CHEM
What is the conjugate base of HNO2 if it reacts as a Bronsted acid in H2O?
NO2-
The hydrogen phosphate ion, HPO42-, can act as both a Bronsted acid and Bronsted base in water. Select all the options that correctly describe the reaction that occurs when HPO42- acts as a Bronsted base in water.
OH- is one of the products. H2O acts as the Bronsted acid. H2PO4- is one of the products.
An acid donates a proton to form its conjugate _____, which therefore has one less _______atom and one more _________charge than its acid.
base ; hydrogen ; negative
In a Bronsted-Lowry acid-base reaction, the acid reacts to form its _______ ________ and the base will form its ______ ________
conjugate base conjugate acid
In an aqueous solution at a given temperature, the product [H3O+][OH-] has a _____ value. This product is equal to _____ at 25oC.
constant, 1.0 x 10-14
A Bronsted-Lowry acid is a proton _____ and must therefore contain at least one ionizable _____ atom in its formula.
donor; hydrogen
An acid can be defined as a substance that loses one or more H+ ions when dissolved in water. In aqueous solution, the H+ ion combines with H2O to produce the ion, which has the formula H3O+.
hydronium
Which of the following mathematical relationships are correct for an aqueous solution at 25oC? Select all that apply.
pOH + pH = 14.00 pH = -log[H3O+]
True or false: pH is a measure of hydronium ion concentration.
true
Without using a calculator, select the pH below of a solution whose [H3O+] is 2.7 × 10−8 M.
7.57
Which of the following compounds are strong acids? Select all that apply.
HClO4 H2SO4 HI
A compound that can act as either a Bronsted acid or a Bronsted base is said to be
amphoteric
Water functions as ________a(n) in reactions with stronger acids, and functions as a(n) ________in reactions with stronger bases.
base ; acid
Without using a calculator, select the pH below of a solution whose [H3O+] is 1.8 × 10−5 M.
4.74
Which of the following options correctly describe strong acids and bases in aqueous solution? Select all that apply.
For a strong acid in water, [H3O+] is equal to the acid concentration. Strong bases dissociate completely in aqueous solution.
Which of the following formulas can be used to represent the proton in aqueous solution? Select all that apply.
H+ H3O+
Which of the following species could act as EITHER an acid OR a base? Select all that apply.
H2O H2PO4- HCO3-
Which statement correctly explains why even distilled and deionized H2O contains some ions?
H2O can autoionize, producing a small concentration of H3O+ and OH- ions.
The autoionization of water is a process whereby water ionizes to a small extent to form____ ions and_______ ions.
Hydronium ; hydroxide
Select all the statements that correctly describe the acid-base behavior of H2O.
In aqueous HCl, water acts as a Bronsted base. In aqueous NH3, water acts as a Bronsted acid. Water is amphoteric.
How does a conjugate acid compare to its conjugate base? Select all that apply.
The conjugate acid of a neutral base will have a charge of +1. The conjugate acid has one more H than its conjugate base.
Which of the following statements accurately describe Bronsted-Lowry acid-base reactions? Select all that apply.
The reactants and products contain an acid and a base. Some species can act as either an acid or a base depending on the other species present.
Which of the following options correctly represent the relationship between [H3O+] and [OH-] in aqueous solutions at 25oC? Select all that apply.
[H3O+] = 1.0 x 10-14/[OH-] [H3O+][OH-] = 1.0 x 10-14
Which of the following options shows the correct mathematical operation required to calculate [H3O+] for a solution with a pH of 3.52?
[H3O+] = 10-3.52 = 3.0 x 10-4 M
Which of the following gives the correct mathematical operation required to calculate the [H3O+] given a pH of 5.0?
[H3O+] = 10-5.0
A Bronsted-Lowry base is a proton
acceptor
