Ch. 9 Acids, Bases and Buffers in the Body

Which of the following pH's represents a neutral solution? 5.40 8.65 1.25 7.00

7.00

In a basic solution, pH is ________ and [H3O+] is ________. > 7, < 1 x 10-7 M < 7, < 1 x 10-7 M = 7, 1 x 10-7 M < 7, > 1 x 10-7 M

> 7, < 1 x 10-7 M

Which of the following cannot act as a Bronsted-Lowry acid? H2O HS- HSO4- CO32-

CO32-

In the following equation which is the proton donor and which is the proton acceptor? CO32- (aq) + H2O (l) → HCO3- (aq) + OH- (aq) Donor: OH-; acceptor: HCO3- Donor: CO32-; acceptor: H2O Donor: H2O; acceptor: CO32- Donor: HCO3-; acceptor: OH-

Donor: H2O; acceptor: CO32-

Which of the following buffers is the one that is mainly contained in our blood? H2CO3/HCO3- HPO42-/PO43- NH4+/NH3 HC2H3O2/C2H3O2-

H2CO3/HCO3-

What is the conjugate acid of HS-? H2S S2- HS- S-

H2S

Which of the following is not a strong acid? HCI (aq) HCIO4 HNO3 HC2H3O2

HC2H3O2

Which of the following is the strongest weak acid? NH4+ pKa = 9.20 HCO3- pKa = 10.32 H2PO4- pKa = 7.18 HC2H3O2 pKa = 4.76

HC2H3O2 pKa = 4.76

When a diabetic does not have enough glucose in their blood it develops a condition called: espiratory acidosis respiratory alkalosis metabolic acidosis metabolic alkalosis

metabolic acidosis

When a person does excess vomiting the condition the blood develops is called: respiratory acidosis metabolic alkalosis metabolic acidosis respiratory alkalosis

metabolic alkalosis

[H3O+] = 1.0 x 10^-7M acidic basic neutral

neutral

A Bronsted-Lowry acid is defined as a substnace which: increases [H+] when placed in water acts as a proton acceptor in any system decreases [H+] when placed in water acts as a proton donor in any system

acts as a proton donor in any system

A Bronsted-Lowry base is describes as a substance which: decreases [H+] when placed in water acts as proton acceptor in any system acts as proton donor in any system increases [H+] when placed in water

acts as proton acceptor in any system

Has a slippery feel. acid base

base

Produces OH- in water. acid base

base

If the [H3O+] is less than [OH−] in aqueous solution, then the solution is said to be _____. basic soluble neutral. acidic

basic

[H3O+] - 4.7 x 10^-11M acidic basic neutral

basic

[H3O+] = 1.2 x 10^-8M acidic basic neutral

basic

[H3O+] = 5.6 x 10^-10M acidic basic neutral

basic

[H3O+] = 6.2 x 10^-8M acidic basic neutral

basic

blood, pH = 7.38 acidic basic neutral

basic

drain cleaner, pH = 11.2 acidic basic neutral

basic

A person who overdoses on antacids may neutralize too much stomach acid which causes an imbalance in the bicarbonate equilibrium in their blood. 2H2O(l) + CO2(g) (equilibrium sign) H3O+(aq) + HCO-(aq) How does blood pH change when this occurs? decreases remains the same increases

increases

An Arrhenius acid is defined as a substance which: increases [H+] when placed in water decreases [H+] when placed in water acts as a proton acceptor in any system acts as a proton donor in any system

increases [H+] when placed in water

If the equilibrium constant, K, is greater than 1, then the predominant species in solution at equilibrium are ___. the reactants the products and reactants are present in equal amounts the products there is not enough information to determine which species is predominant

the products

In the lower atmosphere, oxygen is converted to ozone () by the energy provided from lighting. 3O2(g) + heat(equilibrium sign) 2O3(g) What effect does each of the following changes have on the equilibrium? add O2 the reactants are favored the products are favored the equilibrium doesn't shift

