17. Acid and Base Equilibrium

Ionic Salts

Acidic, Basic, and Neutral Salts - Ionic Compounds

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. 
(b) Fe(OH)3

16.5 Acidity and Basicity of Salts

Predict whether aqueous solutions of the following substances
are acidic, basic, or neutral: (a) AlCl3

Determine the pH of a 0.55 M NaCN solution. The Ka of hydrocyanic acid, HCN, is 4.9 x 10-10.

Predict whether aqueous solutions of the following substances
are acidic, basic, or neutral: (e) Na2SO3.

An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 
mol of the salt is dissolved in water to form 0.500 L of solution, 
the pH of the solution is 8.08. What is the identity of the salt?

Determine if each compound is more soluble in acidic solution
than it is in pure water. Explain.
c. AgCl

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. 
(a) AgBr

Determine whether each cation is acidic or pH-neutral. For
those cations that are acidic, write an equation that shows how
the cation acts as an acid.
d. CH2NH3+

To determine if an anion is basic or neutral you must add an H+ to it. If adding an H+ creates a weak acid then your negative ion is basic, but if adding an H+ creates a strong acid then your negative ion is neutral.&#160;

Determine whether each cation is acidic or pH-neutral. For
those cations that are acidic, write an equation that shows how
the cation acts as an acid.
b. Na+

An unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 
0.100 M solution of the salt is neutral, what is the identity of 
the salt?

Anions (negative ions) can create either basic or neutral solutions.&#160;

Determine whether each cation is acidic or pH-neutral. For
those cations that are acidic, write an equation that shows how
the cation acts as an acid.
c. Co3+

If the main group metal within an ionic compound has a charge of +3 or higher then it creates an acidic solution. If it&#8217;s less than +3 then it creates a neutral solution and is classified as a non-significant ion.&#160;

Determine if each of the following compounds will create an acidic, basic or neutral solution.a) LiC2H3O2&nbsp; &nbsp;b) C6H5NH3Br

Predict whether aqueous solutions of the following substances
are acidic, basic, or neutral: (b) NaBr

(b) If a limestone sculp- ture were treated to form a surface layer of calcium sul- fate, would this help to slow down the effects of acid rain? Explain.

Predict whether aqueous solutions of the following compounds
are acidic, basic, or neutral: (c) Na2CO3

Amines are compounds with only nitrogen or hydrogen (i,e. NH3) or with carbon, nitrogen and hydrogen (i,e. CH3NH2). Positive amines within compounds create acidic solutions.&#160;

The hydrated cation M1H2O26 
3 + has Ka = 10-4, and the 
acid HA has Ka = 10-5. Identify the principal reaction in 
an aqueous solution of each of the following salts, and classify 
each solution as acidic, basic, or neutral. 
(a) NaA

Determine whether each cation is acidic or pH-neutral. For each
cation that is acidic, write an equation that shows how the cation
acts as an acid.
d. Li+

Determine if each of the following compounds will create an acidic, basic or neutral solution.a) Co(HSO4)2&nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp;b) Sr(HSO3)2

Determine if each salt will form a solution that is acidic, basic,
or pH-neutral.
a. Al(NO3)3

Arrange the solutions in order of increasing acidity. 
NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH

Determine whether each cation is acidic or pH-neutral. For
those cations that are acidic, write an equation that shows how
the cation acts as an acid.
a. NH4+

Determine if each of the following compounds will create an acidic, basic or neutral solution.a. C3H7NH3F

Acid–base properties of salts | Acids and bases | AP Chemistry | Khan Academy

Salt Solutions

pH of salt solutions | Acids and bases | Chemistry | Khan Academy

Classify each of the following salt solutions as neutral, 
acidic, or basic. See Appendix C for values of equilibrium 
constants. 
(a) Fe1NO323

How to Determine if Salt is Acidic, Basic, or Neutral Example, Problem, Shortcut, Explained Question

When an acid and base undergo a neutralization reaction they form ions, which can create acidic, basic or neutral solutions.&#160;

Classify each of the following ions according to whether they 
react with water to give a neutral, acidic, or basic solution. 
(a) F-

If the transition metal within an ionic compound has a charge of +2 or higher then it creates an acidic solution. If it&#8217;s less than +2 then it creates a neutral solution and is classified as a non-significant ion.&#160;

Determine whether each anion is basic or neutral. For those anions
that are basic, write an equation that shows how the anion
acts as a base.
c. NO3-

Write a balanced net ionic equation for the principal reaction 
in solutions of each of the following salts. In each case, 
identify the Brønsted–Lowry acids and bases and the conjugate 
acid–base pairs. 
(a) Na2CO3

Calculate Ka for the cation and Kb for the anion in an aqueous 
NH4CN solution. Is the solution acidic, basic, or neutral?

Determine if each salt will form a solution that is acidic, basic,
or pH-neutral.
e. C6H5NH3NO2

Predict whether aqueous solutions of the following substances
are acidic, basic, or neutral: (c) NaClO

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. (c) NaClO4

Predict whether aqueous solutions of the following substances
are acidic, basic, or neutral: (d) 3CH3NH34NO3

Indicate whether each of the following statements is correct or incorrect.
(d) K+ ion is acidic in water because it causes hydrating water molecules to become more acidic.

Cations (positive ions) can create either acidic or neutral solutions.&#160;

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Polyprotic Acid

A&#160;polyprotic acid&#160;possesses more than 2 hydronium ions (H+).&#160;

Diprotic Acid

A diprotic acid&#160;is an acid that can donate two hydronium ions (H+).&#160;

Identifying Acids and Bases

Arrhenius Acid and Base

Bronsted Lowry Acid and Base

Lewis Acid and Base

Amphoteric

pH and pOH

Ka and Kb

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