17. Acid and Base Equilibrium

Identifying Acids and Bases

What Are Acids & Bases? | Chemistry Basics

Weak bases are weak electrolytes that don&#8217;t completely ionize, but instead reach a state of equilibrium.&#160;

The amino acid glycine 1H2N¬CH2¬COOH2 can participate in the following equilibria in water:
H2N¬CH2¬COOH + H2OΔ H2N¬CH2¬COO- + H3O+ Ka = 4.3 * 10-3

H2N¬CH2¬COOH + H2OΔ+H3N¬CH2¬COOH + OH- Kb = 6.0 * 10-5

(b) What is the pH of a 0.050 M aqueous solution of glycine?

Write chemical equations and corresponding equilibrium expressions 
for each of the three ionization steps of phosphoric acid.

Calculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for the change. Assume that the volume remains constant.

What is the concentration of hydroxide ions 3OH-4 in a 
glass of wine with pH = 3.64? (LO 16.5, 16.6) 
(a) 2.3 * 10-4 M (b) 6.4 * 10-3 M 
(c) 6.8 * 10-9 M (d) 4.4 * 10-11 M

Label each of the following as being a strong base, a weak base,
or a species with negligible basicity. In each case write the formula
of its conjugate acid, and indicate whether the conjugate
acid is a strong acid, a weak acid, or a species with negligible
acidity: (a) CH3COO-

With some rules there are exceptions. Oxalic acid and Iodic acid have two more oxygens than hydrogens but are weak acids because carbon are iodine have low electronegativity.&#160;

Morphine is a weak base. A 0.150 M solution of morphine has a 
pH of 10.7. What is Kb for morphine?

They are created by the hydration of nonmetal oxides.&#160;

What Makes Something Acidic? | Acids, Bases & Alkali's | Chemistry | FuseSchool

An acid solution with a concentration of 0.500 M has a 
pH = 3.21. What is the Ka of the acid? (LO 16.8) 
(a) 1.2 * 10-5 (b) 1.7 * 10-6 
(c) 7.6 * 10-7 (d) 5.4 * 10-3

Arrange the following oxides in order of increasing acidity:
K2O, BaO, ZnO, H2O, CO2, SO2.

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
a. HF

Calculate the pH of each acid solution. Explain how the resulting 
pH values demonstrate that the pH of an acid solution should 
carry as many digits to the right of the decimal place as the number 
of significant figures in the concentration of the solution. 
[H3O+] = 0.044 M 
[H3O+] = 0.045 M 
[H3O+] = 0.046 M

Calculate [H3O+] and [OH-] for each solution at 25 °C.
a. pH = 8.55

Write the formula for the conjugate acid of each base.
c. HSO4

Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate
the pH of a solution containing a caffeine concentration of
455 mg>L.

If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate 
the concentration of hydrofluoric acid.

Consider the molecular models shown here, where X represents
a halogen atom. (a) If X is the same atom in both
molecules, which molecule will be more acidic?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b2e0ffaf22da7aaa-1667221411076.jpg" alt="" />

Calculate the percent ionization of a formic acid solution having the given concentration.
d. 0.0500 M

Which of the following solutions is the most basic?
(a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.

Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent dissociation of 0.10 M HN3 in the presence of 0.10 M HCl, and explain the change.

Classify each of the following as a strong acid, weak acid, strong base or weak base.

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true.
(a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table.
(b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms bonded to the central atom.
(c) Hydrotelluric acid 1H2Te2 is a stronger acid than H2S because Te is more electronegative than S.

Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.

Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (c) Calculate the pH of a 0.050 M solution of sodium butyrate.

The following diagrams represent aqueous solutions of
three acids, HX, HY, and HZ. The water molecules have been
omitted for clarity, and the hydrated proton is represented
as H+ rather than H3O+.(c) Which solution would have the highest pH?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/70c40788db5138f8-1666369613336.jpg" alt="" />

Label each of the following as being a strong acid, a weak
acid, or a species with negligible acidity. In each case write the
formula of its conjugate base, and indicate whether the conjugate
base is a strong base, a weak base, or a species with negligible
basicity: (a) HCOOH

(b) Calculate the percent ionization
of 0.0075 M butanoic acid in a solution containing
0.085 M sodium butanoate.

