Considering the solubuility of copper(II) tartrate, which of the following are examples of the common ion...

Considering the solubuility of copper(II) tartrate, which of the following are examples of the common ion effect?

A		addition of copper(II) choride increases the solubility of copper(II) tartrate
B		addition of sodium tartrate causes copper(II) tartrate to precipitate
C		addition of sulfuric acid increases the solbility of copper(II) tartrate
D		addition of copper(II) sulfate causes copper(II) tartrate to precipitate

Expert Solution

B) Addition of sodium tartarate causes copper(II)tartarate to precipitate

D) Addition of copper(II)sufate causes copper(II)tartarate to precipitate

Explanation

Solubility equillibrium of Copper(II)tartarate is

Copper(II)tartarate(s) <-------> Copper(II)(aq) + tartarate(aq)

Equillibrium expression for this equillibrium is

Ksp = [Copper(II)][tartarate]

So, addition of either Copper(II) ion or tartarate ion should move the equillbrium to the left to maintain the Ksp value constant.Thus ,the solubility of Copper(II)tartarate decreasing by adding either Copper(II) ion or tartarate ion.

In B, tartarate ion is added as common ion , so ,the solubility of Copper(II)tartarate is decreasing

In D, copper(II) ion is added as common ion ,so, the solubility of copper(II)tartarate is decreasing

queen_honey_blossom answered 2 years ago

In the determination of the solubility for copper (II) iodate, what common ion of the same...

In the determination of the solubility for copper (II) iodate, what common ion of the same concentration (for example, 0.010 M Cu2+ or 0.010 M IO3-) would have a greater effect on reducing the solubility of Cu(IO3)2? Why?

Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex...

Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , Kf = 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). + + K =

1) The molar solubility of copper(II) sulfide in a 0.266 M copper(II) acetate solution is _______ M.

1) The molar solubility of copper(II) sulfide in a 0.266 M copper(II) acetate solution is _______ M. 2) The maximum amount of cobalt(II) carbonate that will dissolve in a 0.258 M cobalt(II) nitrate solution is _______ M.

In the reaction of copper with potassium permanganate and sulfuric acid, the products are copper (II)...

In the reaction of copper with potassium permanganate and sulfuric acid, the products are copper (II) sulfate, potassium sulfate, water, and manganese (II) sulfate. First, write a balanced net ionic equation for this reaction. Then consider the reaction taking place with 100 grams of copper, 100 grams of potassium permanganate, and 400 grams of sulfuric acid. How many grams of manganese (II) sulfate could be produced in this reaction?

Consider 1.00 g sample of copper (II) nitrate trihydrate. How many moles of copper (II) nitrate...

Consider 1.00 g sample of copper (II) nitrate trihydrate. How many moles of copper (II) nitrate trihydrate formula units are present in this sample? How many moles of nitrate ion are present in the sample? What mass in grams of water is present in this sample? How many oxygen atoms are present in this sample?

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.

3.1. Carefully explain the following observations: (i) Silver dissolves poorly in copper at 100°C. (ii) Copper...

3.1. Carefully explain the following observations: (i) Silver dissolves poorly in copper at 100°C. (ii) Copper dissolves poorly in silver at 100°C. (iii) The amount of copper (in atom per cent) that can dissolve in silver at 100°C is greater than the amount of silver (in atom per cent) that can dissolve in copper at 100°C.

a 0.1965g sample containing copper is analysed iodometrically. copper(ii) is reduced to copper(i) by iodide: 2Cu2+...

a 0.1965g sample containing copper is analysed iodometrically. copper(ii) is reduced to copper(i) by iodide: 2Cu2+ + 4I- --> 2Cul + I2 calculate the percentage of copper in the sample if 25.0mL of 0.1005M Na2S2O3 is required for the titration of the liberated iodine.

12.0 g of copper is concerted to copper (II) oxide by heating in oxygen. Write a...

12.0 g of copper is concerted to copper (II) oxide by heating in oxygen. Write a balanced equation for this reaction. What mass of oxygen is required to convert the 12.0 g of copper into copper (II) oxide? What mass of copper (II) oxide will theoretically be produced? What is the percent yield of copper (II) oxide if 12.8 g of copper (II) oxide is actually produced?

There are two possible methods for recovering copper from a solution of copper (II) sulfate, one...

There are two possible methods for recovering copper from a solution of copper (II) sulfate, one uses precipitation and the other uses redox. Copper(II) ions can be precipitated as copper(II) carbonate. CuSO4(aq) + Na2CO3(aq) → CuCO3(s) + Na2SO4(aq) How many mL of 0.363 M Na2CO3 would be needed to precipitate all of the copper ions in 47.0 mL of 0.323 M CuSO4? mL How many grams of CuCO3(s) would be formed from the copper ions in 47.0 mL of 0.323...

Question