chem test idk abt what though

substances that can act as both an acid and a base are said to be amphoteric

true

the state of equilibrium is dynamic and not static

true

adjusting the concentration of either the reactants or products in a reaction does not put stress on the equilibrium

false

a single arrow in a reaction means that the reaction goes to completion

false

the Arrhenius model states that acid and bases share elctron paris

falso

for a given reaction at a given temperature, keq will vary depending on the initial concentration of the reactants and products

false

an acid is an ion or molecule with a long electron pair that it can donate or share

true

determine the hydrogen ion concentration of 0.500M aqueous solution of NaOH. The ionization product constant for water, Aw is 1.00 × 10^-14

2.00 × 10^-14M

In the Bronstead-Lowry model of acids and bases, a(n) _____ is a hydrogen donor and a(n) ______is a hydrogen acceptor

conjugate acid, conjugate base

If the equilibrium constant is very large

more products that reactant exist at equilibrium

a _______ is produced when a base accepts a hydrogen ion from an acid

conjugate base

when acids react with metals, they produce _____ gas

hydrogen

a basic solution contains more ____ ions than hydrogen

hydroxide

during a titration the pH is read and recorded until the equivalence point is reached, What is the equivalence point below?

moles of H+ ions = moles of OH^- ions

In the reaction SO2Cl2—SO2 + Cl2, heat is evolved. What happens when chlorine (Cl2) is added to the equilibrium mixture at constant volume?

the temperature of the system decreases

a solution that contains equal concentrations of hydrogen and hydroxide ions is

neutral

Calculate the hydrogen ion concentration of an aqueous solution, given the pOH of the pollution is4.50 and the ion product constat for water, Kw is 1.00x10^-14.

3.16x10^-10M

a decrease in the concentration of reactant cause the rate of the _______ reaction to slow

forward

keq-1: reactants are favored at equilibrium

<

if the pH of a solution is changed from 12 to 9. How does the hydrogen ion concentration change?

increased by a factor of 1000

the hydrogen ion concentration of fruit juice is 2.5 × 10^0.5M. What is the pH of the juice?

4.6

acetic acid is a weak monoprotic acid. it is the active ingredient in vinegar. if the initial concentration of acetic acid is 0.200M and the equilibrium concentration of H3O+ is 0.0019M, calculate the Ka=Keq for acetic acid

1.8 × 10^-5

in an exothermic reaction, equilibrium shifts ____ when temperature is lowered

to the right

in an exothermic reaction, equilibrium shifts ____ when temperature is raised

to the left

which model states that an acid is a substance that contains hydrogen and ionized to produce hydrogen ions

arrhenius

the equilibrium constant for their reaction at 700.0K is 0.44. H2O (g)+CO(g)←→ H2(g)+CO2(g)

0.075mol/L

what is the pH of 0.45 M of H2SO4?

0.045

which of the following factors will NOT change to concentration of ammonia (NH3) is the reaction N2(g) +3H2(g) ←-> 2NH3 (g) when (triagnle)H=-xkJ

increase in the amount of catalyst

calculate the pOH of a 0.350 Ba(OH)2 solution

1.55 × 10^-1

an acid that can donate only one hydrogen ion is called a

monoprotic acid

According the Le Chatelier’s principle, when the volume is increased, the equilibrium shifts to the right foronly one the following. For Which of the following reversible reactions is the true?

PCl5(g)←→ PCl3(g)+CL2

a _____ reaction is a chemical reaction that can occur in both the forward and reverse directions

reversible

the hydrogen ion concentration is increased by 100. What would be the corresponding change on the pOH scale

increased by 2in

in this reaction, which of the following factors will NOT change the concentrate of CO2 in the reaction? H2O(g)+CO(g)<--> H2(g) +CO2 (g)

an increase in the amount of catalyst

calculate the hydrogen ion concentration of an aquaseous solution given the concentration of hydroxide ions is 1 × 10^-5 M and the ion constant for water in 1 × 10^-14

1 × 10^-9

what is the base ionization constant expression for ammonia?

Kb = [NH4-][OH^-]/[NH3]

an aqueous solution has a pH of 4.1 at 298K. Calculate the pOH of the aqueous solution

9.9

what is the pH of bloodm given the hydrogen ion concentration is 4.0 × 10^-8M?

7.4

the general equation for a reaction at equilibrium is as follows

aA+bB←→ cC+dD

the pH scale allows scientists to define that acidity of a substance on a scale of

0-14

calculate the pH of 0.45 M H2SO4-

pH=-log(0.45); 0.35

what is the molarity of HCI given the following 17.0mL of the unknown (HCI) is placed in a flask with 15.0mL of water. It is titrated with 23.7 mL of 0.250M MaOH when the analyte turns a fainth pink color

0.348M

calculate the molarity of a solution containing 0.20 mol of sodium hydroxide dissovled in 0.50 L of water.

0.40

during a titration a 0.250M NaOH solution is used but the original solution of NaOH had a concentration of 5.00M, What volume of the 5.00M NaOH must be added to water to make 3.500L of the dilute solution?

175mL

how many grams of NaOH are needed to make 1.75L of 2.25M solution

157.6g NaOH