Question

Calculate the pH of a buffer containing 0.030 M
HC_{2}H_{3}O_{2} and 0.050 M
NaC_{2}H_{3}O_{2}. The K_{a} of
HC_{2}H_{3}O_{2} is 1.75 x
10^{-5}.

Answer #1

Calculate PKa of CH_{3}COOH

Ka for CH_{3}COOH = 1.75 x 10^-5

PKa = −log Ka

= - log 1.75 x 10^-5

** = 4.76**

Concentration of CH_{3}COOH and CH_{3}COONa are
given, so we can calculate the pH of a buffer solution by using
Henderson-Hasselbalch equation

pH = pKa +log[A−]/[HA]

Where

pKa = 4.76

[A-] = [CH_{3}COO-] = 0.050 M

[HA] =[CH_{3}COOH ] = 0.030 M

PH = pKa +log [CH3COO-]/ [CH_{3}COOH]

PH = 4.76 + log [0.050/0.030]

PH = 4.76 + 0.22

**PH = 4.98**

What is the pH of a 0.100 M solution of NaC2H3O2 when
Ka(HC2H3O2) = 1.8 X 10-5?

Find the pH of a 0.342 M NaC2H3O2 solution. (The Ka of acetic
acid, HC2H3O2, is 1.8×10−5.)

Find the pH of a 0.250 M solution of NaC2H3O2 . (The
Ka value of HC2H3O2 is 1.80×10−5).
Express your answer numerically to four significant figures.
Please Help. Thank you!!!

A 1.0 L buffer solution contains 0.192 MHC2H3O2 and 0.192 M
NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Because
the initial amounts of acid and conjugate base are equal, the pH of
the buffer is equal to pKa=−log(1.8×10−5)=4.74.
Calculate the new pH after adding 0.019 mol of solid NaOH to the
buffer.

What is the pH of a buffer containing 0.050 M NH3 and 0.050 M
NH4Cl?

Part A
Consider a buffer solution that is 0.50 M in NH3 and
0.20 M in NH4Cl. For ammonia, pKb=4.75.
Calculate the pH of 1.0 L of the original buffer, upon addition
of 0.190 mol of solid NaOH.
Part B
A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100
mol NaC2H3O2. The value of Ka for HC2H3O2 is
1.8×10−5.
Calculate the pH of the solution, upon addition of 0.030 mol of
NaOH to the original buffer.
(I will leave...

acetic acid (hc2h3o2) is a weak acid (ka= 1.8*10^-5). Calculate
the pH of a15.1 M HC2H3O2 solution.

Given that Buffer A contains 200.0 mL 0.050 M HOCl and 400.0 mL
0.030 M NaOCl, calculate
1. The pH of the buffer solution.
2. The pH of the solution after adding 10.0 mL 0.50 M HCl.
3. The pH of the solution after adding 20.0 mL 0.40 M NaOH

Before preparing the buffer solutions, you must determine the
amounts of acetic acid (HC2H3O2,
M.Wt.= 60.05 g/mol) and sodium acetate
(NaC2H3O2, M.Wt.= 82.03 g/mol)
required. The Ka of
HC2H3O2 is 1.8 X 10-5
(pKa = 4.74). Explain how you will prepare 100 mL of an
HC2H3O2—NaC2H3O2
buffer starting with:
(1) 0.10 M HC2H3O2 and solid
NaC2H3O2
(2) 0.30 M HC2H3O2 and solid
NaC2H3O2
(3) 0.50 M HC2H3O2
and solid NaC2H3O2

1) Ka of 1.0 M
HC2H3O2 with a pH: 2.43
2) Ka of 0.10 M
HC2H3O2 with a pH: 2.94
3) Ka of 0.010 M
HC2H3O2 with a pH: 3.27

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