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In this experiment we will be using a 0.050 M solution of HCl to determine the concentration of hydroxide (OH-) in a saturated solution of calcium hydroxide. The initial volume of "filtered" calcium hydroxide solution used in this example will be 36.0 mL. If it takes 16 mL of the HCl solution to reach the equivalence point of the titration, how many moles of OH- were present in this sample of calcium hydroxide?

How many moles of Ca2+ ?

Recall, the values used to determine Ksp values are concentrations. Considering the initial volume of calcium hydroxide was 36 ml, the concentration of OH- is

, and the concentration of Ca2+ is

Using these values, what is the Ksp of calcium hydroxide according to this data?

Report all your answers in scientific notation.

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mickymike92

Based on the definition of equivalence point and the data provided;

  • the moles of OH- present is 0.0008 moles
  • the moles of Ca2+ present is 0.0004 moles.
  • The Ksp of calcium hydroxide 5.324 × 10^-8

What is equivalence point of a reaction?

The equivalence point of a reaction is the point at which equal amounts of both acid and base have reacted.

Equation of the reaction is as follows:

HCl + Ca(OH)2 ---> CaCl2 + 2 H20

Moles of HCl reacted = molarity × volume in L

Moles of HCl reacted = 0.05 M × 16/1000 = 0.0008 moles

Therefore, moles of OH- present = 0.0008 moles

Also, moles of Ca2+ present = 0.0008/2 = 0.0004 moles

The molar solubility product Ksp of calcium hydroxide is calculated as follows.

  • Ksp = [Ca2+]^2 × 2 × [OH]

volume of solution = 36 mL = 0.036 L

[Ca2+] = 0.0004 / 0.036 = 0.011 M

[OH] = 0.0008 / 0.036 = 0.022 M

Ksp = (0.011)^2 × 2(0.022)

Ksp = 5.324 × 10^-8

Therefore, the moles of OH- present is 0.0008 moles and the moles of Ca2+ present is 0.0004 moles.

The Ksp of calcium hydroxide 5.324 × 10^-8

Learn more about equivalence point at: https://brainly.com/question/24584140

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