Ca oh 2 aq ch3co2h aq

Section 17.2
1. H3PO4, phosphoric acid, can donate two protons to water to form the monohydrogen phosphate ion, H3PO42-. Is the monohydrogen phosphate ion and acid, a base, or amphiprotic?

(a) acid

(b)base

(c) amphiprotic

2. The cyanide ion, CN-, accepts a proton from water to form HCN. Is CN- a Bronsted acid or base or is it amphiprotic?

(a) acid

(b)base

(c) amphiprotic

3. In the following reaction, identify the acid on the left and its conjugate base on the right.

HNO3 (aq) + NH3 (aq) ↔ NH4+ (aq) +NO3- (aq)

(a) acid= NH3 and conjugate base=NH4+

(b) acid= HNO3 and conjugate acid= NO3-

Similarly, identify the baseon the left and its conjugate acid on the right.

(a) base= = NH3 and conjugate base=NH4+

(b) base= HNO3 and conjugate acid= NO3-

4. Identify the conjugate acid/base pairsin the reaction of HF and acetic acid.

HF(aq) + CH3CO2-(aq) ↔F-(aq) + CH3CO2H(aq)

(a) HF/CH3 CO2- and F-/CH3 CO2H

(b) HF/ CH3CO2H and F-/CH3 CO2-

(c) HF/F- and CH3CO2H/CH3CO2-

Section 18.4
1. What is the Kspexpression for silver carbonate?

(a) Ksp = [Ag+][CO32-]

(b) Ksp = [Ag+]2[CO32-]

(c) ) Ksp = [Ag+][CO32-]2

2. Using Ksp values, predict which salt in each pair is more soluble in water.

(a) AgCI (Ksp=1.8x10-10) or AgCN (Ksp=6.0 x 10-17)

(b) Mg(OH)2(Ksp=5.6x10-12) or Ca(OH)2(Ksp=5.5 x 10-5)

(c) Ca(OH)2 (Ksp=5.5x10-5) or CaSO4 (Ksp=4.9 x10-5)

3. What is the solubiluty of PbSO4 in water at 25oC? (Ksp for PbSO4= 2.5 x 10-8)

(a) 2.5 x 10-8M

(b) 1.6 x 10-4M

(c) 6.3 x 10-16M

4. What is the solubility of PbSO4 in water at 25oC if the solution already contains 0.25 M Na2SO4? (Ksp = for PbSO4= 2.5x 10-8)

(a) 1.0 x 10-7 M

(b) 1.6 x 10-4 M

(c) 6.3 x 10-9 M

5. Which compound should be more soluble in 0.1 M HCI?

(a) FeCO3(Ksp =3.1 x 10-11)

(b) AgCI (Ksp= 1.8 x 10-10)