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Concept explainers
Interpretation:
Conjugate acid-base pairs inequation for reaction between
Concept Introduction:
Bronsted-Lowry acid outlined the definition of acids that donate
In accordance with Bronsted definition, the most usual type of acid-base reaction involves lone pair of base that reaches out for an acidic proton. Once deprotonation has occurred species assumes a negative charge and is referred to as the conjugate base of acid and other species with a positive charge as a result of proton acceptance is termed conjugate acid of given base. The strength of conjugate acid-base pairs is inversely related to each other; thus strong acid has a weak and strong base has weak conjugate counterparts and vice-versa.
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Chapter 15 Solutions
FOUND.OF COLLEGE CHEMISTRY
- What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?arrow_forwardFollow the directions of Question 19 for the following acids: (a) hypochlorous acid (b) formic acid, HCHO2 (c) acetic acid, HC2H3O2 (d) hydrobromic acid (e) sulfurous acidarrow_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
- How do I write the chemical equation for the reaction of NaOH and HC2H3O2?arrow_forwardDetermine the pH of a 0.31 M solution of NaN3 (Ka for HN3 = 1.9 × 10−5). Express your answer using at least three significant figures. Do not use scientific notation.arrow_forwardExplain how ammonia can function both as a Brønsted base and as a Lewis base.arrow_forward
- Write a balanced equation showing how the H,PO42 ion can be either a Brønsted-Lowry acid or a Brønsted- Lowry base.arrow_forwardThe substance dimethylamine is a weak nitrogenous base like ammonia.Write a net ionic equation to show how dimethylamine, (CH3)2NH, behaves as a base in water.arrow_forwardWhen lithium oxide 1Li2O2 is dissolved in water, the solution turns basic from the reaction of the oxide ion 1O2-2 with water. Write the equation for this reaction and identify the conjugate acid–base pairs.arrow_forward
- Write separate equations representing the reaction of HSO3−(a) as an acid with OH−(b) as a base with HIarrow_forwardWrite a net ionic equation for the equilibrium that causes the solution of KHTar in water to be slightly acidicarrow_forwardWrite equations that show H2 PO4− acting both as an acid and as a base.arrow_forward
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