Chemistry I Accelerated
Study Guideline - Chapter 19
Acids, Bases and Salts
-----------------------------------------------------------------------------By the end of this unit, the skills you should be able to demonstrate
are:
1. List properties of acids and bases.
2. Define and Give Examples of Arrhenius acids and bases.
3. Classify substances as acids or bases, and identify conjugate acidbase pairs in acid-base reactions, using the Brønstead-Lowry
theory.
4. Classify substances as Lewis acids or bases.
5. Complete and balance a neutralization reaction.
6. Categorize acids and bases as strong or weak using Ka and Kb and
give examples of each.
7. Derive and Use ionization constants.
8. Define acidic and basic anhydrides. Write formulas for them.
9. Write the equation for the self-ionization of water.
10. Classify a solution as neutral, acid or base given the hydrogen-ion
or hydroxide ion concentration.
11. Calculate the pH or the pOH of a solution given either the
hydrogen or hydroxide ion concentration.
12. Describe the processes of hydrolysis and buffering.
13. Describe at least two methods used to measure pH.
14. State the principles and uses of indicators.
15. Explain the process of titration and perform calculations using the
data from titrations.
Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Chemistry Video: Acids, Bases and Salts
1. What do acids, bases and salts form in solution?
2. Why are acids, bases and salts called electrolytes?
3. How are nerve cells like a battery?
4. Litmus turns what color in acid? Base?
5. What does an acid do in solution?
+
6. What is H3O called?
7. What is the general rule about oxides and acids and bases?
8. What is a more useful definition for acids and bases using the term proton?
9. What is the Lewis theory of acids and bases?
10. What does strong and weak refer to with acids and bases?
11. Can water molecules form ions by themselves?
12. What does pH stand for?
13. What pH is Acid? Neutral? Base?
14. What is a buffer?
15. How many buffers are in human blood?
16. What is a salt?
page 2
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Defining Acids and Bases
On the line next to the item, write “A” if the statement is a property of an acidic solution.
Write “B” if it is a property of a basic solution, and write “X” if it is a property of both
acidic and basic solutions.
_____
_____
_____
_____
_____
1. Often feels smooth and slippery
3. Stings in open wounds
5. has a bitter taste
7. is an electrolyte
9. turns litmus paper from red to blue
_____
_____
_____
_____
_____
2. has a sour taste
4. reacts vigorously with metals
6. turns litmus paper from blue to red
8. often looks like pure water
10. does not usually react with metals
Answer the following questions.
11. What is the Arrhenius definition of acids and bases?
12. What is the Brønsted-Lowery definition of acids and bases?
13. Why might ammonia not be considered a base according to the Arrhenius definition while the
ammonium ion is considered an acid?
14. Why is the Brønsted-Lowery definition of acids and bases considered more encompassing than the
Arrhenius definition?
15. Why are Brönsted-Lowery acids and bases sometimes called proton donors and acceptors?
16. What is the Lewis definition of acids and bases?
Define each of the following:
17. Acidic Hydrogens
18. Binary Acids
19. Oxy acids
20. Carboxylic acid
21. Amines
page 3
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Name the following acids and bases
____________________ 22. HNO3
____________________ 23. H3PO3
____________________ 24. HClO
____________________ 25. KOH
____________________ 26. H2SO4
____________________ 27. H2CO3
____________________ 28. HC2H3O2
____________________ 29. CH3NH2
Complete each of the following sentences by filling in the appropriate word or phrase
from the list below.
Word List
amphoteric
hydronium ion
acid-base indicator
neutralization reaction
conjugate
salt
electrolyte
30. An ionic compound that forms from an acid-base neutralization reactions is a(n)
_________________.
31. A(n) __________________ is a substance that conducts electricity when dissolved in water.
+
32. The formula H3O represents a(n) ______________ _______.
33. The reaction between an acid and a base is called a(n) ______________ _______________.
34. A(n) ________–________ _______________ turns one color in an acidic solution and another color
in a basic solution.
–
35. The chloride ion (Cl ) is the __________________ base of hydrochloric acid (HCl).
Reviewing Acids and Bases
Determine whether each of the following compounds contains an acidic hydrogen.
