Br0nsted-Lowry base

A Br0nsted-Lowry base is to a hydrogen-ion acceptor as a Brpnsted-Lowry acid is to —... [Pg.37]

Terms to Understand acid Br0nsted-Lowry base entropy overall formation constant... [Pg.116]

Brpnsted-Lowry acids are proton donors, and Br0nsted-Lowry bases are proton acceptors. An acid increases the concentration of H,0+ in aqueous solution, and a base increases the concentration of OH. An acid-base pair related through the gain or loss of a single proton is described as conjugate. When a proton is transferred... [Pg.116]

A Brpnsted-Lowry acid donates an H+ ion a Br0nsted-Lowry base accepts H+. [Pg.21]

Brpnsted-Lowry acid Br0nsted-Lowry base conjugate acid conjugate base acidity constant Ka pKa organic acid organic base Lewis acid Lewis base... [Pg.38]

Lewis bases are structurally the same as Br0nsted-Lowry bases. Both have an avaQable electron pair—a lone pair or an electron pair in a ji bond. A Br0nsted-Lowry base always donates this electron pair to a proton, but a Lewis base donates this electron pair to anything that is electron deficient. [Pg.74]

Carboxylic acids are strong organic acids, and as such, readily react with Br0nsted-Lowry bases to form carboxylate anions. [Pg.699]

Br0nsted-Lowry base (Section 2.1) A proton acceptor, symbolized by B. A Brpnsted-Lowry base must be able to form a bond to a proton by donating an available electron pair. [Pg.1197]

Again, notice that ammonia, a Brpnsted-Lowry base, is also an Arrhenius base. All Arrhenius bases are also Brpnsted-Lowry bases. Ammonia does not have to react in aqueous solution to be considered a Br0nsted-Lowry base. Even as a gas, ammonia accepts a proton from hydrogen chloride, as Figure 8 shows. [Pg.554]

A Br0n ted-Lowry acid is a substance that donates a hydrogen ion (H ), and a Br0nsted-Lowry base is a substance that accepts (The name proton is often used as a synonym for because loss of the valence... [Pg.51]

The Brpnsted-Lowry definition of a base is even more inclusive, incorporating substances that would never be considered bases by the Arrhenius definition. A Br0nsted-Lowry base is a substance that accepts protons from another species. This definition allows substances such as ammonia NH3, which not only doesn t release OH ions, but doesn t even have oxygen in it, to be considered bases. Look at the following chemical equation, and you will see an example of ammonia acting as a base. [Pg.315]

As you can see, the ammonia is acting as a Br0nsted-Lowry base, because it is accepting a proton from another species, the water. What is water acting like in this equation If you said a Brpnsted -Lowry acid, you are correct. Water is donating a proton to the ammonia, to become the hydroxide ion. [Pg.316]

Write the conjugate acid for each of the following Br0nsted-Lowry bases. [Pg.321]

Identify the two Br0nsted-Lowry bases in the following reaction ... [Pg.321]

Which of the following could be considered a Br0nsted-Lowry base, but not an Arrhenius base ... [Pg.329]

One very important thing to remember is that an acid and base are always present in these reactions. In order for a molecule or ion to donate a proton, there has to be another ion or molecule to receive it. In addition, in reversible acid-base reactions, the roles of the substances as proton donor or acceptor will switch in the reverse reaction. In the example below, note how water (a Br0nsted-Lowry base in this reaction) accepts a proton to form a hydronium ion in the forward reaction. In the reverse reaction, the hydronium ion (Br0nsted-Lowry acid) donates a proton and, after losing the proton, becomes the water molecule once again. [Pg.320]

These pairs of substances—H O/H O and H CO /HCOf—differ only by the presence (or absence) of a proton, which classifies them as conjugate acid-base pairs. A conjugate acid is formed when a proton is added to a Br0nsted-Lowry base. Therefore, in the previous example the conjugate acid is the hydronium ion, since it was formed by the addition of a proton to... [Pg.320]

In the chemical reaction shown below, identify the Br0nsted-Lowry acid, the Br0nsted-Lowry base, the conjugate acid, and the conjugate base. [Pg.321]

Arrhenius acids increase the concentration of H+ ions in solution, while Arrhenius bases increase the concentration of OH in solution. The strongest acids and bases are Arrhenius acids and bases. Br0nsted-Lowry acids donate protons in solution. Br0nsted-Lowry bases accept protons in solution. The definitions for Br0nsted-Lowry acids and bases are more broad and allow for the consideration of many more substances than either of the other two definitions. [Pg.344]

When a Br0nsted-Lowry acid donates a proton, the remaining anion is known as a conjugate base. When a Br0nsted-Lowry base accepts a proton, the protonated base is known as a conjugate acid. [Pg.344]

A base is a proton acceptor, any species that accepts an H ion. A base must contain a lone pair of electrons to bind the ion a few examples are NH3, C03 , and F , as well as OH itself. Br0nsted-Lowry bases are not Arrhenius bases, but all Arrhenius bases contain the Brpnsted-Lowry base OH . [Pg.588]

The other large group of Br0nsted-Lowry bases consists of anions of weak acids ... [Pg.598]

How do the Arrhenius and Br0nsted-Lowry definitions of an acid and a base differ How are they similar Name two Br0nsted-Lowry bases that are not considered Arrhenius bases. Can you do the same for acids Explain. [Pg.611]

Write balanced equations and K, expressions for these Br0nsted-Lowry bases in water ... [Pg.612]

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