Question

Citric acid is a triprotic acidwith Ka values of 7.4 x 10-4, 1.7 x 10-5, and 4.0 x 10-7 for the first, second, and third ionization constants, respectively. A 0.500 M solution of a monoprotic acid with a Ka value of 7.4 x 10-4 has a pH = 1.72. What is the pH of a 0.500 M citric acid solution?

Answer #1

Citric acid, C3H5O(COOH)3,
which is present in citrus fruits, is a triprotic acid. Calculate
the concentration of the citrate,
C3H5O(COO)33- , of a 0.040M solution of
citric acid. Ka,1 = 7.4 x10-4, Ka,2 = 1.7 x
10-5, Ka,3 = 4.0x 10-7
a. 5.08 x10-3 M
b. 1.7x10-5 M
c. 2.29
d. 1.33 x 10-9 M
e. 8.87

1.) If the Ka of a monoprotic
weak acid is 4.5 x 10^-6, what is the pH of a 0.30M solution of
this acid?
2.) The Ka of a monoprotic weak
acid is 7.93 x 10^-3. What is the percent ionization of a 0.170 M
solution of this acid?
3.) Enolugh of a monoprotic acid
is dissolved in water to produce a 0.0141 M solution. The pH of the
resulting solution is 2.50. Calculate the Ka for the
acid.

What is the pH of a 0.350 M solution of lithium citrate? (Ka
Citric Acid = 7.4 x 10-4)

Phosphoric acid is a triprotic acid, and the Ka values are given
below. Calculate pH, pOH, [H3PO4], [H2PO4 2-], [HPO4 -], and [PO4
3-] at equilibrium for a 5.00 M phosphoric acid solution.
Ka1 = 7.5 x 10^-3
Ka2 = 6.2 x 10^-8
Ka3 = 4.2 x 10^-13

1. Valeric acid is a monoprotic acid with a Ka value
of 1.44 x 10-5. A student prepared 100.0 mL of a 0.200 M
solution of valeric acid. What is the pH of the valeric acid
solution?

The triprotic acid H3A has ionization constants of Ka1 = 2.4×
10–3, Ka2 = 4.9× 10–7, and Ka3 = 3.2× 10–11. Calculate the
following values for a 0.0170 M solution of NaH2A. Calculate the
following values for a 0.0170 M solution of Na2HA.

The Ka of a citric acid is 1.95x10^-5 at 25 C. what is the pH of
a 0.35 M aqueous solution of citric acid?

The Ka of a monoprotic weak acid is 5.45 x 10-3. What is the
percent ionization of a 0.101 M solution of this acid?

The Ka of a monoprotic weak acid is 8.87 x 10^-3. What is the
percent ionization of a 0.121 M solution of this acid?

Using the ionization constants for acetic acid (Ka= 1.8 x 10^-5)
and ammonia (Kb= 1.8 x10^-5), calculate the expected pH of the
above four solutions (0.100 M sodium acetate,
ammonium chloride, acetic acid and ammonia). Use the simplified
version instead of the quadratic equation.

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