Predict the products of the following acid–base reactions,
and predict whether the equilibrium lies to the left or to the
right of the reaction arrow:
(c) HCO3-1aq2 + F-1aq2 Δ

Determine the concentration of H3O+ to the correct number of 
significant figures in a solution with each pH. Describe how 
these calculations show the relationship between the number 
of digits to the right of the decimal place in pH and the number 
of significant figures in concentration. 
pH = 2.50 
pH = 2.51 
pH = 2.52

<a href="https://www.clutchprep.com/chemistry/strong-acids-and-strong-bases">Strong Acids</a> are strong electrolytes that completely dissociate into ions when dissolved in water.&nbsp;

Which of the following solutions is the most acidic? (a) 0.2 M 
Ba(OH)2, (b) 0.2 M H2SO3, (c) 1.0 M glucose 1C6H12O6).

Which of the following statements is false? 
(a) An Arrhenius base increases the concentration of OH- in water. 
(b) A Brønsted-Lowry base is a proton acceptor. 
(c) Water can act as a Brønsted–Lowry acid. 
(d) Water can act as a Brønsted–Lowry base. 
(e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.

Rank the following oxyacids in terms of increasing acidity.&nbsp;a) HClO3b) HBrO4c) HBrO3d) HClO4

The pH of a 1.00 M solution of urea, a weak organic base, is 
7.050. Calculate the Ka of protonated urea.

Solve an equilibrium problem (using an ICE table) to calculate 
the pH of each solution. 
c. a mixture that is 0.15 M in HF and 0.15 M in NaF

Arrange each group of compounds in order of increasing
acid strength. Explain your reasoning.
(a) HCl, H2S, PH3

Determine the pH of an HF solution of each concentration. In
which cases can you not make the simplifying assumption that
x is small? (Ka for HF is 6.8 * 10-4.)
a. 0.250 M b. 0.0500 M c. 0.0250 M

16.1 Introduction to Acids and Bases | General Chemistry

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
c. CO32 - (aq) + H2O(l )HCO3-(aq) + OH-(aq)

Weak acids are weak electrolytes that don&#8217;t completely ionize, but instead reach a state of equilibrium.&#160;

The following pictures represent solutions of three salts
NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions
have been omitted for clarity.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/c34d2401dde88154-1672692124871.jpg" alt="" />
(b) Which A- anion has the strongest conjugate acid?

A formic acid solution has a pH of 3.25. Which of these
substances will raise the pH of the solution upon addition?
Explain your answer.
a. HCl b. NaBr
c. NaCHO2 d. KCl

Each of the three molecules shown here contains an OH
group, but one molecule acts as a base, one as an acid, and
the third is neither acid nor base. (c) Which one is neither
acidic nor basic?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/ce994a50a2f074cf-1666367325256.jpg" alt="" />

Conversely, metal oxides create bases when hydrated by water.&#160;

The strength of an oxyacid depends on the number of oxygen atoms and the electronegativity of the nonmetal.&#160;

Most acids have one common feature and that is the presence of the hydronium ion, which is represented by H+ or H3O+.

GCSE Chemistry - Acids and Bases  #34

Acids and Bases and Salts - Introduction | Chemistry | Don't Memorise

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
H2SO3

Write the formula for the conjugate base of each acid.
d. HF

Would you expect zirconium(II) oxide, ZrO, to react more
readily with HCl(aq) or NaOH(aq)?

Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.

Calculate the percent ionization of a 0.15 M benzoic acid solution 
in pure water and in a solution containing 0.10 M sodium 
benzoate. Why does the percent ionization differ significantly 
in the two solutions?

Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base:
C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2
A 0.035 M solution of ephedrine has a pH of 11.33. (a) What are the equilibrium concentrations of C10H15ON, C10H15ONH+, and OH-?

Chlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward 
H+1aq2 or OH-1aq2?

The following pictures represent equal volumes of aqueous 
solutions of three acids HA (A = X, Y, or Z); water molecules 
have been omitted for clarity. Which is the strongest 
acid?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/4da721a73d7e4af9-1672687513036.jpg" alt="" />
(a) HX 
(b) HY 
(c) HZ 
(d) All three acids are strong acids and have equal strength.

Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) PO43- or AsO43-

A 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure 
was dissolved in enough water to make 50.0 mL of 
hydrofluoric acid. 
(a) What is the pH of the solution?

Locate sulfur, selenium, chlorine, and bromine in the periodic
table:

(a) Which binary acid 1H2S, H2Se, HCl, or HBr2 is the strongest?
Which is the weakest? Explain.

A 0.100 M solution of chloroacetic acid 1ClCH2COOH2 
is 11.0% ionized. Using this information, calculate 
3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic 
acid.

Label each of the following substances as an acid, base, salt, 
or none of the above. Indicate whether the substance exists in 
aqueous solution entirely in molecular form, entirely as ions, 
or as a mixture of molecules and ions. (d) Ba1OH22.

In qualitative analysis, Ca2+ and Ba2+ are seperated from Na+, K+, Mg2+ by adding aqueous (NH4)2CO3 to a solution that also contains aqueous NH3 (Figure 17.18). Assume that the concentrations after mixing are 0.080 M (NH4)2CO3 and 0.16 M NH3. 
(a) List all the Bronsted-Lowry acids and based present initially, and identify the principal reaction.

Oxycodone 1C18H21NO42, a narcotic analgesic, is a weak base 
with pKb = 5.47. Calculate the pH and the concentrations of 
all species present (C18H21NO4, HC18H21NO4 
+ , H3O+ , and 
OH-) in a 0.002 50 M oxycodone solution.

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
b. CH3NH2(aq) + H2O(l )CH3NH3+(aq) + OH-(aq)

State whether each of the following statements is true or 
false. Justify your answer in each case. 
(b) HCl is a weak acid.

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
a. H2CO3(aq) + H2O(l )H3O+(aq) + HCO3- (aq)

Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base:
C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2
A 0.035 M solution of ephedrine has a pH of 11.33. (b) Calculate Kb for ephedrine.

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
b. NH3(aq) + H2O(l )NH4+(aq) + OH-(aq)

When NO2 is bubbled into water, it is completely converted 
to HNO3 and HNO2: 
2 NO21g2 + H2O1l2S HNO31aq2 + HNO21aq2 
Calculate the pH and the concentrations of all species present 
(H3O+ , OH-, HNO2, NO2 
-, and NO3 
-) in a solution 
prepared by dissolving 0.0500 mol of NO2 in 1.00 L of 
water. Ka for HNO2 is 4.5 * 10-4.

Write the formula for the conjugate base of each acid.
c. HCHO2

Based on molecular structure, arrange the binary compounds in 
order of increasing acid strength. Explain your choice. 
H2Te, HI, H2S, NaH

Based on these molecular views, determine whether each pictured
acid is weak or strong.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/d711d74bbf93eb2e-1660229917472.jpg" alt="" />

Pick the stronger base from each pair.
c. F- or ClO-

When comparing the strengths of different oxyacids remember:

If they have different number of oxygens then the more oxygens the more acidic&#160;

&#160;

Which of the following species behave as strong acids or as
strong bases in aqueous solution?
(a) HNO2 (b) HNO3(c) NH4+ (d) Cl-

Identify the Brønsted–Lowry acid and the Brønsted–Lowry
base on the left side of each of the following equations, and
also identify the conjugate acid and conjugate base of each
on the right side:
(b) 1CH323N1aq2 + H2O1l2Δ1CH323NH +1aq2 + OH -1aq2

Calculate the concentration of all species in a 0.15 M KF solution.