Explain your answers
1. Nitric Acid
2. Hydrobromic acid
3. Methane
4. Hydrogen gas
page 4
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
For the following reactions write the formula equation, place a single arrow (-->) between
the reactants and the products if the reaction goes to completion. Place a double arrow
(<-->) if the reaction reaches equilibrium. For each reaction label the acid (A), the base
(B), the conjugate acid (CA), and the conjugate base (CB).
5. Nitrous Acid (aq) plus water (l)
Hydronium (aq) and nitrite (aq) ions
6. Hydrocyanic Acid (aq) plus water (l)
Hydronium (aq) and cyanide (aq) ions
7. Nitric acid (aq) plus water
hydronium ion (aq) plus nitrate ion (aq)
8. Acetic acid (aq) plus water
hydronium ion (aq) plus acetate ion (aq)
9. Ammonia (aq) plus water
hydroxide ion(aq) plus ammonium ion(aq)
10. hydronium ion (aq) plus hydroxide ion (aq)
water plus water
Acid-Base Constant Practice Problems
1. Acetic acid is a weak acid. If the initial concentration of acetic acid is 0.200 M and the equilibrium
concentration of hydronium ion is .0019 M, calculate the Ka for acetic acid.
–
+
–
+
HA + H2O ---> A + H3O >>>> Ka = [A ][H3O ]/[HA]
For every one hydronium ion that forms, one conjugate base must also form so if those concentrations
started equal they must end equal. Also for every hydronium ion and conjugate base that forms, one
acid must have dissociated.
Therefore, the starting concentration, 0.200 M minus the amount that dissociated, 0.0019 M equals the
final or equilibrium concentration of 0.1981 M
2
–5
–5
Calculating Ka = (0.0019)(0.0019)/0.1981 or (0.0019) /0.1981 = 1.82 x 10 or in sig. dig. 1.8 x 10
In most cases for weak acids the initial and the equilibrium concentrations are essentially the same.
Does subtracting the amount dissociated make a difference? Let’s compare and find out:
2
–5
Calculating Ka = (0.0019) /0.200 = 1.805 x 10
–5
or in sig. dig. 1.8 x 10
(no difference)
2. Ammonia is a weak base. If the initial concentration of ammonia is 0.150 M and the equilibrium
–3
concentration of hydroxide ion is 1.6 x 10
M, calculate the Kb for ammonia.
page 5
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
3. Butylamine is a weak base. If the initial concentration of butylamine is 0.230 M and the equilibrium
–6
concentration of hydroxide ion is 8.6 x 10
M, calculate the Kb for butylamine.
4. Formic acid is a weak monoprotic acid made by ants. If the initial concentration of the formic acid is
–3
0.10 M and the equilibrium concentration of hydronium ion is 4.2 x 10
formic acid.
M, calculate the Ka for
5. Isobutylamine is a weak base. If the initial concentration of isobutylamine is 0.055 M and the
–3
equilibrium concentration of hydroxide ion is 4.0 x 10
M, calculate the Kb for isobutylamine.
6. Gallic acid is a weak monoprotic acid. If the initial concentration of the gallic acid is 0.280 M and the
–3
equilibrium concentration of hydronium ion is 3.3 x 10
M, calculate the Ka for gallic acid.
7. Triethylamine is a weak base. If the initial concentration of triethylamine is 0.390 M and the
–3
equilibrium concentration of hydroxide ion is 4.4 x 10
M, calculate the Kb for triethylamine.
8. Dipropylamine is a weak base. If the initial concentration of dipropylamine is 0.160 M and the
equilibrium concentration of hydroxide ion is 0.012 M, calculate the Kb for dipropylamine.
9. Uric acid is a weak monoprotic acid made by ants. If the initial concentration of the uric acid is 0.110
–2
M and the equilibrium concentration of hydronium ion is 3.4 x 10
acid.
M, calculate the Ka for uric
10. Hydrocyanic acid is a weak monoprotic acid. If the initial concentration of the Hydrocyanic acid is
–2
0.150 M and the equilibrium concentration of hydronium ion is 4.8 x 10
cyanic acid.
11.
M, calculate the Ka for
0.230 mol of a weak base is dissolved in water to a total volume of 1.5 L. At equilibrium the
concentration of hydroxide ion is 0.0040 M, calculate the Kb for this base.
page 6
ChemIAcc-19Acids,Bases,Salts WS
12.