the products are favored

In the lower atmosphere, oxygen is converted to ozone () by the energy provided from lighting. 3O2(g) + heat(equilibrium sign) 2O3(g) What effect does each of the following changes have on the equilibrium? raise temperature the reactants are favored the products are favored the equilibrium doesn't shift

the products are favored

In the lower atmosphere, oxygen is converted to ozone () by the energy provided from lighting. 3O2(g) + heat(equilibrium sign) 2O3(g) What effect does each of the following changes have on the equilibrium? add O3 the reactants are favored the products are favored the equilibrium doesn't shift

the reactants are favored

In the lower atmosphere, oxygen is converted to ozone () by the energy provided from lighting. 3O2(g) + heat(equilibrium sign) 2O3(g) What effect does each of the following changes have on the equilibrium? lower the temperature the reactants are favored the products are favored the equilibrium doesn't shift

the reactants are favored

When a system is a equilibrium: the amount of product and reactant is exactly equal. the reaction rate of the reverse reaction is small compared to forward. the reaction rate of the forward reaction is equal to the rate of the reverse. the reaction rate of the forward reaction is small compared to the reverse.

the reaction rate of the forward reaction is equal to the rate of the reverse.

The two products formed as a result of a neutralization reaction are ___. water and a weak acid water and a salt water and a weak base a salt and a strong acid

water and a salt

A buffer will contain relatively equal amounts of which two compounds? A weak acid and a conjugate base A strong acid and the conjugate base of the strong acid A strong base and the conjugate acid of the strong base A strong acid and a strong base

A weak acid and a conjugate base

A person who overdoses on antacids may neutralize too much stomach acid which causes an imbalance in the bicarbonate equilibrium in their blood. 2H2O(l) + CO2(g) (equilibrium sign) H3O+(aq) + HCO-(aq) To treat severe forms of this condition, patients are administered NH4Cl, which acts as a weak acid. How does this restore the bicarbonate equilibrium? Adding acid will bring the pH up. Adding acid will bring the pH down.

Adding acid will bring the pH down.

Which of the following is not a strong base? Al(OH)3 NaOH Ca(OH)2 KOH

Al(OH)3

Which of the following is a correct balanced equation for the neutralization reaction that occurs between AI(OH)3 and HCI(aq)? Al(OH)3 + HCl (aq) → AlCl3 + H2O Al(OH)3 + 3 HCl (aq) → AlCl3 + 3 H2O Al(OH)3 + 3 HCl (aq) → AlCl3 + H+ + OH- Al3+ + OH- + H+ + Cl- → AlCl3 + H2O

Al(OH)3 + 3 HCl (aq) → AlCl3 + 3 H2O

During stress or trauma, a person can start to hyperventilate. The person may then be instructed to breathe into a paper bag to avoid fainting. CO2(g) + 2H2O(l) (equilibrium sign) H3O+(aq) + HCO-3(aq) How does breathing into a paper bag help return the blood pH to normal? Breathing into a bag will increase the CO2 level, which increases H3O+ (by shifting the equilibrium to the right), and lowers the blood pH. Breathing into a bag will decrease the CO2 level, which decreases H3O+ (by shifting the equilibrium to the left), and increases the blood pH. Breathing into a bag will decrease the CO2 level, which increases H3O+ (by shifting the equilibrium to the left), and lowers the blood pH. Breathing into a bag will increase the CO2 level, which decreases H3O+ (by shifting the equilibrium to the right), and increases the blood pH.

Breathing into a bag will increase the CO2 level, which increases H3O+ (by shifting the equilibrium to the right), and lowers the blood pH.

An Arrhenius acid accepts protons. True False

False

During stress or trauma, a person can start to hyperventilate. The person may then be instructed to breathe into a paper bag to avoid fainting. CO2(g) + 2H2O(l) (equilibrium sign) H3O+(aq) + HCO-3(aq) How does blood pH change during hyperventilation? Hyperventilation will increase the CO2 level in the blood, which increases the H3O+ and decreases the blood pH. Hyperventilation will lower the CO2 level in the blood, which decreases the H3O+ and increases the blood pH. The blood pH remains the same.