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
c. H2SO4

Label each of the following as being a strong base, a weak base,
or a species with negligible basicity. In each case write the formula
of its conjugate acid, and indicate whether the conjugate
acid is a strong acid, a weak acid, or a species with negligible
acidity: (c) O2-

The following pictures represent solutions of three salts
NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions
have been omitted for clarity.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/5ea3853a611b35b2-1672757043658.jpg" alt="" />
(a) Arrange the three A- anions in order of increasing base 
strength.

Which acid in each of the following pairs has the stronger
conjugate base? See Table 16.1 to compare the relative
strengths of conjugate acid-base pairs.
(a) HCl or HF

Write the formula for the conjugate base of each acid.
b. H2SO3

Positive Amines are considered weak acids.&#160;

Binary acids can be identified by the fact that they all possess an H+ ion attached to an electronegative element.&#160;

Calculate the concentration of all species in a 0.225 M 
C6H5NH3Cl solution.

The following pictures represent aqueous solutions of three 
acids HA1A = X, Y, or Z2; water molecules have been omitted 
for clarity. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/3c396ecb28f53acc-1672780526621.jpg" alt="" /> 
(e) What is the percent dissociation in the solution of HZ?

Indicate whether each of the following statements is correct or incorrect.
(c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases.

Determine the percent ionization of a 0.225 M solution of
benzoic acid.

Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S

An element X reacts with oxygen to form XO2 and with chlorine
to form XCl4. XO2 is a white solid that melts at high temperatures
(above 1000 °C). Under usual conditions, XCl4 is a
colorless liquid with a boiling point of 58 °C. (a) XCl4 reacts
with water to form XO2 and another product. What is the
likely identity of the other product?

Predict the stronger acid in each pair: (c) HBrO3 or HBrO2

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
c. HBr

Acetic acid 1CH3COOH; Ka = 1.8 * 10-52 has a concentration 
in vinegar of 3.50% by mass. What is the pH of 
vinegar? 
(The density of vinegar is 1.02 g/mL.)

Solve an equilibrium problem (using an ICE table) to calculate 
the pH of each solution. 
a. 0.15 M HF

Citric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3). (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make any approximations or assumptions in completing your calculations? (c) Is the concentration of citrate ion 1C6H5O7 3-2 equal to, less than, or greater than the H+ ion concentration?

A vitamin C tablet containing 250 mg of ascorbic acid 
1C6H8O6; Ka = 8.0 * 10-52 is dissolved in a 250 mL glass 
of water. What is the pH of the solution?

In aqueous solution, sodium acetate behaves as a strong 
electrolyte, yielding Na+ cations and CH3CO2 
- anions. A 
particular solution of sodium acetate has a pH of 9.07 and 
a density of 1.0085 g/mL. What is the molality of this solution, 
and what is its freezing point?

Which of the following acids would be classified as the strongest?

Predict the products of the following acid–base reactions,
and predict whether the equilibrium lies to the left or to the
right of the reaction arrow:
(c) NO2-1aq2 + H2O1l2 Δ

Strong Bases are strong electrolytes that completely dissociate into ions when dissolved in water.&#160;

Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.

The acid-dissociation constant for chlorous acid 1HClO22 is
1.1 * 10-2. Calculate the concentrations of H3O+, ClO2-,
and HClO2 at equilibrium if the initial concentration of
HClO2 is 0.0125 M.

Phenylephrine, an organic substance with molecular formula
C9H13NO2, is used as a nasal decongenstant in over-thecounter
medications. The molecular structure of phenylephrine
is shown below using the usual shortcut organic
structure. (a) Would you expect a solution of phenylephrine
to be acidic, neutral, or basic?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/9d536ee4529b2120-1666367467509.jpg" alt="" />

Identify the weakest acid in each of the following sets. 
Explain your reasoning. 
(b) NH3, H2O, H2S

Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) BrO- or BrO2-

Calculate the percent ionization of a formic acid solution having the given concentration.
a. 1.00 M

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true.
(a) Acid strength in a series of H¬A molecules increases with increasing size of A.
(b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom.
(c) The strongest acid known is HF because fluorine is the most electronegative element.