Dr. Corell - Chemistry I Accelerated
0.690 mol of a weak acid is dissolved in water to a total volume of 0.75 L. At equilibrium the
concentration of hydronium ion is 0.0024 M, calculate the Ka for this acid.
Predict whether the final solution in each situation will be acidic, basic, neutral or if it is
impossible to predict. In all cases you can assume equal concentrations of acid and base
are used.
13. A strong acid reacts with a strong base
13. __________________
14. A strong acid reacts with a weak base
14. __________________
15. A weak acid reacts with a strong base
15. __________________
16. A weak acid reacts with a weak base
16. __________________
Acid-Base Hydrolysis
Hydrolysis occurs when certain salts dissolve in water to form solutions that have acidic
or basic properties. A rule for predicting the properties of solutions of salts is based upon
the concept of strong acids and strong bases in the Arrhenius sense. The rules are
summarized in the table below:
Salt formed from
Water solution exhibits
Example
Strong acid + strong base
Strong acid + weak base
no hydrolysis - neutral solutions
hydrolysis to form acidic solution
FeSO4
Weak acid + strong base
hydrolysis to form basic solution
Na2CO3
Weak acid + weak base
Must use Ka and Kb to determine
Pb(C2H3O2)2
KCl
The commonly used strong acids are hydrochloric, nitric and sulfuric. The commonly
used strong bases are sodium hydroxide, potassium hydroxide, and calcium hydroxide.
Predict the hydrolysis effect of each of the following salts. For each answer write acidic,
basic neutral or need Ka and Kb.
____________________ 1. Na3PO4
____________________ 2. Na2SO4
____________________ 3. NaC2H3O2
____________________ 4. NH4NO3
____________________ 5. NH4Cl
____________________ 6. Fe3(PO4)2
____________________ 7. Ca(NO3)2
____________________ 8. KC2H3O2
____________________ 9. CuSO4
____________________ 10. Al(NO3)3
____________________ 11. NaCl
____________________ 12. K2CO3
page 7
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Any oxygen-containing substance that will produce an acid when dissolved in water is
called an acid anhydride. Any oxygen-containing substance that will produce a base
when dissolved in water is called an basic anhydride. Anhydride means without water.
Metal oxides tend to form basic anhydrides and nonmetal oxides tend to form acidic
anhydrides.
Predict the acidic or basic nature of the following anhydrides:
____________________ 13. CaO
____________________ 14. NO
____________________ 15. CO2
____________________ 16. SO3
____________________ 17. Na2O
____________________ 18. Rb2O
Complete and balance the following:
19.
CaO + H2O ---------->
20.
CO2 + H2O ---------->
21.
Na2O + H2O ---------->
22.
SO3 + H2O ---------->
Determining the Strengths of Acids and Bases
If the statement is true, write “true”. If it is false change the underlined word(s) to make
the statement true.
+
_________________ 1. A strong acid readily transfers H ions to water to form hydronium ions.
_________________ 2. Strong acids are weak electrolytes.
_________________ 3. Substances that have the strongest affinity for hydrogen ions are strong bases.
_________________ 4. Weak acids do not completely ionize in water.
_________________ 5. The stronger an acid, the stronger its conjugate base.
_________________ 6. Salts are weak electrolytes.
Answer the following questions
7. What do acid and base dissociation constants measure?
8. What are salt-hydrolysis reactions?
page 8
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
9. Why is spilling 1 M acetic acid relatively harmless compared to spilling 1 M hydrochloric acid?
10. Defend or refute this statement: Strong acids are strong electrolytes.
11. Describe the relative strength of acids and their conjugate bases. Bases and their conjugate acids.
Kw/pH problems
1. What is the hydroxide ion concentration in saturated limewater if hydronium ion concentration = 3.98
–13
x 10
M? Is limewater acidic, basic, or neutral?
+
–8
2. What is the [H3O ] in a wheat flour and water solution if hydroxide ion concentration = 1.00 x 10
M? Is wheat flour and water acidic, basic, or neutral?
3. What is the hydronium ion concentration in 0.1 M ammonia if hydroxide ion concentration = 1.26 x
–3
10
M? Is ammonia acidic, basic, or neutral?
