# Chemistry Explanation??

So what would the explanation for this be? Its really confusing me.
The Ksp is independent of [NaOH] while the solubility of Ca(OH)2 decreases as the [NaOH] increases. Explain why this is the case.
( in the data table, the naoh concentration is 0 M, and the solubility is 2.30 x 10^-2, and ksp is around 5.5x10^-5; next table the concentration of naoh increases and the solubility and ksp go down)

1. 👍 0
2. 👎 0
3. 👁 195
1. Ca(OH)2 ==> Ca^2+ + 2OH^-
and Ksp = (Ca^2+)(OH^-)^2
Ksp is a constant. NaOH is a strong base and ionizes 100%; therefore, NaOH ==> Na^+ + OH^-. Le Chatelier's Principle tells you that when the OH^- increases, due to the NaOH, the Ksp equilibrium of Ca(OH)2 is forced to the left thereby decreasing the solubility of Ca(OH)2 in the solution.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

A solution is 5.0× 10–5 M in each of these ions: Ag , SO42–, Cl–, CO32– Which precipitate will form? Ag2SO4 (Ksp = 1.12× 10–5) AgCl (Ksp = 1.77× 10–10) Ag2CO3 (Ksp = 8.46× 10–12)

2. ### Chemistry

At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.56. What is the Ksp of the compound at 22 °C? I have found my [OH-] concentration

3. ### Chem 2

what is the solubility of silver carbonate in water in 25 degrees celcius if Ksp=8.4X10-12? i don't know what to do Write the equation. Ag2CO3(s) ==> 2Ag^+ + CO3^= Ksp = (Ag^+2)(CO3^=) Let x = solubility of Ag2CO3. At

4. ### Chemistry

Which of the following compounds has the greatest molar solubility? A) AgBr, Ksp= 5.4 x 10^13 B) Ba3(PO4)2, Ksp = 3.0 x 10^-23 C) Al(OH)3, Ksp = 1.9 x 10^-33 D) MgF2, Ksp = 7.4 x 10^-11 E) Pb(OH)2, Ksp = 1.2 x 10^-15 I know the

1. ### Chemistry

Calculate the solubility of Ag2CrO4 in a) 0.05M KClO4 b) 0.005M AgNO3 a) I have figured out: Ag2CrO4=2Ag- + CrO42- Ksp=1.12*10^-12. Ksp=[2Ag]^2*[CrO4] Ksp=(2x)^2(x) = 1.12*10^-12=4x^3= x=2.65*10^-5 (?) b)Ag2CrO4=2Ag- + CrO42-

2. ### AP Chem

What is the net ionic equation when NaOBr is dissolved in water and the Ksp if the Ksp of the dissocataion of HOBr is 6.4 * 10^-6

3. ### Chemistry

A solution contains 2.2×10−4 M Ag+ and 1.3×10−3 M If NaI is added, will AgI(Ksp=8.3×10−17) or PbI2(Ksp=7.9×10−9) precipitate first? I know the answer to this is AgI Specify the concentration of I− needed to begin

4. ### Chemistry

Calculate solubility of AgCl (in g/L) in a 6.5*10^-3 M silver Nitrate solution ksp= 1.8 * 10^-10 (AgCl molecular mass is 143.3g) any idea on how to do this this is what i tried> AgCl--> Ag + Cl I 6.5*10^-3 0 C same x E same x ksp

1. ### Chemistry

Approximately 1.5 10-3 g of iron(II) hydroxide, Fe(OH)2(s) dissolves per liter of water at 18°C. Calculate Ksp for Fe(OH)2(s) at this temperature. This is what I've done: 1.5x10^-3 g Fe(OH)2/L x 1mol Fe(OH)2/89.863g Fe(OH)2 =

2. ### chemistry

Most Soluble compound CuS, Ksp = 1.27 x10^-36 PbS, Ksp = 9.04 x 10^-29 AgCl,Ksp = 1.77 X 10^-10 AgI, Ksp = 8.51 x 10^17 My book states that AgCl is insoluble in water and so are MOST phosphates and Sufides, So am I reasonable to

3. ### Probability

Determine whether each of the following statements about events A,B,C is always true or not. 1. Suppose that A,B and C are independent events; then A^c (A complement) and B U C^c are independent. (T/F) 2. From now on, we do not

4. ### English

5. You can always go back to your old ways AFTER YOU HAVE BEEN HIRED. A) independent B) subordinate*** 6. IF YOUR WRITING SLANTS TO THE RIGHT, you are probably friendly & open. A) independent B) subordinate*** 7. If your writing