Hyperventilation will lower the CO2 level in the blood, which decreases the H3O+ and increases the blood pH

When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s) + H2O(g) + heat (equilibrium sign) CO(g) + H2(g) What effect does each of the following changes have on the equilibrium? add H2O The equilibrium shifts to products. The equilibrium shifts to reactants. The equilibrium doesn't shift.

The equilibrium shifts to products.

When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s) + H2O(g) + heat (equilibrium sign) CO(g) + H2(g) What effect does each of the following changes have on the equilibrium? add heat The equilibrium shifts to products. The equilibrium shifts to reactants. The equilibrium doesn't shift.

The equilibrium shifts to products.

When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s) + H2O(g) + heat (equilibrium sign) CO(g) + H2(g) What effect does each of the following changes have on the equilibrium? remove CO The equilibrium shifts to products. The equilibrium shifts to reactants. The equilibrium doesn't shift.

The equilibrium shifts to products.

When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s) + H2O(g) + heat (equilibrium sign) CO(g) + H2(g) What effect does each of the following changes have on the equilibrium? lower temperature The equilibrium shifts to products. The equilibrium shifts to reactants. The equilibrium doesn't shift.

The equilibrium shifts to reactants.

When does a reversible reaction reach equilibrium? The rates of the forward and reverse reactions are equal. The rates of the forward reaction is less than the rate of the reverse reaction. The rates of the forward reaction is higher than the rate of the reverse reaction.

The rates of the forward and reverse reactions are equal.

Carbonic acid has a K a value of 4.5×10−7. Based on this value, carbonic acid can be classified as a _____. a weak acid a weak base a strong base a strong acid

a weak acid

Donates a proton. acid base

acid

Neutralized by a base. acid base

acid

CO32-(aq) + H2O(l) (equilibrium symbol) HCO3-(aq) + OH-(aq) acid (proton donor) H2O, base (proton acceptor) CO2-3 acid (proton donor) CO2-3, base (proton acceptor) H2O

acid (proton donor) H2O, base (proton acceptor) CO2-3

NH3(aq) + H2O(l) (equilibrium symbol) NH4+(aq) + OH-(aq) acid (proton donor) H2O, base (proton acceptor) NH3 acid (proton donor) NH3, base (proton acceptor) H2O

acid (proton donor) H2O, base (proton acceptor) NH3

F-(aq) + H2O(l) (equilibrium symbol) HF(aq) + OH-(aq) acid (proton donor) H2O, proton acceptor (base) F- acid (proton donor) F-, proton acceptor (base) H2O

acid (proton donor) H2O, proton acceptor (base) F-

H2SO4(aq) + H2O(l) --> H3O+(aq) + HSO4-(aq) acid (proton donor) H2SO4, proton acceptor (base) H2O acid (proton donor) H2O, proton acceptor (bade) H2SO4

acid (proton donor) H2SO4, proton acceptor (base) H2O

HCN(aq) + NO-2(aq) (equilibrium sign) CN-(aq) + HNO2(aq) acid HCN; conjugate base CN- base NO-2; conjugate acid HNO2 base HCN; conjugate acid CN- acid NO-2; conjugate base HNO2

acid HCN; conjugate base CN- base NO-2; conjugate acid HNO2

HSO-4(aq) + H2O(l) (equilibrium sign) H3O_(aq) _ SO 2-4(aq) acid HSO-4; conjugate base SO2-4 base H2O; conjugate acid H3O+ base HSO-4; conjugate acid SO2-4 acid H2O; conjugate base H3O+

acid HSO-4; conjugate base SO2-4 base H2O; conjugate acid H3O+

NH+4(aq) + H2O(l) (equilibrium sign) H3O+(aq) + NH3(aq) acid NH+4; conjugate base NH3 base H2O; conjugate acid H3O+ base NH+4; conjugate acid NH3 acid H2O; conjugate base H3O+

