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Acids
Bases
Concentrations
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100
The basic equation for Ka.
What is Ka = [H+][A-] / [HA].
100
The basic equation for Kb.
What is Kb= [HB+][OH-] / [B].
100
How much potassium sulfate salt would be required to make 750mL if 0.50M potassium sulfate solution.
What is 65 grams.
100
The number of moles of solute in 1L of a saturated solution (mol/L).
What is molar solubility.
100
pH + pOH = ?
What is 14.
200
An acid that donates a hydrogen is a _____ and an acid that accepts an electron pair is a _____.
What is a Bronsted acid and a Lewis acid.
200
What is the concentration of KOH in a solution at 25C that has pOH 3.31?
What is 4.9x10^-4M.
200
Calculate the molality of the following solution 7.15 moles of ethylene glycol in 3505 grams of water.
What is 2.04 m.
200
Calculate the molar solubility and the solubility in g/L of AgCl.
What is 1.3x10^-5 M and 1.8x10^-3 g/L.
200
The seven strong acids and the eight strong bases include...
What is HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4 and LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2.
300
The Ka of a weak acid is 5.5x10^-4. What is the pH of a 0.63M solution of this acid at 25C?
What is 1.73.
300
A Bronsted base and a Lewis base are different due to the fact that...
What is a Bronsted base accepts hydrogen ions and a Lewis base donates electron pairs.
300
Stock nitric acid is 16M. How much stock nitric would you need to prepare 500mL of 0.5M nitric acid?
What is 15.6mL.
300
Given the solubility, calculate the solubility product constant (Ksp) of MnCO3, s=4.2x10^-6g/L.
What is 1.3x10^-15.
300
List the solubility rules.
What is Soluble compounds include anything from group 1A and ammonium, as well as (NO3-, C2H3O2-), (ClO3-, Cl-, Br-, I-) unless with Ag+, Hg+2, Pb+2, (SO4-2) unless with Ag+, Hg+2, Pb+2, Ca+2, Sr+2, Ba+2 Insoluble compounds include (CO3-2, PO4-3, CrO4-2, S-2) unless with Group 1A and NH4+, (OH-) unless with Group 1A.
400
A 0.042M solution of a weak acid has pH 4.01 at 25C. What is the Ka of this acid?
What is 2.3x10^-7.
400
A 0.12M solution of a weak base has a pH of 10.76 at 25C. Determine Kb.
What is 2.8x10^10^-6.
400
WARNING: NOT A CONCENTRATION PROBLEM! Label each of the species as an acid, base, conjugate acid, or conjugate base. CH3COO-(aq) + H20 (l) --> CH3COOH(aq) + OH- (aq)
What is base, acid, conjugate acid, conjugate base.
400
Predict whether a precipitate will form from 1.5L of 0.025M BaCl2 and 1.25L of 0.014M Pb(NO3)2.
What is no.
400
A larger Ka represents a
What is stronger acid.
500
Determine the pH and percent ionization fro hydrocyanic acid (HCN) solution of concentration 8.3x10^-5M. Ka= 4.9x10^-10
What is 6.70 and 0.24%.
500
Calculate the pH at 25C of a 0.61M aqueous solution of a weak base B with a Kb of 1.5x10^-4.
What is 11.98.
500
WARNING: NOT A CONCENTRATION PROBLEM! Label each of the species as an acid, base, conjugate acid, or conjugate base. HF(aq) + NH3(aq) --> F-(aq) + NH4+(aq)
What is acid, base, conjugate base, conjugate acid.
500
What precipitate if any will form if 0.10M solutions of Pb(NO3)2 and NaI are mixed?
What is PbI2.
500
The 5% rule when using ICE tables says...
What is that we can disregard the x in the denominator if the value for x when solved is 5% or less than the initial concentration.