Concept explainers
Interpretation:
All the given solutions are to be arranged in accordance with increasing hydroxide concentration present in the solutions.
Concept Introduction
The
The relation between hydroxyl concentration,
The relation between the ionic product of water,
Answer to Problem 135QP
Solution:
Explanation of Solution
Given Information: The given concentrations of the solutions are
In equation (1),
In equation (3),
The hydroxyl ion concentration in the given buffer solution is calculated by the substitution of
The hydroxyl ion concentration of pure water at
Therefore, the order of increasing hydroxyl ion concentration is given as follows,
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Chapter 13 Solutions
INTO TO CHEMISTRY (EBOOK ACCESS CODE)
- An aqueous solution contains formic acid and formate ion. Determine the direction in which the pH will change if each of the following chemicals is added to the solution. (a) HCl (b) NaHSO4 (c) CH3COONa (d) KBr (e) H2Oarrow_forwardTwo strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?arrow_forwardWhich of the solutions listed below has the lowest pH? (a) 0.10 M HCl (b) 0.10 M NaOH (c) 2.5 105 M HNO3 (d) pure H2Oarrow_forward
- The 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_forwardFor each of the following pairs of solutions, indicate whether the first listed solution has a higher or lower pH than the second listed solution. a. 1.0 M NaOH and 1.0 M HCl b. 1.0 M HNO3 and 0.10 M HNO3 c. 0.10 M HClO4 and 0.10 M HCN d. [H3O+] = 3.3 103 and [H3O+] = 9.3 103arrow_forwardWrite the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases. (a) hydrazoic add, HN3 (b) citric acid, H2C6H6O7 (c) squaric acid, H2C4O4arrow_forward
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- Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardA solution of acetic acid, HC2H3O2, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.57, what was the concentration of the acetic acid? The Ka of acetic acid is 1.7 105.arrow_forwardWrite chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2CO3 (carbonic acid) b. H2C3H2O4 (malonic acid)arrow_forward
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