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Acids and Bases: pH based on % dissociation

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Wize University Chemistry Textbook > Acids and Bases

pH

4 Activities

Wize University Chemistry Textbook > Acids and Bases

Percent Dissociation

2 Activities

In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution

If an answer is an exponent such as 4.3x10-7, input the answer as: 4.3e-7
More pH Questions:
Weak Acids and Bases
Calculate the pH of the following solution.
A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Note: Acetic Acid Ka = 1.8 x 10-5
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.
Henderson Hasselbalch: Titrations and pH
For the titration of 50.00 mL of 0.1000 M ammonia (NH3) with 0.1000 M HCl calculate the pH (For ammonia Kb​=1.8×10−5)(For\ ammonia\ Kb​=1.8\times10^{-5})
Before the addition of any HCl
After 20.00 mL of the acid has been added
Molecular formula: Concentration
A solution of HBr has a pOH of 12.2, what is the [H+] concentration?
100 mL of a 0.5 M solution of nitric acid (HNO3\rm HNO_3) was added to 75 mL of a 0.37 M solution of sodium benzoate (C6H5COONa\rm C_6H_5COONa) the conjugate base of benzoic acid (C6H5COOHKa=6.6×10−5\rm C_6H_5COOH Ka = 6.6 \times 10^{-5}). Calculate the pH\rm pH of the resulting solution.
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
Acids and Bases: pH of Alkaline Earth Metal Hydroxides
Calculate the pH of a 1.00 x 10-4 M Mg(OH)2 solution.
Acids and Bases: Strong Acid Mixture
Practice Question: Strong Base Mixture
Calculate the pH and pOH of a solution containing a mixture of 75.00 mL of 0.100 M HI and 25.00 mL of 0.250 M HClO4.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.500 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 150.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a) A 6.30 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 4.25 x 10-4 g of CH3COONa in 100.0 mL of water.
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 10.00 mL of 0.700 M NaOH solution and diluting it to 100.00 mL with water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 100.0 mL of 3.00 x 10-2 M KOH with 50.0 mL of 2.50 x 10-2 M Be(OH)2.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a) 2.75 x 10-3 M aqueous HNO3 solution.
b) 1.50 x 10-2 g of CaO dissolved in 200.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions, knowing that Ka = 1.8x10^-5.
a) A 5.33 x 10-2 M solution of CH3COOH in water.
b) A solution prepared by dissolving 1.15 x 10-3 g of CH3COONa in 100.0 mL of water.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.150 g of sodium hydrogen phosphate (Na2HPO4, MW = 141.9579 g/mol) in 125.0 mL of water.
Ka (HPO42−) = 4.2 x 10−13;  Kb (HPO42−) = 1.6 x 10−7. K_a\ \left(HPO_4^{2-}\right)\ =\ 4.2\ x\ 10^{-13};\ \ K_b\ \left(HPO_4^{2-}\right)\ =\ 1.6\ x\ 10^{-7}.\
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 20.00 mL of 0.500 M Be(OH)2 solution and diluting it to 100.00 mL with water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 25.00 mL of 0.100 M HCl with 75.00 mL of 2.50 x 10-2 M HBr.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a) 3.00 x 10-4 M aqueous HClO4 solution.
b) 8.00 x 10-3 g of Na2O dissolved in 150.0 mL of water.
Consider the following reaction in water:
NaOH <----> Na+ + OH-
This reaction has a Kb of 1 x 10-10 and a pOH of 3. If there is 1 M of NaOH at equilibrium, what is the concentration of Na+ in solution?
Which of the solutions below would have the HIGHEST pH value?
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (Ka for HF = 6.8×10-4)?
Methyl diethanolamine CH3N(C2H4OH)2 is a weak base which we will abbreviate as mdea. The conjugate acid, mdeaH+, has a pKa = 8.52.
More Percent Dissociation Questions:
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H3O+], pH and pOH of the solution
Weak Acids and Bases
Calculate the percent dissociation for the following solutions.
a) A 0.223 M aqueous solution of HF.
b) A 1.70 x 10-2 M aqueous solution of NaF.
Weak Acids and Bases
Which equation best describes the dissociation of hydrofluoric acid in water?
Weak Acids and Bases
Calculate the percent dissociation for the following solutions.
a) A 0.444 M aqueous solution of HCN (Ka = 6.2 x 10-10).
b) A 3.50 x 10-2 M aqueous solution of NaCN.
Le Chatelier's Principle: Percent dissociation
A solution made by dissolving 0.1 mol of acetic acid in 1.0 L of water is 4.1% dissociated. Which of the modifications below would cause the % dissociation of the acetic acid in the container to increase? (Ka for acetic acid is 1.8×10-5.)