the common ion effect in your text. You add a small amount of NaOH to a test tube containing cadmium nitrate solution. Initially nothing happens, but as you add more NaOH you begin to observe the formation of a white, powdery solid that resembles snowflakes. Eventually, all the precipitate settles to the bottom of your test tube. a. Explain why you do not see the precipitate initially as you first begin to add NaOH...

The Common-Ion Effect and pH Buffers 1. Calculate the pH at 25°C of 1.00 L of...

The Common-Ion Effect and pH Buffers 1. Calculate the pH at 25°C of 1.00 L of a buffer that is 0.120 M HNO2 and 0.150 M NaNO2 before and after the addition of 1.00 mL of 12.0 M HCl. pH Indicators and Acid–Base Titrations 2. A 25.0 mL sample of 0.100 M acetic acid is titrated with 0.125 M NaOH. Calculate the pH at 25°C of the titration mixture after 10.0, 20.0, and 30.0 mL of the base have been...

Depending on the sample of interest, different ion sources are used for mass spectrometry. What ion...

Depending on the sample of interest, different ion sources are used for mass spectrometry. What ion source would you use if you wanted to examine many different small molecules and compare your results to a large database? Why?

What are the benefits that common stockholders may receive? How do common stock and preferred stock...

What are the benefits that common stockholders may receive? How do common stock and preferred stock differ? Discuss the similarities between preferred stock and debt. Why do corporations utilize different forms of equity?

Question