General
What is another name for a hydrogen atom?
Proton
Why is water described as amphoteric?
Because it acts as both an acid and a base
water and a salt
What is the partner of a conjugate acid?
A base
What are the formulas for Ka and Kb?
Ka = [H+]2 / [HA]
Kb = [OH-]2 / [B]
If the hydrogen ion concentration is 2.3 x 10-3 M, what is the pH?
2.64
What is the range of the pH scale?
0-14
According to the Arrhenius definition, acids contain _____ and produce ______ and bases contain _____ and produce ______
hydrogen, hydrogen ions, hydroxide, hydroxide ions
What is the equivalence point? What is the end point?
Equivalence point - end of titration (when the known neutralizes the unknown)
End point - when the color of indicator changes
The stronger the conjugate base...
the weaker the acid
Write the Ka expression for the weak acid:
H2CO3(aq) + H2O(l) = HCO3-1(aq) + H3O+1(aq)
Ka = [HCO3-1] [H3O+1] / [H2CO3]
or Ka = [HCO3-1] [H+1] / [H2CO3]
Calculate the hydrogen ion concentration if the hydroxide ion concentration is 1.8 x 10-3 M and Kw = 1.0 x 10-14
5.56 x 10-12 M
What is present in a container of the weak acid, HF?
HF molecules and hydrogen (hydronium) ions and fluoride ions
What is a Bronsted-Lowry acid?
A hydrogen ion donor (or a proton donor)
If a strong base and a weak acid are titrated, the indicator should have a pH range of _____
8 - 9 or 10
Identify the base and conjugate acid pair in this reaction: C6H5COOH + NH3 = C6H5COO-1 + NH4+1
Base = NH3 and conjugate acid is NH4+1
What is the hydroxide ion concentration for a 0.033 M base whose Kb is 5.6 x 10-4?
0.0043 M or 4.3 x 10-3 M
What is the hydrogen ion concentration of a solution with a pOH of 4.4 given the Kw = 1.0 x 10-14?
2.51 x 10-10 M
How much does the hydrogen ion concentration increase from pH 9 to pH 6?
concentration increases by 1000
What is the difference between a strong base and a weak base?
A strong base completely dissociates (splits) into ions; a weak base partially dissociates into ions
HBr + KOH = H2O + KBr
0.93M
What is the conjugate acid of CrO4-2 ?
HCrO4-1
Find the pH of a 0.45 M acid whose Ka is 8.3 x 10-12
5.7
What is the pOH of a 0.125 M solution of NaOH?
0.9 or 9.0 x 10-1
Write the ionization for Ca(OH)2 and for H2SO4
Ca(OH)2 = Ca2+ + 2OH-1 and
H2SO4 = H+1 + HSO4-1
What solution resists a change in pH?
15.00mL of a solution of calcium hydroxide is titrated with 9.88mL of 0.75 M hydrochloric acid. Calculate the molarity of the base (write the BCE)
Write the dissociation of HMnO4 in water and label the acid, base, and conjugates
HMnO4 + H2O = MnO4-1 + H3O+1 (A + B = CB + CA)
Find the Kb for a 0.0156 M basic solution with a pH of 8.7?
1.61 x 10-9
Calculate the hydrogen ion concentration of a 0.33 M solution of Sr(OH)2 given the ionization constant Kw is 1.0 x 10-14.
1.52 x 10-14