The following pictures represent aqueous solutions of three
acids HA1A = X, Y, or Z2; water molecules have been omitted
for clarity.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b184b631e07f6c08-1672674829268.jpg" alt="" />
(c) Which acid, if any, is a strong acid?

Determine the percent ionization of a 0.125 M HCN solution.

Calculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following concentrations 1Ka is given in Appendix D): (a) 0.250 M

Determine the pH of each solution.
a. 0.10 M NH4Cl

The hydronium ion H3O+ is the strongest acid that can exist 
in aqueous solution because stronger acids dissociate by 
transferring a proton to water. What is the strongest base 
that can exist in aqueous solution?

In nonaqueous solvents, it is possible to react HF to create 
H2F+. Which of these statements follows from this observation? 
(a) HF can act like a strong acid in nonaqueous 
solvents, (b) HF can act like a base in nonaqueous solvents, 
(c) HF is thermodynamically unstable, (d) There is an acid 
in the nonaqueous medium that is a stronger acid than HF.

If your oxyacid has 2 or more oxygens than hydrogens then your oxyacid is a strong acid.&#160;

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
b. HCl

Consider the molecular models shown here, where X represents
a halogen atom. (b) Does the acidity of each molecule increase or decrease as the electronegativity of the atom X increases?

Solve an equilibrium problem (using an ICE table) to calculate 
the pH of each solution. 
b. a solution that is 0.16 M in NH3 and 0.22 M in NH4Cl

Find the pH of each mixture of acids.
a. 0.115 M in HBr and 0.125 M in HCHO2

(a) Calculate the percent ionization of 0.125 M lactic acid 
1Ka = 1.4 * 10-42.

Solve an equilibrium problem (using an ICE table) to calculate 
the pH of each solution. 
b. 0.15 M NaF

(a) Calculate the percent ionization of 0.0075 M butanoic 
acid 1Ka = 1.5 * 10-52.

Acid and base behavior can be observed in solvents other 
than water. One commonly used solvent is dimethyl 
sulfoxide (DMSO), which can be treated as a monoprotic 
acid “HSol.” Just as water can behave either as an acid or a 
base, so HSol can behave either as a Brønsted–Lowry acid 
or base. 
(b) The weak acid HCN has an acid dissociation constant 
Ka = 1.3 * 10-13 in the solvent HSol. If 0.010 mol of 
NaCN is dissolved in 1.00 L of HSol, what is the equilibrium 
concentration of H2Sol + ?

Phenylephrine, an organic substance with molecular formula
C9H13NO2, is used as a nasal decongenstant in over-thecounter
medications. The molecular structure of phenylephrine
is shown below using the usual shortcut organic
structure. (c) Would you expect a solution of
phenylephrine hydrochloride to be acidic, neutral, or basic?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/3ad949aefce75e48-1667222868800.jpg" alt="" />

A 0.185 M solution of a weak acid (HA) has a pH of 2.95.
Calculate the acid ionization constant (Ka) for the acid.

Determine the [OH-] and pH of a solution that is 0.140 M in F-.

Calculate the pH and the percent dissociation of the hydrated
cation in the following solutions. See Appendix C for
the value of the equilibrium constant.
(a) 0.010 M Cr1NO323

Calculate the pH and the percent dissociation of the hydrated 
cation in 0.020 M solutions of the following substances. 
See Appendix C for values of equilibrium constants. 
(a) Fe1NO322

Strychnine 1C21H22N2O22, a deadly poison used for killing 
rodents, is a weak base having Kb = 1.8 * 10-6. Calculate 
the pH of a saturated solution of strychnine (16 mg/100 mL).

Write balanced equations for the following reactions: 
(d) arsenic trioxide with aqueous potassium hydroxide.

A typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic 
acid, C9H8O4), a monoprotic acid having Ka = 3.0 * 10-4. 
If you dissolve two aspirin tablets in a 300 mL glass of water, 
what is the pH of the solution and the percent dissociation?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/7e6faafa38ca60a5-1672822867584.jpg" alt="" />

Calculate [H3O+] and [OH-] for each solution at 25 °C.
b. pH = 11.23

You are asked to prepare a pH = 4.00 buffer starting
from 1.50 L of 0.0200 M solution of benzoic acid
1C6H5COOH2 and any amount you need of sodium benzoate
1C6H5COONa2. (a) What is the pH of the benzoic acid
solution prior to adding sodium benzoate?

A 0.148 M solution of a monoprotic acid has a percent ionization 
of 1.55%. Determine the acid ionization constant (Ka) for the 
acid.

Neutral Amines are considered weak bases.&#160;

Which is a stronger base, S2 - or Se2 -? Explain.

Label each of the following as being a strong base, a weak base,
or a species with negligible basicity. In each case write the formula
of its conjugate acid, and indicate whether the conjugate
acid is a strong acid, a weak acid, or a species with negligible
acidity: (d) Cl-

Any Group 1A metal when combined with OH &#8211;, H &#8211;, O2&#8211; or NH2 &#8211; makes a STRONG BASE.

Complete the table. (All solutions are at 25 °C.)

Identify the weakest acid in each of the following sets. 
Explain your reasoning. 
(a) H2SO3, HClO3, HClO4

Label each of the following substances as an acid, base, salt, 
or none of the above. Indicate whether the substance exists in 
aqueous solution entirely in molecular form, entirely as ions, 
or as a mixture of molecules and ions. (a) HF

Group 2A metals, from Ca2+ to Ba2+, when combined with OH &#8211;, H &#8211;, O2&#8211; or NH2 &#8211; makes a STRONG BASE.&#160;

What is the conjugate acid of HSO3-? What is its conjugate base?

Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate 
the pH of a solution containing an amphetamine concentration 
of 225 mg>L.

Determine the [OH-], pH, and pOH of a 0.15 M ammonia 
solution.

Consider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine?

Identify the Brønsted–Lowry acid and the Brønsted–
Lowry base on the left side of each equation, and also
identify the conjugate acid and conjugate base of each on
the right side.
(a) HBrO1aq2 + H2O1l2ΔH3O+1aq2 + BrO-1aq2

Codeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M 
solution of codeine has a pH of 9.95. Calculate the value of 
Kb for this substance. What is the pKb for this base?

Write the formula for the conjugate base of each acid.
a. HCl

Write balanced equations for the following reactions:
(a) boron trichloride with water

Acids and Bases - Basic Introduction - Chemistry

Label each of the following as being a strong base, a weak base,
or a species with negligible basicity. In each case write the formula
of its conjugate acid, and indicate whether the conjugate
acid is a strong acid, a weak acid, or a species with negligible
acidity: (b) HCO3-

Lactic acid is a weak acid found in milk. Its calcium salt is a
source of calcium for growing animals. A saturated solution of
this salt, which we can represent as Ca(Lact)2, has a
[Ca2 + ] = 0.26 M and a pH = 8.78. Assuming the salt is completely
dissociated, calculate the Ka of lactic acid.

Based on molecular structure, arrange the oxyacids in order of 
increasing acid strength. Explain your choice. 
HClO3, HIO3, HBrO3

Which is the strongest acid? (LO 16.4) 
(a) HClO3 (b) HBrO3 
(c) H2SO3 (d) H2TeO3

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral:
(a) 3H+4 = 0.0505 M

Calculate the H3O+ concentration to the correct number of 
significant figures for solutions with the following pH values. 
(d) 14.25

Calculate the [H3O+] and pH of each polyprotic acid solution.
a. 0.350 M H3PO4

Write balanced net ionic equations and the corresponding 
equilibrium equations for the stepwise dissociation of the 
triprotic acid H3PO4.

Classify each of the following as a strong acid, weak acid, Strong base, or weak base.&nbsp;

Ritalin is the trade name of a drug, methylphenidate, used
to treat attention-deficit/hyperactivity disorder in young
adults. The chemical structure of methylphenidate is
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/9e77557700c36fb7-1661365540940.jpg" alt="" />
(a) Is Ritalin an acid or a base? An electrolyte or a nonelectrolyte?

