Question

a. Give the conjugate acid (or base) for each species listed below, and label which it is. a. H2O b. HS- c. HCO3- d. HNO2 e. NH3 f. CH3COO- 2. Find the pH of each solution given below. a. 0.55 M NaOH b. 0.023 M HNO3 c. 0.054 M Sr(OH)2 3. What is the pH of a solution with [HCOOH] = 1.50 M? 4. What is the pH of a solution with [(CH3)3N] = 2.75 M? 5. What is the Ka of a particular weak acid HA if at equilibrium [HA] = 0.50 M, [A-] = 0.0035 M, and [H3O+] = 0.0035 M? 6. Write the chemical equilibrium for the weak acid HF reacting with water, then predict what will happen to the equilibrium concentration of HF if a. HCl is added b. KF is added c. NaCl is added d. NaOH is added e. HF is added

          a. Give the conjugate acid (or base) for each species listed below, and label which it is.
a. H2O
b. HS-
c. HCO3-
d. HNO2
e. NH3
f. CH3COO-

2. Find the pH of each solution given below.
a. 0.55 M NaOH
b. 0.023 M HNO3
c. 0.054 M Sr(OH)2

3. What is the pH of a solution with [HCOOH] = 1.50 M?
4. What is the pH of a solution with [(CH3)3N] = 2.75 M?
5. What is the Ka of a particular weak acid HA if at equilibrium [HA] = 0.50 M, [A-] = 0.0035 M, and [H3O+] = 0.0035 M?
6. Write the chemical equilibrium for the weak acid HF reacting with water, then predict what will happen to the equilibrium concentration of HF if
a. HCl is added
b. KF is added
c. NaCl is added
d. NaOH is added
e. HF is added

Added by Austin J.

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