Acids and Base Classwork

____1.Calculate the hydrogen ion concentration of an aqueous solution, given the concentration of hydroxide ions is 1 x 10-5 M and the ion constant for water is 1 x 10-14.

[H]

[H+] = (1 x 10-14/1 x 10-5)

a. / / c. /
b. / / d. /

____2.When acids react with metals, they produce _____ gas.

Example: Zn(s) + HCl(aq) ͢ ZnCl2(aq) + H2(g)

a. / hydrogen / c. / sulfur
b. / nitrogen / d. / oxygen

____3.A basic solution contains more _____ ions than hydrogen. (Arrhenius’ Definition)

a. / oxygen / c. / hydroxide
b. / nitrogen / d. / sulfide

____4.A _____ is produced when a base accepts a hydrogen ion from an acid.(Bronsted-Lowry concept)

a. / conjugate acid / c. / acid
b. / conjugate base / d. / base

____5.The _____ of a weak acid is strong.(Bronsted-Lowry concept)

a. / conjugate acid / c. / acid
b. / conjugate base / d. / base

____6.What is the pH of blood, given the hydrogen ion concentration is 4.0 x 10-8 M?

pH –log [H]

pH = -log 4.0 x 10-8

a. / 7.0 / c. / 7.4
b. / 7.2 / d. / 7.6

____7.An acid that can donate only one hydrogen ion is called a _____ acid.

a. / monoprotic / c. / triprotic
b. / diprotic / d. / polyprotic

____8.In the Bronsted-Lowry model of acids and bases, an _____ is a hydrogen donor and a _____ is a hydrogen acceptor.

a. / acid, base / c. / conjugate acid, conjugate base
b. / base, acid / d. / conjugate base, conjugate acid

____9.Which model states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions?

a. / Arrhenius / c. / Lewis
b. / Bronsted-Lowry / d. / Hydrogen

____10.What is the pH of 0.45 M of H2SO4?

Note: [H+] = 2(0.45) M

Therefore, pH = -log 0.90

a. / 0.0045 / c. / 0.45
b. / 0.045 / d. / 4.50

____11.Identify the acid and conjugate base pair in the following equation: HF + H2O H3O+ + F-

(Bronsted-Lowry concept)

a. / HF & H2O / c. / HF & F-
b. / HF & H3O / d. / H2O & H3O+

____12.An acid that can donate more than one hydrogen ion is called a _____ acid.

a. / monoprotic / c. / triprotic
b. / diprotic / d. / polyprotic

____13.Calculate the H concentration of an aqueous solution, given the concentration of OH–is 1  10–5M and the ion product constant for water, KW is 1  10–14.

[H]

a. / 1  10–9M / c. / 1  10–5M
b. / 1  109M / d. / 1  105M

____14.Calculate the hydrogen ion concentration of an aqueous solution, given the pOH of the solution is 4.50 and the ion product constant for water, KW, is 1.00  10–14.

[H]

a. / 3.16  10–10M / c. / 3.16  10–5M
b. / 3.16  10–9M / d. / 3.16  10–7M

____15.Calculate pH of an aqueous solution of hydrogen chloride acid. Given the hydrogen ion concentration is 8.75  10–9M.

pH –log [H]

Note: [H+] = 8.75  10–9M.

a. / 7.85 / c. / 8.06
b. / 7.81 / d. / 7.77

____16.Calculate the pOH of a 0.410 M Ba(OH) solution.

pOH –log [OH–]

Note: [OH-] = 2(0.410)M

a. / / c. /
b. / / d. /

17.Write a chemical equation for the neutralization of sodium hydroxide and hydrochloric acid.

NaOH + HCl NaCl + H2O

18.Calculate the pH of a buffer solution that is 0.250 M in formic acid, HCOOH, and 0.200 M in formate ion, HCOO–. The ionization constant for formic acid is 1.80  10–4.

HCOOH(aq) H+(aq) + HCOO-(aq)

Ka = [H+][ HCOO-]/[HCOOH]

1.80  10–4 = (x)(x)/0.250

x = [H+] = [(1.80 x 10-4)(0.250)]1/2

pH –log [H+]

19.Determine the following with respect to HNO.

a.Ionization equation.

HNOH +

b.Ionization constant (Ka) expression for the given acid.

c.If the ionization constants (Ka) for HNO and HF are 4.0  10–4and 6.3  10–4 respectively, identify the

weaker acid.