Question

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the [H ] of a 0.27 M solution of this acid?

Answer #1

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the
pH of a 0.12 M solution of this acid?

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.

If the Ka of a monoprotic weak acid is 7.5 × 10-6, what is the
pH of a 0.12 M solution of this acid?

If the Ka of a monoprotic weak acid is 3.3 × 10-6, what is the
pH of a 0.30 M solution of this acid?

If the Ka of a monoprotic weak acid is 5.7 × 10-6, what is the
pH of a 0.14 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
pH of a 0.43 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
pH of a 0.50 M solution of this acid?

1. The Ka of a monoprotic weak acid is 5.90 × 10-3. What is the
percent ionization of a 0.148 M solution of this acid?
2. If the Kb of a weak base is 4.5 × 10-6, what is the pH of a
0.26 M solution of this base?
3. Assuming complete dissociation, what is the pH of a 3.00 mg/L
Ba(OH)2 solution?

The Ka of a monoprotic weak acid is 6.69 × 10-3. What is the
percent ionization of a 0.158 M solution of this acid?

The Ka of a monoprotic weak acid is 3.16 × 10-3. What is the
percent ionization of a 0.188 M solution of this acid?

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