–7
4. What is the hydroxide ion concentration in butter if hydronium ion concentration = 6.00 x 10
butter acidic, basic, or neutral?
M? Is
5. During the course of the day, human saliva varies between acidic and basic. What is the hydronium
–8
ion concentration in saliva if hydroxide ion concentration = 3.16 x 10
acidic, basic, or neutral?
+
M? Is this sample of saliva
–11
6. What is the [H3O ] in peaches if hydroxide ion concentration = 3.16 x 10
basic, or neutral?
page 9
M? Are peaches acidic,
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
7. What is the hydroxide ion concentration in 0.1 M bicarbonate of soda if hydronium ion concentration
–9
= 3.98 x 10
M? Is bicarbonate of soda acidic, basic, or neutral?
–8
8. A sample of human blood is found to have a hydronium ion concentration = 3.72 x 10
the pH of this sample? Is it acidic, basic, or neutral?
M? What is
–8
9. Analysis of samples of maple syrup reveals that the hydroxide ion concentration = 5.00 x 10
What is the pH of this syrup? Is it acidic, basic, or neutral?
M.
–5
10. In a sample of bananas and water it was found that the hydronium ion concentration = 2.51 x 10
M. What is the pH of this sample? Is it acidic, basic, or neutral?
–9
11. A soft drink was found to have a hydroxide ion concentration = 4.11 x 10
this soft drink? Is it acidic, basic, or neutral?
–5
12. Tomatoes are found to have a hydronium ion concentration = 6.20 x 10
these tomatoes? Are they acidic, basic, or neutral?
M? What is the pH of
M? What is the pH of
–6
13. A sample of urine is found to have a hydronium ion concentration = 6.30 x 10
of this sample? Is it acidic, basic, or neutral?
–10
14. In sour pickles the hydroxide ion concentration = 1.60 x 10
Are they acidic, basic, or neutral?
page 10
M? What is the pH
M. What is the pH of the pickles?
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
The self-ionization of Water and pH
Matching - On the line at the left, write the letter of the definition that best matches each
term.
+
–7
_____ 1. self-ionization
a. has H3O concentration greater than 1 x 10
_____ 2. pure water
b. has H3O and OH concentrations of 1 x 10
_____ 3. ion-product constant
c. has pH greater than 7
_____ 4. pH scale
d. describes this reaction: H2O + H2O <-----> H3O + OH
_____ 5. acidic solution
e. has pH = 7; may contain ions other than H3O + OH
_____ 6. basic solution
f. is equal to 1 x 10
_____ 7. neutral solution
g. describes acidity or basicity of a solution
+
–
M
–7
M
+
+
–14
+
–
–
at 25°C
–
8. In pure water, what is the concentration of H3O + OH ions? What is the pH?
+
9. The pH of a solution decreases from 9 to 7. How does the [H3O ] change? By what factor?
True or False - If the statement is true, write “true”. It is false, change the underlined
word or words to make the statement true.
+
–
_________________ 10. In the reaction H2O + H2O <-----> H3O + OH , products are favored.
_________________ 11. The ion product constant applies to every water solution at a given
temperature.
+
_________________ 12. An acidic solution contains only H3O ions.
_________________
_________________
_________________
_________________
13. A solution with a pH of 4 is acidic.
14. A buffer is usually made up of a weak acid or base and its salt.
15. An increase in the concentration of a buffer decreases the buffer capacity.
16. The pH of a solution remains constant in the presence of a buffer if acid or a
base is added beyond the buffer capacity.
–
_________________ 17. Adding OH ions beyond the buffer capacity causes a decrease in the pH.
+
–
_________________ 18. All buffers have a limited capacity to neutralize H3O + OH ions.
_________________ 19. Indicators are made from neutral solutions.
In each of the following situations, determine if the pH is decreased, increased or remains
constant.
_________________ 20. Acid is added to a buffered solution until the buffer capacity is surpassed.
_________________ 21. Base is added to a buffered solution, not exceeding the buffer capacity.
_________________ 22. Base is added to a buffered solution, until the buffer capacity is surpassed.
_________________ 23. Acid is added to a buffered solution, not exceeding the buffer capacity.
page 11
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
24. What is the function of a buffer in blood? Why is it so important?
25. How can large changes in pH levels affect reactions?
26. What happens at the molecular level when an acid is added to a buffer solution? What about a base?
27. An acid is added to a buffer solution of acetic acid and its conjugate base. Write the equation for the
reaction that occurs.
