Chemistry acids and bases

Acid-base indicator

A chemical dye that changes color based on the pH of a solution

Titration

A method for using a neutralization reaction to determine the concentration of a solution.

Neutralization

A reaction in which an acid and a base react to product a salt and water.

Classify each compound as an Arrhenius acid or an Arrhenius base. A. H2S. B. RbOH. C. Mg(OH)2. D. H3PO4

A. Acid. B. Base. C. Base. D. Acid.

Common acids and bases use the data in table 8 to answer the following questions A. Which substance is the best basic? B. Which substance is closest to neutral? C. Which has concentration of H^+= 4.0×10^-10M? D. which has a pOH of 11.0?

A. Ammonia. B. Blood. C. pH=-log(H^+)- 9.4=-log(4x10^-10) antacid. D. pOH=11, pH+pOH=14, pH+11=14. pH=3 soft drink.

Reacts with certain metals? Acid, Base, or both?

Acid

Polyprotic

Acid can donate more than one H^+

Bronsted

Acid- H^+ donor, Base- H^+ acceptor

Arrhenius

Acid- H^+ producer, Base- OH^- producer.

Contains more hydrogen ions than hydroxide ions? Acid, Base, or both.

Acid.

Tastes sour? Acid, Base, or both?

Acid.

Arrhenius model

Acids and bases state that and acid contains the element of hydrogen and forms ions of this element when it is dissolved in water. A bass contains the Hydroxide group and dissociates to produce hydroxide ions in aqueous solution

Bases react with... produce a salt and...

Acids, water.

Butter capacity

Amount of acid or base in a buffer solution that can absorb without a significant change in pH

Bronsted-Lowry model

An acid donate hydrogen ions, and a base accepts hydrogen ion's. According to this model, in an acid-base reaction, each acid has a conjugate base, and each base has a conjugate acid.

Salt

An ionic product of an acid-base reaction

Feels slippery? Acid, Base, or both?

Base

Tastes bitter? Acid, Base, or both?

Base

Basis tend to taste... and feel...

Bitter, slippery.

Can turn litmus papers a different color? Acid, Base, or both?

Both

Explain how the definition of a Lewis acid differs from the definition of a Brønsted-Lowry acid.

Brønsted-Lowry- acids give away H^+, bases gain H^+. Lewis- acids accept electron pair bases donate electron pair.

Select a strong acid, and explain how you would prepare a ditlue solution of the acid. Select a weak acid, and explain how you would prepare a concentrated solution of the acid.

Dilute= a little strong acid in a lot of water. Concentration= a lot of weak acid a little of water.

Like acid, aqueous basic solutions contains... are identified as...

Electricity, electrolyte.

Because aqueous acid solutions contains electricity, they are identified as...

Electrolyte.

Lewis

Electron pairs acceptor- acid, electron pairs donate- base

Write a balanced chemical equation that represents the self-ionization of water.

H2O↔️H^++OH^-

What is [OH^-] in an aqueous solution at 298 K in which [H^+]= 5.40x10^-3M?

H3O^+=H^+,OH^-]*[H3O^+]=1x10^-14. X*[5.4x15^-3]=(1x10^-14). (1x10^-14)/(5.4x15^-3). X=1.85x10^-12M.

Formulas for acids contains an H and formulas for bases contains an OH and if they have neither they are considered to be salt.

HBr-acid. Mg(OH)2- Base. KCl-salt.

In terms of ion concentrations, distinguish between acidic, natural, and basic solutions.

H^+ acidic, OH^- basic, H^+=OH^- neutral.

If the concentration of H^+ ions is a aqueous solution decreases, what must happen to the concentrated of OH^- ions? Why?

H^+⬇️, OH^-⬆️. H^+⬆️OH^-⬇️

Acids react with some metals to produce... gas.

Hydrogen

Acids turns... different colors.

Indicators

Bases turn... different colors

Indicators

Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.

Monoprotic- one H^+ can be produced, HCl. Diprotic- two H^+ can be produced, H2SO4. Triprotic- three H^+ can be produced, H3PO4.

Contains equal number of hydrogen and hydroxide ions? Acid, Base, or both?

Neither.

Feels rough? Acid, Base, or both?

Neither.

Acids react with bases to produce a... and water.

Salt

pH scale

Skill using numbers to represent acid and base. If it below 7= acidic. If it is 7 it is neutral. If it is above 7= Basic

Buffer

Solutions that resist changes in pH.

A... taste is a characteristic property of all...

Sour, Acids in aqueous.

Explain the difference between a strong acid and a weak acid

Strong- all of it breaks apart. Weak-some of it breaks apart. Same for bases

End point

The point in a titration in which an indicator changes color

Equivalence point

The stoichiometric point of a titration.

Lithium hydroxide is used to puffy air by removing carbon dioxide. A 25.00 mL sample of lithium hydroxide solution is titrated to an end point by 15.22 mL of 0.3340M hydrochloride acid solution. What is the molarity of the LiOH solution?

Titration: V1*M1=V2*M3, v=volume (L), m=concentration. 0.01522*0.3340=0.025*M2, 0.00508= 0.025*M2, 0.00508/0.025=0.2. M2=0.2

Amphoteric

a substance that can act as both an acid and a base

acid ionization constant (Ka)

equilibrium constant for the ionization of a weak acid

What are the pH and pOH for the solution describe in question 80? ph= 5.40x10^-3. pOH=1.u5x10^-12

pH=-log(H^+)= -log(5.40x10^-3= 2.27. pOH=-log(OH^-)= -log(1.85x10^-12= 11.7