Brønsted–Lowry Acids and Bases

Key Questions

• What are Bronsted-Lowry acids and bases?

  Bronsted Acid is an H+ donor, Bronsted Base is an H+ acceptor.

  Usually Bronsted Acids have an H bonded to a halogen or an oxygen. A base, usually OH- or H2O, will have a lone pair of electrons that forms a bond with an H+ on the acid. The proton essentially transfers from acid to base during an acid-base reaction.

  ChemGuy · 2 · Apr 11 2014

• How do Bronsted-Lowry acids and bases form conjugate pairs?
• What are Bronsted-Lowry acids and bases?
• How do you predict the products of an acid base reaction? I know a salt and water is formed - which salt or how?
• What are the two acid-base pairs in water?
• Using the Brønsted-Lowry concept of acids and bases, which is the Brønsted-Lowry acid and base in the following reaction? (CH3)2NH(g)+BF3(g)→(CH3)2NHBF3(s)
• Is NH3 a Bronsted-Lowry base?
• Is methylamine a Bronsted-Lowry base?
• Is ethylamine a Bronsted-Lowry base?
• Using the Brønsted-Lowry concept of acids and bases, which is the Brønsted-Lowry acid and base in the following reaction? HS−(aq)+H2O(l)→H2S(aq)+OH−(aq)
• Is the following acid-base reaction Arrhenius, Bronsted-Lowry, or Lewis: AlCl3 + Cl --> AlCl4-
• Is the following acid-base reaction Arrhenius, Bronsted-Lowry, or Lewis: H2SO4 + NH3 --> HSO4- + NH4+
• Is the following acid-base reaction Arrhenius, Bronsted-Lowry, or Lewis: Ag+ + 2 NH3 --> Ag(NH3)2+
• In the following equation, identify Arrhenius acids or bases and Bronsted-Lowry acids or bases. NH3 + H2O --> NH4 +1 + OH-1
• When was the Brønsted–Lowry theory proposed?
• How can I determine a Bronsted-Lowry base?
• What are some examples of Bronsted-Lowry bases?
• What is an example of a Bronsted-Lowry bases practice problem?
• What is an example of a Bronsted-Lowry acids practice problem?
• What is a Bronsted-Lowry acid?
• Question #69f70
• In the equation #HCl(g) + H_2O(l) -> H_3O^+(aq) + Cl^(-)(aq)#, which species is a Bronsted-Lowry acid?
• How would you write the formula of the conjugate base of the Bronstead-Lowry acids H2SO3 and HI?
• Question #c2861
• Can someone explain the Bronsted-Lowry definition of acids and bases?
• Question #a90b7
• Question #c4072
• Which of the following are Bronsted-Lowry acids? #a.# #HSO_3^(-)#, #b.# #HF#, #c.# #SO_3^(2-)#, #d.# #SO_4^(2-)#, #e.# #Cl_2#?
• Question #d290a
• In this example, which species acts as an acid and why? #H_2SO_4^- +H_2O -> SO_4^(2-) + H_3O^+#
• Considering #CO_3^(2-) + H_2O rightleftharpoons HCO_3^- + OH^#, which species acts as a Bronsted Lowry base in the forward reaction?
• What substance is acting as the Bronsted-Lowry base in the following forward reaction? #HNO_3 + H_2O -> H_3O^+ + NO_3^-#?
• How does a Brønsted-Lowry acid form its conjugate base when dissolved in water? How is the water involved in this process?
• How do we assess whether an acid is strong in aqueous solution?
• How does hydrogen chloride behave in aqueous solution?
• How would you complete this Bronsted-Lowrt reaction? #HCO_3^(-) (aq)+ H^(+) (aq) rightleftharpoons ?#
• How is the #"Bronsted Lowry"# theory of acidity formulated?
• Why does calcium oxide give rise to TWO equiv of hydroxide ion in aqueous solution?
• What is the difference between #"oxalic acid"#, and #"barbituric acid"#?
• Which compounds are the Bronsted-Lowry bases in this equilibrium: #HC_2O_4^- + H_2BO_3^(-) rightleftharpoons H_3BO_3 + C_2O_4^(2-)#?
• Question #d6e9e
• Question #c9e57
• Why do ionic solids NOT dissolve in water?
• How do you distinguish strong acids and weak acids?
• Question #5c225
• What is the #pH# of an aqueous solution of sodium carbonate?
• Question #b54aa
• Question #b85c7
• For #HSO_4^(-)#, #NH_3(aq)#, and #NH_4^(+)# which species are Bronsted acids, and which are Bronsted bases?
• What is a Bronsted Base?
• What is the Bronsted-Lowry definition of an acid and a base?
• What are all of the ions that may be formed when #H_3PO_4# ionizes in water?
• Question #a6045
• Question #dc93c