28. A base is added to a buffer solution of ammonia and its conjugate acid. Write the equation for the
reaction that occurs
Titration Practice Problems
1. A volume of 30.0 mL of 0.25 M hydrochloric acid neutralizes a 50.0 mL sample of potassium
hydroxide. What is the concentration of the potassium hydroxide?
2. A volume of 46.0 mL of 0.40 M sodium hydroxide neutralizes an 80.0 mL sample of hydrocyanic
acid. What is the concentration of the hydrocyanic acid?
3. A volume of 90.0 mL of 0.20 M hydrobromric acid neutralizes a 60.0 mL sample of sodium
hydroxide. What is the concentration of the sodium hydroxide?
page 12
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
4. A volume of 50.0 mL of 0.30 M hydrochloric acid neutralizes a 60.0 mL sample of calcium
hydroxide. What is the concentration of the calcium hydroxide?
5. A volume of 20.0 mL of 0.25 M Aluminum hydroxide neutralizes a 75.0 mL sample of sulfuric acid.
What is the concentration of the sulfuric acid?
6. A volume of 135.0 mL of 0.40 M hydrosulfuric acid neutralizes a 90.0 mL sample of aluminum
hydroxide. What is the concentration of the aluminum hydroxide?
7. A mass of 2.91 g of hydrobromric acid neutralizes a 80.0 mL sample of calcium hydroxide. What is
the concentration of the calcium hydroxide?
21
8. A total of 4.51 x 10 formula units of sodium hydroxide neutralizes a 30.0 mL sample of
phosphorous acid. What is the concentration of the phosphorous acid?
Acids - Bases Titration
acid-base titration
phenolphthalein
end point
standard solution
equivalence point
titration curve
indicator
1. The point at which exactly enough standard solution is added to neutralize the unknown solution is
the ______________________.
2. A(n) ______________________ is used to represent pH data.
3. A(n) ______________________ is a carefully controlled neutralization reaction.
4. A(n) ______________________ changes color at certain pH values.
5. A(n) ______________________ contains an acid or a base in known concentration.
6. A common indicator used in titrations is ______________________.
7. The point at which the indicator changes color is the ______________________ of the reaction.
page 13
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
8. Why is it difficult to directly measure the concentration of a weak acid such as acetic acid?
9. How is an indicator useful in a titration?
10. Why should the end point of a titration be close to the equivalence point.
Acids and Bases - Review Activity
acid
acidic solution
basic solution
conjugate pair
equivalence point
hydronium ion
ionization
logarithm
nonelectrolyte
proton donor
standard solution
strong electrolyte
weak electrolyte
acid-base neutralization
amphoteric substance
Brönsted-Lowry definition
dissociation
hydrogen ion
hydroxide ion
ionization constant
neutral solution
pH
salt
strong conjugate acid
weak conjugate acid
acid-base titration
base
buffer
end point
hydrolysis
ion–product
indicator
neutralization
proton acceptor
self–ionization
strong conjugate base
weak conjugate base
A substance whose water solution does not conduct an electric current is called a(n)
________________. A substance whose water solution is a poor conductor is a (n) _____
_____________. One whose solution is a good conductor is a(n) ______ ____________. The ability to
conduct an electric current can result from __________________, the action of water on ionic solids to
produce and dispense hydrated ions. The ability to conduct can also result from ________________,
the formation of charged particles by means of the reaction between water molecules and molecular
substances.
According to Arrhenius, a(n) ____________ is a substance that, when mixed with water,
produces the positively charged ____________ _______. This charged particle is hydrated by a water
molecule, producing a(n) _____________ _______. The equilibrium constant for the formation of
charged particles by an acid is called a(n) ___________ ___________ of the acid. According to the
_________ __________ ____________, an acid is a(n) _________ __________ and a base is a(n)
__________ __________. A substance that can act as either is called a(n) ____________
_____________.
An acid-base pair in which the acid and base are on opposite sides of an equation and are
related by the transfer of a proton is called a(n) ____________ ______. A strong acid has a(n) ______
___________ _______, and a weak acid has a(n) _______ _____________ _________.
page 14
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Salts of weak acids or weak bases can react with water in a process called
__________________. Water molecules can react with one another to produce charged particles in a
process called _________– _____________. The quantity Kw, which is the ______–_____________ for
water, gives information on the concentration of these particles. The negative __________________ of
the hydrogen-ion concentration is called the __________. The value of this quantity is greater than 7 in
a(n) ________ ___________. Its value equals 7 in a(n) _________ _____________, and is less than 7 in
a(n) _________ _____________.