When looking at a binary acid we look at both electronegativity and size to determine their strength.&#160;

Label each of the following substances as an acid, base, salt, 
or none of the above. Indicate whether the substance exists in 
aqueous solution entirely in molecular form, entirely as ions, 
or as a mixture of molecules and ions. (b) acetonitrile, CH3CN

Determine the pH of an HNO2 solution of each concentration.
In which cases can you not make the simplifying assumption
that x is small?
a. 0.500 M b. 0.100 M c. 0.0100 M

By what factor does 3H+4 change for a pH change of (a) 2.00 units?

The following diagrams represent aqueous solutions of
three acids, HX, HY, and HZ. The water molecules have been
omitted for clarity, and the hydrated proton is represented
as H+ rather than H3O+. (a) Which of the acids is a strong
acid? Explain.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/81ae59795562f20a-1666366931525.jpg" alt="" />

The following picture represents the hydrated metal cation 
M1H2O26 
n + , where n = 1, 2, or 3. 
 
(c) Which M1H2O26n + ion 1n = 1,2, or 32 is the strongest 
acid, and which has the strongest conjugate base?

State whether each of the following statements is true or 
false. Justify your answer in each case. 
(c) Methanol is a base.

You may have been told not to mix bleach and ammonia. 
The reason is that bleach (sodium hypochlorite) reacts with 
ammonia to produce toxic chloramines, such as NH2Cl. 
For example, in basic solution: 
OCl-1aq2 + NH31aq2S OH-1aq2 + NH2Cl1aq2 
(b) The following mechanism has been proposed for this 
reaction in basic solution: 
H2O + OCl-HOCl + OH- Fast, equilibrium constantK1 
HOCl + NH3 S H2O + NH2Cl Slow, rate constantk2 
Assuming that the first step is in equilibrium and the 
second step is rate-determining, calculate the value of 
the rate constant k2 for the second step. Ka for HOCl is 
3.5 * 10-8.

Which base in each of the following pairs has the stronger 
conjugate acid? See Table 16.1 to compare the relative 
strengths of conjugate acid-base pairs. 
(a) Cl- or CO32-

Oxyacids can be identified by the fact that they all possess an H+ ion connected to a nonmetal and oxygen, hence the prefix &#8220;oxy&#8221;.&#160;

Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hydroxylamine.

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral:
(c) a solution in which 3H+4 is 1000 times greater than 3OH-4.

Which is the weakest acid from the following?

Which of the following compound(s) cannot be classified as an acid?A. H2SB. HCNC. H2D. C2H6E. All are acids

Classify each acid as strong or weak. If the acid is weak, write an
expression for the acid ionization constant (Ka).
a. HNO3

Bases are characterized by THREE major features:they may possess metals, they may have a negative charge or they may be an amine.&#160;

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral:
(b) 3H+4 = 2.5 * 10-10 M

A 7.0 mass % solution of H3PO4 in water has a density of
1.0353 g/mL. Calculate the pH and the molar concentrations
of all species present (H3PO4, H2PO4-, PO43-, H3O+ ,
and OH-) in the solution. Values of equilibrium constants
are listed in Appendix C.

Predict the stronger acid in each pair: (e) benzoic acid (C6H5COOH) or phenol (C6H5OH).

Calculate the percent ionization of a formic acid solution having the given concentration.
c. 0.100 M

Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (b) Calculate the pH of a 0.050 M solution of butyric acid.

What is the pH at 25 C of water saturated with CO2 at a 
partial pressure of 1.10 atm? The Henry’s law constant for 
CO2 at 25 C is 3.1 * 10-2 mol>L@atm.

Calculate 3H+4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral:
(b) 3OH-4 = 8.8 * 10-9 M

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
d. C5H5N(aq) + H2O(l )C5H5NH+(aq) + OH-(aq)