Question

- What is the pH of a 0.15 M solution of HClO? K
_{a}for HClO = 3.5 x 10^{-8 }

- The value of K
_{a}for the weak acid Benzoic acid (C_{6}H_{6}COOH) is 1.5 × 10^{-5}. What are the equilibrium concentrations of all species if 1.50 g of Benzoic acid is dissolved in enough water to make a 250.0 mL solution? What is the pH of the solution?

- Ammonium ion is the conjugate acid of Ammonia. What
is the pH of a 0.25 M solution of NH
_{4}Cl? The K_{b}for Ammonia, NH_{3}, is 1.8 × 10^{-5}.

Steps:

- What is the balanced chemical reaction?
- Set up Ka expression:
- Determine the value of K
_{a}for the conjugate acid from the K_{b}given - Determine the initial concentrations of each species present:
- Set up table:

initial concentration (M) |
|||

change in conc (M) |
|||

equilibrium conc (M) |

- Solve for Q to determine the direction of the reaction:
- Solve for the equilibrium concentrations in terms of x:
- Solve for x: (Can you make the assumption that x is small compared to the initial concentrations?)
- Determine the % reaction to verify assumption if made:
- Check your equilibrium concentrations in Ka to determine if answers are correct.
- Calculate pH from the equilibrium concentration of
H
_{3}O^{+}

Answer #1

Question:
Consider a .045 M solution of benzoic acid
(C6H5CO2H) whose Ka
value is 6.5 x 10-5.
A). write the acid-base reaction equation for this acid with
water:
B). write the equilibrium expression (Ka) for this
reaction:
C). Calculate the concentration of benzoic acid, benzoate ion
(the conjugate base), and hydronium ion for this solution.
D). Calculate the pH of this solution.
E). Calculate the concentration of hydroxide ions in this
solution.

Question #1)
a) What is the pH of a 0.273 M aqueous solution
of potassium hypochlorite,
KClO at 25 °C?
(Ka for HClO =
3.5×10-8)
b) The value of Ka for acetic acid
is 1.80×10-5. What is the value of
Kb, for its conjugate base,
CH3COO-?
c) The hydronium ion concentration of an aqueous solution of
0.456 M ammonia is ...
[H3O+] = ____ M.
d) In the laboratory, a general chemistry student measured the
pH of a 0.456 M...

Calculate the pH of a 0.334 M aqueous solution
of phenol (a weak acid)
(C6H5OH, Ka =
1.0×10-10) and the equilibrium
concentrations of the weak acid and its conjugate base.
pH
=
[C6H5OH
]equilibrium
=
M
[C6H5O-
]equilibrium
=
M

Calculate the pH of a 0.375 M aqueous solution
of nitrous acid (HNO2,
Ka = 4.5×10-4) and the
equilibrium concentrations of the weak acid and its conjugate
base.
pH
=
[HNO2 ]equilibrium
=
M
[NO2-
]equilibrium
=
M

Calculate the pH of a 0.501 M aqueous solution of chlorous acid
(HClO2, Ka = 1.1×10-2) and the equilibrium concentrations of the
weak acid and its conjugate base.
pH =
[HClO2]equilibrium = M
[ClO2- ]equilibrium = M

The Ka for benzoic acid is what is 6.28 x 10-5. If 13.7
mL a solution with an analytical concentration of HNO3 of 1.65
M is added to 363.4 mL solution with an equilibrium
concentration of benzoate of 0.516 M and an equilibrium
concentration of benzoic acid of 0.0861M, what is the pH
of the resulting solution?

What is the pH of a 0.10 M solution of KClO, Ka (HClO) =
3.0x10^8

What is the pH of 40 mL of a 0.10M solution of HClO with a
Ka of 3.0 x 10-8 after 10mL of 0.20M NaOH has
been added?

Determine the [H3O⁺] in a 0.265 M HClO solution. The Ka of HClO
is 2.9 × 10-8.

1.ka for HF is 6.8x10^-4. calculate the kb for its
conjugate base, the flouride ion, F-
2. which of the following salts dissovled in water
will form basic solutions?
NH4Cl? Cu(No3)2? NaCN? LiF?
3. what is the concentration (in M) of hydronium ions
[H3O+] or [H+] in a solution at 25°C with pH=4.282
4. what is the pOH of a solution with a pH of 3.7?
5. the kb of methylamine is 4.4 x 10^-4. calculate tje
pH of a...

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