acid NH+4; conjugate base NH3 base ; conjugate acid H3O+

[H3O+] = 1.8 x 10^-6M acidic basic neutral

acidic

[H3O+] = 5 x 10^-2M acidic basic neutral

acidic

[H3O+] = 7.0 x 10^-3M acidic basic neutral

acidic

coffee, = 5.5 acidic basic neutral

acidic

vinegar, pH = 2.8 acidic basic neutral

acidic

During stress or trauma, a person can start to hyperventilate. The person may then be instructed to breathe into a paper bag to avoid fainting. CO2(g) + 2H2O(l) (equilibrium sign) H3O+(aq) + HCO-3(aq) What is this condition called? respiratory alkalosis metabolic acidosis

respiratory alkalosis

When a person hyperventilates the condition is known as: respiratory acidosis metabolic alkalosis respiratory alkalosis metabolic acidosis

respiratory alkalosis

A person who overdoses on antacids may neutralize too much stomach acid which causes an imbalance in the bicarbonate equilibrium in their blood. 2H2O(l) + CO2(g) (equilibrium sign) H3O+(aq) + HCO-(aq) In which direction will the bicarbonate equilibrium shift during an Alka-Seltzer® overdose? shift to the left remain the same shift to the right

shift to the left

During stress or trauma, a person can start to hyperventilate. The person may then be instructed to breathe into a paper bag to avoid fainting. CO2(g) + 2H2O(l) (equilibrium sign) H3O+(aq) + HCO-3(aq) In which direction will the bicarbonate equilibrium shift during hyperventilation? shift to the left shift to the right remain the same

shift to the left

A person who overdoses on antacids may neutralize too much stomach acid which causes an imbalance in the bicarbonate equilibrium in their blood. 2H2O(l) + CO2(g) (equilibrium sign) H3O+(aq) + HCO-(aq) In which direction will the bicarbonate equilibrium shift as the pH returns to normal? shift to the right shift to the left remain the same

shift to the right

During stress or trauma, a person can start to hyperventilate. The person may then be instructed to breathe into a paper bag to avoid fainting. CO2(g) + 2H2O(l) (equilibrium sign) H3O+(aq) + HCO-3(aq) In which direction will the bicarbonate equilibrium shift as the pH returns to normal? shift to the left remain the same shift to the right

shift to the right

Hydrogen chloride can be made by reacting hydrogen gas and chlorine gas. H2(g) + Cl2(g)(equilibrium sign) 2HCl(g) + heat What effect does each of the following changes have on the equilibrium? add H2 the equilibrium shifts to products the equilibrium shifts to reactants the equilibrium doesn't shift

the equilibrium shifts to products

Hydrogen chloride can be made by reacting hydrogen gas and chlorine gas. H2(g) + Cl2(g)(equilibrium sign) 2HCl(g) + heat What effect does each of the following changes have on the equilibrium? remove HCl the equilibrium shifts to products the equilibrium shifts to reactants the equilibrium doesn't shift

the equilibrium shifts to products

Hydrogen chloride can be made by reacting hydrogen gas and chlorine gas. H2(g) + Cl2(g)(equilibrium sign) 2HCl(g) + heat What effect does each of the following changes have on the equilibrium? add heat (raise temperature) the equilibrium shifts to products the equilibrium shifts to reactants the equilibrium doesn't shift

the equilibrium shifts to reactants

Hydrogen chloride can be made by reacting hydrogen gas and chlorine gas. H2(g) + Cl2(g)(equilibrium sign) 2HCl(g) + heat What effect does each of the following changes have on the equilibrium? remove Cl2 the equilibrium shifts to products the equilibrium shifts to reactants the equilibrium doesn't shift

the equilibrium shifts to reactants

After you o[en a bottle of soda, the drink eventually goes flat. How can Le Chatelier's principle explain this using the following reaction? H+(aq) + HCO3-(AQ) (equilibrium sign) CO2(g) + H2O(l) the escape of CO2 gas removes CO2; equilibrium favors the formation of the reactants. The soda no longer bubbles. the escape of CO2 gas removes CO2; equilibrium favors the formation of the products. The soda no longer bubbles.

the escape of CO2 gas removes CO2; equilibrium favors the formation of the products. The soda no longer bubbles.