ALEKS 360 AC INTRD CHEM >I<
5th Edition
ISBN: 9781260977585
Author: BAUER
Publisher: MCG
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Chapter 13, Problem 39QP
Sodium fluoride,
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Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?
The acidity of a solution is measured by its pH.
If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution,
the pH is defined by pH = – log H+
Based on careful measurements and calculations, a chemist examines two solutions and asserts:
"The hydrogen ion concentration of Solution A
is 158 times greater than
the hydrogen ion concentration of Solution B."
If the pH of solution B is 3.4, determine the pH of Solution A.
Report your answer to one decimal place.
Solution A has pH equal to
Number
(Report to the nearest 0.1)
Acidity of a solution is determined by the concentration H of hydrogen ions in the solution (measured in moles per liter of solution). Chemists use the negative of the logarithm of the concentration of hydrogen ions to define the pH scale. pH = − log H
Solution A has a pH value of 5.6 and solution B has a pH value of 2.7. Compare the acidity of the two solutions.
a) Solution A is more acidic by a factor of 2.07b) Solution B is more acidic by a factor of 794.33c) Solution A is more acidic by a factor of 794.33d) Solution A is more acidic by a factor of 2.90
Chapter 13 Solutions
ALEKS 360 AC INTRD CHEM >I<
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?arrow_forwardWrite chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)arrow_forwardStudents are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2arrow_forward
- Two 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_forwardMost naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forward12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’arrow_forward
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