Solubility
Solubility
Acids and Bases
Acids and Bases
Acids and Bases
100

What is the solubility of silver chloride (AgCl) in pure water?

  • 1.34×10−5M
100

Without solving, predict if PbI2 will be more soluble in

a) Pure water

or

b) KI

And why?

Water

100

HIO3

Acid or Base? Strong or Weak?

weak acid

100

Which is the weaker base? NO2- or HSO4-

HSO4-

100

True or False?

“All Bronstend-Lowry acids are Arrhenius acids”

False

200

The solubility of calcium fluoride (CaF₂) is 0.015 M at 25 °C. What is the Ksp at this temperature?

  • 1.35×10−5
200

If 10.0 mL of 0.0010 M CaCl₂ are added to 40.0 mL of 0.0010 M Na₂CO₃, will there be any precipitation observed?

No

200

Identify the acid, base, conjugate acid, and conjugate base? Also identify the classification(s) of acids/bases present. 

H2SO4+H2O→H3O++HSO4−

  • Acid:H2SO4  BL, A, Lewis
  • Base: H2O BL, Lewis
  • Conjugate acid:  H3O+
  • Conjugate base: HSO4-
200

What are the pH and pOH of a 0.025 M NaOH solution?

  •  pOH= 1.6
  • pH = 12.4
200

If you take 5.0 mL of 0.015 M HNO₃ and dilute it to 100.0 mL, what is the pH?

3.12

300

The solubility of barium iodide (BaI₂) is 0.020 M at 25 °C. What are the concentrations of the cation and anion at equilibrium?

  • [Ba2+]=0.020M, [I−]=0.040M
300

Calculate the molar solubility of solid CaF₂ in a solution of 0.30 M CaCl₂.Will this solution result in more reactants or products (compared to pure water)?

  • More reactants
  • 5.7x10^-6 M
300

Determine if there will be more products or reactants for the reaction below, must use Kb values to prove your answer.

CN- + HCOOH --> HCN + HCOO-

more products

300

What are [H+], [OH-], and pOH in a solution with a pH of 5.25?

  •  [H+] = 5.6x10^-6 M
  • pOH = 8.75
  • [OH-] = 1.8x10^-9 M
300

Will the following solutions have a pH less than, equal to, or greater than 7:

  1. 1M NaOH
  2. 1M KCl
  3. 1M NaNO2
  4. 1M NH4Br

Greater, 7, greater, less than

400
  1. A solution contains 0.15 M Fe(NO₃)₂ and 0.10 M Zn(NO₃)₂. How much [OH-] would need to be added to separate the ions?
  • How much of the first cation to precipitate is left in solution when the second cation begins to precipitate?
  • [OH]=1.65x10^-7 M
  • 1.1x10^-2 M
400
  1. In order to precipitate zinc hydroxide, you can combine a solution of Zn2+ with a separate solution of OH-. If the concentration of Zn2+ is 4x10^-4 M, what concentration of hydroxide ion would be needed to just begin precipitating the solid?

8.7x10^-7M

400

What are [H+], [OH-], pH, and pOH of a 0.100 M solution of HNO2?

  • [H+]= 8.4x10^-3 M
  • pH= 2.08
  • pOH= 11.92
  • [OH-]= 1.2x10^-12 M
400

A 0.120 M solution of a     monoprotic weak acid has a percent ionization of 2.50%.

What is Ka?

  • Ka=7.7x10^-5
400

0.25g of CH3NH3OH (MM=49.08     g/mol) is dissolved in 0.1 L of water. What is the pH of the solution?

pH=5.967

500
  1. The following Ksp values are given: (see external source)
  • Which compound will precipitate first?
  • Which compound has the highest molar solubility in water?
  • Which compound will precipitate first?  
    • Zn(OH)2
  • Which compound has the highest molar solubility in water? 
    • Ba(OH)2
500
  1. A student is trying to see if only CaF₂ will precipitate in a solution where: (see external source)
  • Calculate Q and determine whether CaF₂ will precipitate.
  • Q=1.6x10^-10
  • Yes
500

What is the solubility of Zn(OH)2 in a solution that has a pOH of 6?

3x10^-4 M

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