Question

Calculate the solubility of **MnCO _{3}**
(a) in pure water and (b) in a solution in which
[

Solubility in pure water = ______M Solubility in |

Answer #1

**The Ksp of manganese(II) carbonate, MnCO3, is
2.42*10^-11**

**a)**

**At equilibrium:**

**MnCO3 ----> Mn2+ + CO32-**

** s s**

**Ksp = [Mn2+][CO32-]**

**2.42*10^-11=(s)*(s)**

**2.42*10^-11= 1(s)^2**

**s = 4.92*10^-6 M**

**Answer: 4.92*10^-6 M**

**b)**

**[CO32-] = 0.285 M**

**At equilibrium:**

**MnCO3 ----> Mn2+ + CO32-**

** s 0.285 + s**

**Ksp = [Mn2+][CO32-]**

**2.42*10^-11=(s)*(0.285+ s)**

**Since Ksp is small, s can be ignored as compared to
0.285**

**Above expression thus becomes:**

**2.42*10^-11=(s)*(0.285)**

**2.42*10^-11= 1(s)^1 * 0.285**

**s = 8.49*10^-11 M**

**Answer: 8.49*10^-11 M**

Calculate the solubility of NiCO3
(a) in pure water and (b) in a solution in which
[CO32-] =
0.283 M.
*Ksp NiCO3 = (6.6 × 10-9)
Solubility in pure water = ______M
Solubility in 0.283 M
CO32- = ______M

Calculate the solubility at 25°C of CoOH2 in pure water
and in a 0.0050M CoCl2 solution.
(Ksp = 5.92 x 10^-15)
Round both of your answers to 2 significant digits
Solubility in pure water? g/L
Solubility in 0.0050 M CoCl2 solution? g/L

A.) Calculate the solubility in g/L of AgBr in pure water.
B.) Calculate the solubility in g/L of AgBr in 0.0018 M NaBr.
(Enter answer in scientific notation.)

2. Calculate the molar solubility of the following:
a. AgCl added to pure water
b. AgCl added to water that is already 0.25 M Cl-

Calculate the solubility at 25 Celsius of CuBr in pure water and
in 0.071 M NaI. Round your answer to 2 significant digits.
Solubility in pure water:
Solubility in 0.071 M NaI:
CuBr: 6.27 x 10^-9

The molar solubility of AgBr in pure water is 7.3x10^-7 M.
Calculate the Ksp.

A. Calculate the solubility (in grams per 1.00×10^2mL of
solution) of magnesium hydroxide in a solution buffered at
pH=11
B. Calculate the solubility (in grams per 1.00×10^2mL of
solution) of magnesium hydroxide in pure water.
C. How does the solubility of Mg(OH)2 in a buffered solution
compare to the solubility of Mg(OH)2 in pure water?

Determine the g/100 mL solubility of calcium hydroxide:
(a) in pure water. (4 pts)
(b) in a solution of sodium hydroxide, pH
= 12.8.

A) Calculate the solubility (in grams per 1.00×102mL of
solution) of magnesium hydroxide in a solution buffered at
pH = 10.
B)How does this compare to the solubility of Mg(OH)2 in pure
water?

What is the molar solubility of plumbous sulfate in a) pure
water; and b) in 0.0500 M plumbous nitrate? Ksp plumbous sulfate =
1.6x10-8

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