Concept explainers
Calculate the pH of a
Interpretation:
The pH of the solution with dissolved salt is to be calculated, with given concentration.
Concept introduction:
The relationship between
The formula to calculate the pOH of the solution from the concentration of hydroxide ions is given as follows:
The relation between pH and pOH is as follows:
The formula to calculate the pH of a solution is:
Answer to Problem 151AP
Solution:
Explanation of Solution
Given information:
The concentration of
In the salt
The cation
Refer to table
The reaction is as follows:
Now, prepare an equilibrium table and represent each of the species in terms of
Now, substitute these concentrations in equation (2) as follows:
Assume
Thus,
Similarly, the anion
Refer to table
The reaction is given as follows:
Now, prepare an equilibrium table and represent each of the species in terms of
Now, substitute these concentrations in equation (3) as follows:
Assume
Thus,
The equilibrium table for this reaction is shown below.
Thus,
Use equation (4) to calculate the pOH of the solution as follows:
Now, use equation (5) to calculate the pH of the solution as follows:
The pH of the salt solution containing
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Chapter 16 Solutions
Chemistry
- The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.arrow_forwardCalculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 Marrow_forwardThe base ethylamine (CH3CH2NH2) has a Kb of. A closely related base, ethanolamine(HOCH2CH2NH2), has a Kb of 3.2105. (a) Which of the two bases is stronger? (b) Calculate the pH of a 0.10M solution of the strong base?arrow_forward
- Define pH and explain why pH, rather than molarity, is used as a concentration measure of H3O+.arrow_forwardAcids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forwardWhich of the following conditions indicate an acidic solution? pH = 3.04 (H+| > 1.0 X IO’7 A/ pOH = 4.51 |OH-J = 3.21 X 10"12 Marrow_forward
- Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.arrow_forwardWrite equations that show H2PO4- acting both as an acid and as a base.arrow_forward
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