A(n) ______________ is a mixture of a _________ acid and a _________ or a _________ base
and a _________ that causes a solution to resist changes in its hydrogen-ion concentration. A(n)
________________ is a substance that changes color over a narrow range of hydrogen-ion
concentrations.
Hydrogen ions combine with hydroxide ions during a reaction called ________–_________
_____________. A laboratory procedure that makes use of this reaction is called a(n) _______–
________ ________________. This procedure makes use of a solution of known concentration, called
a(n) ___________ ___________. When enough of this solution has been added to react completely
with the solution of unknown concentration, the _______________ _________ has been reached.
Acid/Base - Challenge Problems
1. What is the effect of dissolving potassium sulfite in a 0.100 M solution of sulfuric acid? Would you
expect the acidity to increase or decrease? Describe a mechanism that explains your answer.
–38
2. What is the pH of a saturated solution Iron(III) hydroxide? Ksp = 3.98 x 10
page 15
.
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
–5
3. What is the pH of a 0.0100 M solution of Acetic Acid? Ka = 1.75 x 10 .
–7
4. What is the pH of a 0.150 M solution of the base diammine? Kb = 8.71 x 10
page 16
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
–5
–
5. What is the pH of a 0.650 M solution of Phosphoric Acid? Ka(H3PO4) = 7.08 x 10 . Ka(H2PO4 ) =
–10
6.31 x 10
2–
–15
. Ka(HPO4 ) = 4.17 x 10
.
6. You are titrating a 50.0 mL sample of hydrochloric acid with 0.250 M potassium hydroxide. After
you have already added 42.3 mL of the potassium hydroxide you realize that you forgot to add the
phenolphthalein indicator. When you add the indicator, the solution turns bright pink indicating that
you have already missed the end point. You decide to “back-titrate” by adding 0.100 M nitric acid.
The solution turns colorless after an addition of 10.1 mL of the nitric acid. What is the concentration
of the original solution of hydrochloric acid.
page 17
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
7. What is the final pH of a solution that is made with acetic acid and of Copper(II) hydroxide in
1000.0 mL of solution in each of the following two situations.
–5
–20
Ka acetic acid = 1.75 x 10
Ksp Copper(II) hydroxide = 2.19 x 10
a. 50.000 g of each solid
b. 75.000 g of acid and 25.000 g base
page 18
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
Acid-Base Crossword
ACROSS
DOWN
1. Number for which a given logarithm stands
2. Analytical method involving neutralization
3. One more oxygen
3. Acid that can donate more than one proton
6. Hydroxide ion formula
4. Describes a solution for which pH = 7
7. Scale for ranking hydronium ion concentrations
5. Naturally occurring acid in ants
8. Taste of bases
7. Commonly used indicator
9. Hydrated proton
8. Symbol for element 5
11 Hydrochloric acid formula
13. Describes an acid containing one reacting
hydrogen atom.
23
14. Contains 6.023 x 10
particles
9. Ion released by many bases
10. Loss of electrons
12. Common name for calcium oxide
16. Describes a strongly irritating basic
substance
15. Weak acid or base whose color depends on
hydronium ion concentration
18. A scientist who proposed an acid-base
theory
17. Sodium hydroxide formula
19. Has formula NH3
18. Symbol for element 18
20. Acid with formula HC2H3O2
21. Describes species that are related by a
difference in protons
22. Acid with formula HNO3
23. Mineral containing metal
24. Acid found in fruits
25. Scientist who created electron dot structures
26. Has pH less than 7
27. Charged atom
28. Symbol for element 16
page 19
ChemIAcc-19Acids,Bases,Salts WS
Dr. Corell - Chemistry I Accelerated
4
3
1
2
5
6
7
8
9
11
10
12
17
13
18
14
15
16
19
20
21
22
23
25
27
24
26
page 20
28